Ch.3 - Chemical ReactionsSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Jules Bruno

Stoichiometry deals with the numerical relationship between compounds in a balanced chemical reaction by following the Law of Conservation of Mass. This relationship is depicted through the use of coefficients, which tells us the number of moles for each compound. 

Coefficients-Balanced-Reaction-Mole-Map-RatioBalanced Equation

The given equation would mean 3 moles of H2 reacts with 1 mole of N2 to produce 2 moles of NH3.

The Limiting Reactant

Within stoichiometry, the limiting reactant or limiting reagent represents the compound that is totally consumed when a chemical reaction occurs. The maximum amount of product formed from the limiting reactant called the theoretical yield. 

In order to determine the theoretical yield of a reaction you must utilize the stoichiometric chart. 

Stoichiometric-Chart-Avogadro-Number-Mole-to-mole-comparison-conversion-limiting-reactant-reagent-stoichiometryHow to do StoichiometryStoichiometry 

In order to calculate the theoretical yield of a chemical reaction we must deal with stoichiometry and have a balanced equation. 

First, always make sure to check to see if your chemical equation is balanced.  

Unbalanced-Chemical-Equation-Fe-O2-Fe2O3-reaction-combinationFe, O2, Fe2O3 Unbalanced Chemical Equation Now let's take on a typical question dealing with stoichiometry and given quantities for the reactants. 

If 115.0 g Fe reacts with 72.3 g O­2 to produce Fe2O3, what is the amount of product (in grams) formed? 

STEP 1: Balance your chemical equation if needed. 

Balanced-Chemical-Equation-Integers-Fe-O2-Fe2O3Fe, O2, Fe2O3 Balanced Chemical Equation

STEP 2: Find the atomic masses of the elements from the periodic table

Atomic-Masses-Periodic-Table-Fe-O-Iron-OxygenAtomic Masses from Periodic Table

Now find the molar masses of Fe, O­2 and Fe2O3

Molar-Masses-Fe-O2-Fe2O3Molar Masses of Molecular Formulas

STEP 3: Convert the grams of reactants into moles. 

Grams-to-moles-reactantsGrams to moles conversion (Fe and O2 Reactants)

STEP 3: Convert the moles of reactants by doing mole-to-mole comparisons. 

Balanced-Chemical-Equation-4-Fe-3-O2-2-Fe2O3Balanced Chemical Equation (Fe, O2, Fe2O3)

During this step we use the coefficients from the balanced equation. 

Mole-mole-comparisons-conversionsMole to Mole comparisons (O2 to Fe2O3)

STEP 4: Convert the moles of product into grams of product. 

Moles-to-grams-conversionMoles to grams conversion (Fe2O3 product)

STEP 5: Determine the theoretical yield. 

The theoretical yield, sometimes referred to as the 100% yield, represents the smaller amount. The theoretical yield is 165 g Fe2O3

STEP 5: Determine the limiting reactant and the excess reactant. 

The limiting reactant is the compound that gives the smaller amount of product, while the excess reactant is the compound that gives the larger amount of product. Therefore Fe is the limiting reactant and O­2 is the excess reactant. 

Beyond Stoichiometry

Stoichiometry is one of the most fundamental calculations you’ll do in chemistry. It shares connection with other concepts such as mass conversionsempirical formulapercent yieldmolarity and solution chemistry


Jules Bruno

Jules felt a void in his life after his English degree from Duke, so he started tutoring in 2007 and got a B.S. in Chemistry from FIU. He’s exceptionally skilled at making concepts dead simple and helping students in covalent bonds of knowledge.


Additional Problems
Photosynthesis occurs by the following chemical reaction. If a plant consumes 28.9 g of CO2 in one week, what mass of glucose (g) can the plant produce? Molar mass: CO2 = 44.01 g/mol; C6H12O6 = 180.2 g/mol 6CO2(g) + 6H2O → 6O2(g) + C6H12O6(aq) A. 42.3 g B. 19.7 g C. 118 g D. 60.5 g
Aqueous solutions of sodium hypochlorite (NaOCl), also known as household bleach, are prepared by reaction of sodium hydroxide with chlorine:                 2 NaOH (aq) + Cl 2 (g)  →  NaOCl (aq) + NaCl (aq) + H 2O (l)   The grams of NaOH needed to react with 25.0 g of Cl 2 are:             35.2 g 55.0g 28.2 g 45.3 g 22.7 g
When 1 mole of glucose (C6H12O6) is completely burned into CO2, how many moles of H2O are produced? The unbalanced equation for this reaction is as follows: C6H12O6 + O2 → CO2 + H2O   a. 1 b. 2 c. 3 d. 6 e. 12
Diborane, B2H6, can be prepared according to the following equation: 3 NaBH4 (aq) + 4 BF3 → 3 NaBF4 (aq) + 2 B2H 6 If 10.5 moles of NaBF4 are produced in this reaction, how many hydrogen atoms in B 2H6 are also produced? A. 1.58 x 1024 B. 5.69 x 1025 C. 2.03 x 1023 D. 2.53 x 1025
What is the minimum grams of air needed for the complete combustion of 8.00 g of heptane (C7H16)? Air is 21% O2 by mass.   a) 28 b) 5.9 c) 130 d) 65 e) 18
Calculate the total number of grams of ammonia, NH 3, required to produce 566.0 g of Cu(NH3)4SO4 using the balanced reaction given below. CuSO4 + 4NH3 ➞ Cu(NH3)4SO4 M.W. of NH3 = 17.03 M.W. of Cu(NH3)4SO4 = 227.76            
How many moles of oxygen are formed when 58.6 g of KNO 3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol. 4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g) A. 0.290 mol O2 B. 0.580 mol O2 C. 18.5 mol O2 D. 0.724 mol O2 E. 1.73 mol O2
Hydrogen peroxide (H2O2) decomposes into water and oxygen gas. How many moles of oxygen gas are formed from the decomposition of 3 moles of hydrogen peroxide? 1. 1 2. 1.5 3. 3 4. 6 5. 2 6. 0
Potassium reacts with chlorine gas to produce potassium chloride. How many moles of K will react with 0.40 moles of Cl2? a. 0.20 mol b. 0.32 mol c. 0.80 mol d. 0.60 mol e. 0.40 mol  
Taxol is a remarkable new weapon in the war against cancer. Isolated from the bark of the Pacific Yew, it has been shown to be highly effective against refractive ovarian and breast cancers. Due to the extremely low concentrations of it found in nature, a great deal of effort has gone into alternative ways of obtaining it. The Taxol nucleus has the molecular formula C32H40O11. If a 115 mg sample of Taxol were subjected to combustion, calculate both the amount of carbon dioxide and water (in mg) expected. 
How many moles of NH 3 are needed to react completely with 30.0 mol of F 2? 2 NH3 + 5 F2 → N2F4 + 6 HF (A) 2 mol (B) 12 mol (C) 5 mol (D) 30 mol (E) 75 mol
Calculate the mass of hydrogen and the mass of oxygen required to make 250 L of water assuming the reaction goes to completion (i.e. 100% yield). The molar mass of water is 18.013 g/mol. 2 H2 (g) + O2 (g)      →       2 H 2O (/)
How many grams of oxygen are formed when 6.21 moles of KOH are formed?  4 KO (s) + 2 H2O (l) → 4 KOH (s) + O2 (g) A) 11.7 g O2 B) 27.9 g O2 C) 3.59 g O2 D) 19.9 g O2 E) 49.7 g O2
A self-contained breathing apparatus uses potassium superoxide, KO2, to  convert the carbon dioxide and water in exhaled air into oxygen, as shown by this equation. 4 KO2 (s) + 4 CO2 (g) + 2 H2O (g) → 4 KHCO3 (s) + 3 O2 (g) How many molecules of oxygen gas will be produced from the 0.0468 g of carbon dioxide that is exhaled in a typical breath? a) 4.8 x 1020 b) 6.4 x 1020 c) 8.5 x 1020 d) 1.9 x 1021
How many grams of nitrogen gas are formed when 58.6 g of KNO  3 decomposes according to the following reaction? (Molar masses: KNO3 = 101.11 g/mol, N2 = 28.02 g/mol) 4 KNO3(s)  →  2 K2O(s) + 2 N2(g)  + 5 O 2(g) A. 8.12 g B. 16.3 g C. 20.3 g D. 48.5 g E. 518. g
A mixture containing 9 mol of F2, and 4 mol of S is allowed to react. This equation represent the reaction that takes place. 3F2 + S → SF6 How many of F2, remain after 3 mol of S have reacted? a) 4 b) 3 c) 1 d) 0
How many moles of iron react with 1.75 mol of oxygen gas? The equation  for the reaction is: 3 O2 (g) + 4 Fe (s) → 2 Fe2O3 (s) a) 1.31 mol b) 1.75 mol c) 2.33 mol d) 5.25 mol
Sulfuric acid dissolves aluminum metal according to the reaction: 2 Al (s) + 3 H2SO4 (aq)      →       Al 2(SO4)3 (aq) + 3 H2 (g) Suppose you want to dissolve an aluminum block with a mass of 15.2 g. a) What minimum mass of H 2SO4 (in grams) do you need?                   b) What mass of H 2 gas (in grams) does the complete reaction of the aluminum block produce? 
For the following acid-base reaction, calculate the mass (in grams) of the acid necessary to completely react with and neutralize 4.85 g of the base. 2 HNO3 (aq) + Ca(OH)2 (aq)      →       2 H 2O (l) + Ca(NO3)2 (aq)
What is reaction stoichiometry?
Toilet bowl cleaners often contain hydrochloric acid to dissolve the calcium carbonate deposits that accumulate within a toilet bowl.What mass of calcium carbonate (in grams) can be dissolved by 3.9 g of HCl? (Hint: Begin by writing a balanced equation for the reaction between hydrochloric acid and calcium carbonate.)
The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8 H18 ) and calculate the mass (in kg) of carbon dioxide that is added to the atmosphere per 2.1 kg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)
Many home barbeques are fueled with propane gas (C3 H8 ). What mass of carbon dioxide (in kg) is produced upon the complete combustion of 18.9 L of propane (approximate contents of one 5-gallon tank)? Assume that the density of the liquid propane in the tank is 0.621 g/mL. (Hint: Begin by writing a balanced equation for the combustion reaction.)
The decomposition of ZnCO3(s) into ZnO(s) and CO2(g) at constant pressure requires the addition of 71.5 kJ of heat per mole of ZnCO3. You may want to reference (Pages 177 - 178) Section 5.4 while completing this problem.Write a balanced equation for the reaction.
If 1.5 mol of each of the following compounds is completely combusted in oxygen, which one will produce the largest number of moles of H2O? C2H5OH, C3H8, CH3CH2COCH3.
The fat stored in the hump of a camel is a source of both energy and water.Calculate the mass of H2O produced by metabolism of 2.2 kg of fat, assuming the fat consists entirely of tristearin (C57H110O6), a typical animal fat, and assuming that during metabolism, tristearin reacts with O2 to form only CO2 and H2O.
A mixture of N2 (g) and H2 (g) reacts in a closed container to form ammonia, NH3 (g). The reaction ceases before either reactant has been totally consumed. At this stage 2.6 mol N2, 2.6 mol H2, and 2.6 mol NH3 are present.How many moles of N2 and H2 were present originally?
The reaction of NH3 and O2 forms NO and water. The NO can be used to convert P4 to P4O6, forming N2 in the process. The P4O6 can be treated with water to form H3PO3, which forms PH3 and H3PO4 when heated.Find the mass of PH3 that forms from the reaction of 1.55 g NH3.
An important reaction that takes place in a blast furnace during the production of iron is the formation of iron metal and CO2 from Fe2O3 and CO.Find the mass of Fe2O3 required to form 910 kg of iron.
A liquid fuel mixture contains 30.05 % hexane (C6H14), 16.05 % heptane (C7H16), and the rest octane (C8H18).What maximum mass of carbon dioxide is produced by the complete combustion of 13.0 kg of this fuel mixture?
A mixture of C3H8 and C2H2 has a mass of 2.6 g . It is burned in excess O2 to form a mixture of water and carbon dioxide that contains 1.6 times as many moles of CO2 as of water.Find the mass of C2H2 in the original mixture.
If an automobile travels 230 mi with a gas mileage of 21.5 mi/gal , how many kilograms of CO2 are produced? Assume that the gasoline is composed of octane, C8H18 (l), whose density is 0.69 g/mL.
A particular coal contains 2.5% sulfur by mass. When this coal is burned, the sulfur is converted into sulfur dioxide gas. The sulfur dioxide reacts with solid calcium oxide to form solid calcium sulfite.If the coal is burned in a power plant that uses 2100 tons of coal per day, what mass of calcium oxide is required daily to eliminate the sulfur dioxide?
The source of oxygen that drives the internal combustion engine in an automobile is air. Air is a mixture of gases, which are principally N2 (~79%) and O2 (~20%). In the cylinder of an automobile engine, nitrogen can react with oxygen to produce nitric oxide gas, NO. As NO is emitted from the tailpipe of the car, it can react with more oxygen to produce nitrogen dioxide gas.The production of NOx gases is an unwanted side reaction of the main engine combustion process that turns octane, C8H18, into CO2 and water. If 85% of the oxygen in an engine is used to combust octane, and the remainder used to produce nitrogen dioxide, calculate how many grams of nitrogen dioxide would be produced during the combustion of 600 grams of octane.
A particular coal contains 2.55% sulfur by mass. When the coal is burned, it produces SO2 emissions which combine with rainwater to produce sulfuric acid.Determine how much sulfuric acid (in metric tons) is produced by the combustion of 1.2 metric ton of this coal. (A metric ton is 1000 kg.)
A mixture of carbon and sulfur has a mass of 9.0 g. Complete combustion with excess O2 gives 24.6 g of a mixture of CO2 and SO2.Find the mass of sulfur in the original mixture.
One of the best-selling light, or low-calorie, beers is 4.4 % alcohol by volume and a 12-oz serving contains 110 Calories; remember: 1 Calorie = 1000 cal = 1 kcal. To estimate the percentage of Calories that comes from the alcohol, consider the following questions. Write a balanced chemical equation for the reaction of ethanol, C2H5OH, with oxygen to make carbon dioxide and water.
Burning methane in oxygen can produce three different carbon-containing products: soot (very fine particles of graphite), CO(g), and CO2(g).Write balanced equation for the reaction of methane gas with oxygen to produce soot. Assume that H2O(l) is the only other product.
Burning methane in oxygen can produce three different carbon-containing products: soot (very fine particles of graphite), CO(g), and CO2(g).Write balanced equation for the reaction of methane gas with oxygen to produce CO(g). Assume that H2O(l) is the only other product.
Burning methane in oxygen can produce three different carbon-containing products: soot (very fine particles of graphite), CO(g), and CO2(g).Write balanced equation for the reaction of methane gas with oxygen to produce CO2(g). Assume that H2O(l) is the only other product.
People sometimes use sodium bicarbonate as an antacid to neutralize excess hydrochloric acid in an upset stomach.What mass of hydrochloric acid (in grams) can 2.5 g of sodium bicarbonate neutralize? (Hint: Begin by writing a balanced equation for the reaction between aqueous sodium bicarbonate and aqueous hydrochloric acid.)
The diagram represents a high-temperature reaction between CH4 and H2O.Based on this reaction, find how many moles of CO can be obtained starting with 6 mol CH4?
The diagram represents a high-temperature reaction between CH4 and H2O.Based on this reaction, how many moles of H2 can be obtained starting with 6 mol CH4?
Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide.How many grams of aluminum hydroxide are obtained from 16.2 g of aluminum sulfide?
Calcium hydride reacts with water to form calcium hydroxide (aqueous) and hydrogen gas.How many grams of calcium hydride are needed to form 4.750 g of hydrogen gas?
When 1.57 mol O2 reacts with H2 to form H2O, how many moles of H2 are consumed in the process?
You may want to reference (Pages 102 - 105)Section 3.6 while completing this problem.Propane, C3H8, is a common fuel used for cooking and home heating. What mass of O2 is consumed in the combustion of 1.00 g of propane?
Gasoline is composed primarily of hydrocarbons, including many with eight carbon atoms, called octanes. One of the cleanest-burning octanes is a compound called 2,3,4-trimethylpentane, which has the structural formula shown in the figure . The complete combustion of one mole of this compound to CO2 (g) and H2O(g) leads to HH = -5064.9 { m kJ/mol}.Write a balanced equation for the combustion of 1 mol of C8H18 (l).
Diethyl ether, C4H10O (l), a flammable compound that has long been used as a surgical anesthetic, has the structure CH3 - CH2 - O - CH2 - CH3 The complete combustion of 1 mol of C4H10O (l) to CO2 (g) and H2O (l) yields Ho= -2723.7 kJ.Write a balanced equation for the combustion of 1 mol of C4H10O (l).
Consider the following unbalanced equation for the combustion of hexane:αC6H14(g) + βO2(g) → γCO2(g) + δH2O(g)a. Balance the equation.b. Determine how many moles of O2 are required to react completely with 5.2 moles C6H14
In a chemical reaction, exactly 2 mol of substance A react to produce exactly 3 mol of substance B. 2A → 3BHow many molecules of substance B are produced when 26.8 g of substance A reacts? The molar mass of substance A is 16.7 g/mol.
When heated, KClO3 decomposes into KCl and O2. 2KClO3 → 2KCl + 3O2 If this reaction produced 50.6 g of KCl, how much O2 was produced (in grams)?
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH 3, according to the equation 3H2 (g) + N2 (g) → 2NH3 (g) How many molecules (not moles) of  NH3 are produced from 3.76×10−4 g of H2?
The compound P4S3 is used in matches. It reacts with oxygen to produce P4O10 and SO2. The unbalanced equation is shown below. P4S3(s) + O2(g) → P4O10(s) + SO2(g) What mass of SO2 is produced from the combustion of 0.331 g P4S3 ?
Molecular hydrogen is used as the “liquid fuel” (liquefied hydrogen) for rockets. How much water is generated from 1000 gallons of liquefied hydrogen? (1 gallon = 3.80 L. The density of liquefied hydrogen at 20 K is 71 g/L.) a. 4860 kgb. 2430 kgc. 1220 kgd. 135 kge. 17 kg
What mass of oxygen is needed for the complete combustion of 155 mL of C6H6 (molar mass = 78.1 g/mol) to produce carbon dioxide and water? Density of C 6H6 = 0.88 g/mL.2 C6H6 (l)   +   15 O 2 (g)   →   12 CO 2 (g)   +   6 H 2O (l) A. 55.9 g          B. 419 g          C. 240 gD. 330 g          E. 476 g
Using the following equation for the combustion of octane, calculate the amount of moles of carbon dioxide formed from 100.0 g of octane. The molar mass of octane is 114.22 g/mol. The molar mass of carbon dioxide is 44.01 g/mol.a. 6.997 molesb. 8.000 molesc. 10.93 molesd. 18.18 molese. 14.00 moles
A 1.42-g sample of a pure compound, with formula M2SO4, was dissolved in water and treated with an excess of aqueous calcium chloride, resulting in the precipitation of all the sulfate ions as calcium sulfate. The precipitate was collected, dried, and found to weigh 1.36 g. Determine the atomic mass of M, and identify M.
When heated, KClO3 decomposes into KCl and O2.2KClO3 → 2KCl +3O2 If this reaction produced 42.0 g of KCl, how much O 2 was produced (in grams)?
In the chemical reaction N2 + 3 Mg → Mg 3N2 if you begin with 1.35 moles of Mg, how many moles of N2 are required to react all of the Mg?A. 0.45              B. 1.01          C. 1.35            D. 1.80            E. 4.05 
A 1.00-g sample of an alkaline earth metal chloride is treated with excess silver nitrate. All of the chloride is recovered as 1.38 g of silver chloride. Identify the metal.
Consider the reaction of hydrogen gas (H2) and oxygen gas (O2) to form water. How many molecules of water will be made by the reaction of 12.0 g of O2 gas?(A) 1.13 x 1023 molecules(B) 2.26 x 1023 molecules(C) 4.52 x 1023 molecules(D) 2.26 x 1024 molecules(E) 4.52 x 1024 molecules
How many moles of H3PO4 are produced when 36.5 g of HCl are produced by the reaction PCl5 + H2O → H3PO4 + HCl?(A) 0.2 mol H3PO4(B) 0.5 mol H3PO4(C) 1 mol H3PO4(D) 2 mol H3PO4(E) 5 mol H3PO4
Consider the following balanced equation for the neutralization of acetic acid. 2HC2H3O2(aq) + Ca(OH)2(aq) → 2H2O(l) + Ca(C2H3O2)2(aq) Determine how many moles of Ca(OH)2 are required to completely neutralize 8.67 mol of HC2H3O2.
Barium hydroxide (used in corrosion inhibitors and lubricants) reacts with chloric acid (HClO3) to form barium chlorate [Ba(ClO3)2] and water. What mass of water is formed when 138 g of barium hydroxide reacts with chloric acid?(A) 32.5 g(B) 29.0 g(C) 16.2 g(D) 7.31 g(E) 138 g
Use this chart when given a chemical equation with the  KNOWN quantity of a compound or element and asked to find the UNKNOWN quantity of another compound or element. 
Lead(II) sulfide (PbS) was once used in glazing earthenware. It will also react with hydrogen peroxide (H2O2) to form lead(II) sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide?(A) 151 g(B) 123 g(C) 37.7 g(D) 9.41 g(E) 265 g
Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide.a. Write a balanced equation for this reaction.b. How many grams of aluminum hydroxide can be obtained from 10.5 g of aluminum sulfide?
Copper(II) nitrate decomposes upon heating to form copper(II) oxide, nitrogen dioxide gas, and oxygen gas. If 1.0 mole of copper(II) nitrate decomposes, how many moles of nitrogen dioxide would be formed? a) 0.50 mol b) 4.0 mol c) 1.0 mol d) 2.0 mol e) 6.0 mol  
How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl3. 2 ICl3 + 3 H2O → ICl + HIO 3 + 5 HCl A) 6.09 ×1025 molecules HCl B) 3.65 ×1024 molecules HCl C) 2.78 ×1024 molecules HCl D) 5.02 ×1025 molecules HCl E) 1.67 ×1024 molecules HCl
BaCl2 (aq) + AgNO3 (aq) → AgCl(s) + Ba(NO 3)2 (aq)a. Write the balanced equation.b. What mass AgNO3, in grams, is required for complete reaction with 0.156g of BaCl 2? What mass of AgCl is produced?
How many moles of NH3 can be produced from 15.0 mol of H2 and excess N2? Express your answer numerically in moles. 
A 2.000 g sample of an unknown metal, M, was completely burned in excess O 2 to yield 0.02224 mol of the metal oxide, M2O3. What is the metal? a) Y b) Ca c) Al d) Se
How many grams of sulfur are required to react with 1.50 moles of copper in the process? 2Cu + S → Cu2S  
Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel rocket motors. The reaction isFe2O3(s) + 2Al(s) → 2Fe(l) + Al2O3(s)What masses of iron(III) oxide and aluminum must be used to produce 15.0 g iron? What is the maximum mass of aluminum oxide that could be produced?
Plants incorporate CO2 from the atmosphere into biologically available carbon during photosynthesis: CO2 + H2O → C6H12O6 + O2  Balance the equation first, then calculate how many molecules of C 6H12O6 are produced from 1.00g of CO2.    
One of relatively few reactions that takes place directly between two solids at room temperature isBa(OH)2 • 8H2O(s) + NH4SCN(s) → Ba(SCN)2(s) + H2O(l) + NH3(g)In this equation, the • 8H2O in Ba(OH) 2 • 8H2O indicates the presence of eight water molecules. This compound is called barium hydroxide octahydrate.b. What mass of ammonium thiocyanate (NH 4SCN) must be used if it is to react completely with 6.5 g barium hydroxide octahydrate?
Bacterial digestion is an economical method of sewage treatment. The reaction below is an intermediate step in the conversion of the nitrogen in organic compounds into nitrate ions. What mass of bacterial tissue is produced in a treatment plant for every 1.0 x 104 kg of wastewater containing 3.0% NH4+ ions by mass? Assume that 95% of the ammonium ions are consumed by the bacteria.
When glucose, C6H12O6, reacts with oxygen it produces carbon dioxide and water. What mass of oxygen (in grams) is required for complete reaction of 75.0 g of glucose? How many grams of water and carbon dioxide form?
Phosphorus can be prepared from calcium phosphate by the following reaction:2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) → 6CaSiO3(s) + P4(s) + 10CO(g)Phosphorite is a mineral that contains Ca 3(PO4)2 plus other non-phosphorus-containing compounds. What is the maximum amount of P4 that can be produced from 1.0 kg of phosphorite if the phorphorite sample is 75% Ca3(PO4)2 by mass? Assume an excess of the other reactants.
Calcium metal reacts with water to form calcium hydroxide and hydrogen gas. How much hydrogen is formed when 0.50 g of calcium are added to water? 1. 0.050 g 2. 0.025 g 3. 0.50 g 4. 0.10 g
You have seven closed containers, each with equal masses of chlorine gas (Cl 2). You add 10.0 g of sodium to the first sample, 20.0 g of sodium to the second sample, and so on (adding 70.0 g of sodium to the seventh sample). Sodium and chlorine react to form sodium chloride according to the equation2 Na (s) + Cl2 (g) → 2 NaCl (s)After each reaction is complete, you collect and measure the amount of sodium chloride formed. A graph of your results is shown below.Calculate the mass of NaCl formed when 20.0 g of sodium is used.
I2 is produced by the reaction of 0.4235 mol of CuCl2 according to the following equation: 2CuCl2 + 4KI ⟶ 2CuI + 4KCl + I 2.(a) How many molecules of  I2 are produced?
I2 is produced by the reaction of 0.4235 mol of CuCl2 according to the following equation: 2CuCl2 + 4KI ⟶ 2CuI + 4KCl + I 2.(b) What mass of  I2 is produced?
Silver is often extracted from ores such as K[Ag(CN)2] and then recovered by the reaction 2K[Ag(CN)2](aq) + Zn(s) ⟶ 2Ag(s) + Zn(CN)2(aq) + 2KCN(aq)(a) How many molecules of Zn(CN)2 are produced by the reaction of 35.27 g of K[Ag(CN) 2]?
A student forgets to weigh a mixture of sodium bromide dihydrate and magnesium bromide hexahydrate. Upon strong heating, the sample loses 252.1 mg of water. The mixture of anhydrous salts reacts with excess AgNO3 solution to form 6.00×10−3 mol of solid AgBr. Find the mass % of each compound in the original mixture.
Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel rocket motors. The reaction isFe2O3 (s) + 2Al (s) → 2 Fe (l) + Al2O3 (s) What masses of iron(III) oxide and aluminum must be used to produce 15.0 g iron? What is the maximum mass of aluminum oxide that could be produced?
What mass of silver oxide, Ag 2O, is required to produce 25.0 g of silver sulfadiazine, AgC10H9N4SO2, from the reaction of silver oxide and sulfadiazine?2C10H10N4SO2 + Ag2O ⟶ 2AgC10H9N4SO2 + H2O
The reusable booster rockets of the U.S. space shuttle employ a mixture of aluminum and ammonium perchlorate for fuel. A possible equation for this reaction is3 Al (s) + 3 NH4ClO4 (s) → Al2O3 (s) + AlCl3 (s) + 3 NO (g) + 6 H2O (g)What mass of NH4ClO4 should be used in the fuel mixture for every kilogram of Al?
One of relatively few reactions that takes place directly between two solids at room temperature isBa(OH)2 • 8 H 2O (s) + NH 4SCN (s) → Ba(SCN) 2 (s) + H 2O (l) + NH 3 (g)In this equation, the • 8 H 2O in Ba(OH) 2 • 8 H2O indicates the presence of eight water molecules. This compound is called barium hydroxide octahydrate.What mass of ammonium thiocyanate (NH4SCN) must be used if it is to react completely with 6.5 g barium hydroxide octahydrate?
Automotive air bags inflate when a sample of sodium azide, NaN3, is very rapidly decomposed.2NaN3(s) ⟶ 2Na(s) + 3N2(g)What mass of sodium azide is required to produce 2.6 ft3 (73.6 L) of nitrogen gas with a density of 1.25 g/L?
Elixirs such as Alka-Seltzer use the reaction of sodium bicarbonate with citric acid in aqueous solution to produce a fizz:3 NaHCO3 (aq) + C6H8O7 (aq) → 3 CO 2 (g) + 3 H2O (l) + Na 3C6H5O7 (aq)What mass of C6H8O7 should be used for every 1.0 x 10 2 mg NaHCO3?
Urea, CO(NH2)2, is manufactured on a large scale for use in producing urea-formaldehyde plastics and as a fertilizer. What is the maximum mass of urea that can be manufactured from the CO2 produced by combustion of 1.00 × 103 kg of carbon followed by the reaction? CO2(g) + 2NH3(g) ⟶ CO(NH2)2(s) + H2O(l)
Aspirin (C9H8O4) is synthesized by reacting salicylic acid (C7H6O3) with acetic anhydride (C4H6O3). The balanced equation isC7H6O3 + C4H6O3 → C9H8O4 + HC2H3O2What mass of acetic anhydride is needed to completely consume 1.00 x 10  2 g salicylic acid?
A particular kind of emergency breathing apparatus-often placed in mines, caves, or other places where oxygen might become depleted or where the air might become poisoned-works via the following chemical reaction:4KO2(s) + 2CO2(g) → 2K2CO3(s) + 3O2(g)Notice that the reaction produces O2, which can be breathed, and absorbs CO2, a product of respiration. Suppose you work for a company interested in producing a self-rescue breathing apparatus (based on the above reaction) which would allow the user to survive for 13 minutes in an emergency situation.Estimate how much KO2 would be required for the apparatus. (Find any necessary additional information. Assume that normal air is 20% oxygen and human breathing rate is about 8 Lair/min. Assume that 4% of the air would need to be replenished with oxygen..)
Hydrolysis of the compound B5H9 forms boric acid, H3BO3. Fusion of boric acid with sodium oxide forms a borate salt, Na2B4O7.Without writing complete equations, find the mass (in grams) of B5H9 required to form 152 g of the borate salt by this reaction sequence.
In 1997 and 2009, at United Nations conferences on climate change, many nations agreed to expand their research efforts to develop renewable sources of carbon-based fuels. For more than a quarter century, Brazil has been engaged in a program to replace gasoline with ethanol derived from the root crop manioc (cassava).What mass (g) of oxygen is required to burn completely 1.00 L of a mixture that is 90.0% gasoline (d = 0.742 g/mL) and 10.0% ethanol (d = 0.789 g/mL) by volume?
Consider the following unbalanced chemical equation for the combustion of pentane (C5H12):C5H12 (l) + O2 (g) → CO2 (g) + H2O (l)If 20.4 g of pentane are burned in excess oxygen, what mass of water can be produced, assuming 100% yield?
Manganese(IV) oxide reacts with aluminum to form elemental manganese and aluminum oxide:3 MnO2 + 4Al → 3 Mn + 2 Al2O3You may want to reference (Page 142) Section 4.2 while completing this problem.What mass of Al is required to completely react with 25.0 g MnO2?
In a car engine, gasoline (represented by C8H18) does not burn completely, and some CO, a toxic pollutant, forms along with CO2 and H2O. If 5.0% of the gasoline forms CO:What is the ratio of CO2 to CO molecules in the exhaust?
Gaseous dichlorine monoxide decomposes readily to chlorine (green) and oxygen (red) gases.(c) If each oxygen atom represents 0.050 mol, how many molecules of dichlorine monoxide were present before the decomposition?
In a car engine, gasoline (represented by C8H18) does not burn completely, and some CO, a toxic pollutant, forms along with CO2 and H2O. If 5.0% of the gasoline forms CO:What is the mass ratio of CO2 to CO?
In a car engine, gasoline (represented by C8H18) does not burn completely, and some CO, a toxic pollutant, forms along with CO2 and H2O. If 5.0% of the gasoline forms CO:What percentage of the gasoline must form CO for the mass ratio of CO2 to CO to be exactly 1/1?
Butane gas is compressed and used as a liquid fuel in disposable cigarette lighters and lightweight camping stoves. Suppose a lighter contains 5.50 mL of butane (d = 0.579 g/mL).(a) How many grams of oxygen are needed to burn the butane completely?
Butane gas is compressed and used as a liquid fuel in disposable cigarette lighters and lightweight camping stoves. Suppose a lighter contains 5.50 mL of butane (d = 0.579 g/mL).(b) How many moles of H2O form when all the butane burns?
Butane gas is compressed and used as a liquid fuel in disposable cigarette lighters and lightweight camping stoves. Suppose a lighter contains 5.50 mL of butane (d = 0.579 g/mL).(c) How many total molecules of gas form when the butane burns completely?
Reactants A and B form product C. Draw a road map and write a Plan to find the mass (g) of C when 25 g of A reacts with excess B.
Reactants D and E form product F. Draw a road map and write a Plan to find the mass (g) of F when 27 g of D reacts with 31 g of E.
Chlorine gas can be made in the laboratory by the reaction of hydrochloric acid and manganese(IV) oxide: 4HCl(aq) + MnO2(s) ⟶MnCl2(aq) + 2H2O(g) + Cl2(g) When 1.82 mol of HCl reacts with excess MnO2, how many moles of Cl 2 form?
Chlorine gas can be made in the laboratory by the reaction of hydrochloric acid and manganese(IV) oxide: 4HCl(aq) + MnO2(s) ⟶MnCl2(aq) + 2H2O(g) + Cl2(g) When 1.82 mol of HCl reacts with excess MnO2, how many grams of Cl 2 form?
Bismuth oxide reacts with carbon to form bismuth metal: Bi 2O3(s) + 3C( ) ⟶2Bi(s) + 3CO(g) When 0.607 mol of Bi2O3 reacts with excess carbon, how many moles of Bi form?
The toxic pigment called white lead, Pb3(OH)2(CO3)2, has been replaced in white paints by rutile, TiO2. How much rutile (g) can be prepared from 379 g of an ore that contains 88.3% ilmenite (FeTiO3) by mass?2FeTiO3 + 4HCl + Cl2 ⟶ 2FeCl3 + 2TiO2 + 2H2O
Bismuth oxide reacts with carbon to form bismuth metal: Bi 2O3(s) + 3C( ) ⟶2Bi(s) + 3CO(g) When 0.607 mol of Bi2O3 reacts with excess carbon, how many grams of CO form?
Potassium nitrate decomposes on heating, producing potassium oxide and gaseous nitrogen and oxygen: 4KNO3(s) ⟶2K2O(s) + 2N2(g) + 5O2(g) To produce 56.6 kg of oxygen, how many moles of KNO3 must be heated?
Potassium nitrate decomposes on heating, producing potassium oxide and gaseous nitrogen and oxygen: 4KNO3(s) ⟶2K2O(s) + 2N2(g) + 5O2(g) To produce 56.6 kg of oxygen, how many grams of KNO3 must be heated?
Chromium(III) oxide reacts with hydrogen sulfide (H2S) gas to form chromium(III) sulfide and water: Cr2O3(s) + 3H2S(g) ⟶Cr2S3(s) + 3H2O(l) To produce 421 g of Cr2S3, how many moles of Cr2O3 are required?
Chromium(III) oxide reacts with hydrogen sulfide (H2S) gas to form chromium(III) sulfide and water: Cr2O3(s) + 3H2S(g) ⟶Cr2S3(s) + 3H2O(l) To produce 421 g of Cr2S3, how many grams of Cr2O3 are required?
Calculate the mass (g) of each product formed when 43.82 g of diborane (B 2H6) reacts with excess water: B2H6(g) + H2O(l) ⟶H3BO3(s) + H2(g) [unbalanced]
Consider the balanced equation:SiO2(s) + 3C(s) → SiC(s) + 2CO(g)Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.Mol SiO2Mol CMol SiCMol CO3____________________9_________________________162.8____________________2.45__________Complete the first row.
Consider the balanced equation:SiO2(s) + 3C(s) → SiC(s) + 2CO(g)Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.Mol SiO2Mol CMol SiCMol CO3____________________9_________________________162.8____________________2.45__________Complete the second row.
Consider the balanced equation:SiO2(s) + 3C(s) → SiC(s) + 2CO(g)Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.Mol SiO2Mol CMol SiCMol CO3____________________9_________________________162.8____________________2.45__________Complete the third row.
Consider the balanced equation:SiO2(s) + 3C(s) → SiC(s) + 2CO(g)Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.Mol SiO2Mol CMol SiCMol CO3____________________9_________________________162.8____________________2.45__________Complite the fourth row.
Consider the balanced equation:SiO2(s) + 3C(s) → SiC(s) + 2CO(g)Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.Mol SiO2Mol CMol SiCMol CO3____________________9_________________________162.8____________________2.45__________Complite the fifth row.
Consider the following balanced equation:2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g)Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.Mol N2H4Mol N2O4Mol N2Mol H2O4____________________8_________________________184.5____________________4.5___________________13.6_____Complete the first row.
Consider the following balanced equation:2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g)Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.Mol N2H4Mol N2O4Mol N2Mol H2O4____________________8_________________________184.5____________________4.5___________________13.6_____Complete the second row.
Consider the following balanced equation:2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g)Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.Mol N2H4Mol N2O4Mol N2Mol H2O4____________________8_________________________184.5____________________4.5___________________13.6_____Complete the third row.
Consider the following balanced equation:2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g)Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.Mol N2H4Mol N2O4Mol N2Mol H2O4____________________8_________________________184.5____________________4.5___________________13.6_____Complete the fourth row.
Consider the following balanced equation:2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g)Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.Mol N2H4Mol N2O4Mol N2Mol H2O4____________________8_________________________184.5____________________4.5___________________13.6_____Complete the fifth row.
Consider the following balanced equation:2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g)Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.Mol N2H4Mol N2O4Mol N2Mol H2O4____________________8_________________________184.5____________________4.5___________________13.6_____Complete the sixth row.
An ionic compound forms when lithium (Z = 3) reacts with oxygen (Z = 8). If a sample of the compound contains 8.4×1021 lithium ions, how many oxide ions does it contain?
An ionic compound forms when calcium (Z = 20) reacts with iodine (Z = 53). If a sample of the compound contains 7.4×1021 calcium ions, how many iodide ions does it contain?
Calculate how many moles of NO2 form when each quantity of reactant completely reacts.2N2O5(g) → 4NO2(g) + O2(g)2.6 mol N2O5
Calculate how many moles of NO2 form when each quantity of reactant completely reacts.2N2O5(g) → 4NO2(g) + O2(g)7.0 mol N2O5
Calculate how many moles of NO2 form when each quantity of reactant completely reacts.2N2O5(g) → 4NO2(g) + O2(g)16.2 g N2O5
Calculate how many moles of NO2 form when each quantity of reactant completely reacts.2N2O5(g) → 4NO2(g) + O2(g)3.01 kg N2O5
Methanol, CH3OH, is produced from the reaction of carbon monoxide and hydrogen: CO(g) + 2H2(g) ⟶CH3OH(l)How many moles of methanol can be produced when 4.5 mol of CO reacts with 7.2 mol of H  2?
Hydrobromic acid dissolves solid iron according to the following reaction:Fe(s) + 2HBr(aq) → FeBr2(aq) + H2(g)What mass of HBr (in g) would you need to dissolve a 3.2 -g pure iron bar on a padlock?
In the following reaction, 2.35 mol of NH3 reacts with 2.75 mol of O2; how many moles of water form?4NH3(g) + 5O2(g) ⟶4NO(g) + 6H2O(l)
Many metal react with oxygen gas to form the metal oxide. For example, calcium reacts as follows:2Ca(s) + O2(g) ⟶2CaO(s)You wish to calculate the mass (g) of calcium oxide that can be prepared from 4.20 g of Ca and 2.80 g of O2.(a) What amount (mol) of CaO can be produced from the given mass of Ca?
Many metal react with oxygen gas to form the metal oxide. For example, calcium reacts as follows:2Ca(s) + O2(g) ⟶2CaO(s)You wish to calculate the mass (g) of calcium oxide that can be prepared from 4.20 g of Ca and 2.80 g of O2.(b) What amount (mol) of CaO can be produced from the given mass of O 2?
Lead(II) chromate (PbCrO4) is used as the yellow pigment for marking traffic lanes but is banned from house paint because of the risk of lead poisoning. It is produced from chromite (FeCr2O4), an ore of chromium: 4FeCr2O4(s) + 8K2CO3(aq) + 7O2(g) ⟶ 2Fe2O3(s) + 8K2CrO4(aq) + 8CO2(g) Lead(II) ion then replaces the K + ion. If a yellow paint is to have 0.511% PbCrO 4 by mass, how many grams of chromite are needed per kilogram of paint?
Metal hydrides react with water to form hydrogen gas and the metal hydroxide. For example,SrH2(s) + 2H2O(l) ⟶Sr(OH)2(s) + 2H2(g)You wish to calculate the mass (g) of hydrogen gas that can be prepared from 5.70 g of SrH2 and 4.75 g of H2O.(a) What amount (mol) of H 2 can be produced from the given mass of SrH 2?
Metal hydrides react with water to form hydrogen gas and the metal hydroxide. For example, SrH2(s) + 2H2O(l) ⟶Sr(OH)2(s) + 2H2(g)You wish to calculate the mass (g) of hydrogen gas that can be prepared from 5.70 g of SrH  2 and 4.75 g of H2O.(b) What amount (mol) of H 2 can be produced from the given mass of H 2O?
ABS plastic is a tough, hard plastic used in applications requiring shock resistance. The polymer consists of three monomer units: acrylonitrile (C3H3N), butadiene (C4H6), and styrene (C8H8). A sample of ABS plastic contains 8.80% N by mass. It took 0.605 g of Br  2 to react completely with a 1.20-g sample of ABS plastic. Bromine reacts 1:1 (by moles) with the butadiene molecules in the polymer and nothing else. What is the percent by mass of acrylonitrile and butadiene in this polymer?
ABS plastic is a tough, hard plastic used in applications requiring shock resistance. The polymer consists of three monomer units: acrylonitrile (C3H3N), butadiene (C4H6), and styrene (C8H8). A sample of ABS plastic contains 8.80% N by mass. It took 0.605 g of Br  2 to react completely with a 1.20-g sample of ABS plastic. Bromine reacts 1:1 (by moles) with the butadiene molecules in the polymer and nothing else. What are the relative numbers of each of the monomer units in this polymer?
When powdered zinc is heated with sulfur, a violent reaction occurs, and zinc sulfide forms: Zn(s) + S8(s) ⟶ZnS(s) [unbalanced] Some of the reactants also combine with oxygen in air to form zinc oxide and sulfur dioxide. When 83.2 g of Zn reacts with 52.4 g of S8, 104.4 g of ZnS forms.(b) If all the remaining reactants combine with oxygen, how many grams of each of the two oxides form?
What mass of Ca(OH)2 will react with 25.0 g of butanoic to form the preservative calcium butanoate according to the equation?
Sulfuric acid dissolves aluminum metal according to the following reaction:2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g)Suppose you wanted to dissolve an aluminum block with a mass of 15.6ga. What minimum mass of H2SO4 would you need? Express your answer in grams.b. What mass of H2 gas would be produced by the complete reaction of the aluminum block? Express your answer in grams. 
You may want to reference (Pages 141 - 145) Section 4.2 while completing this problem.Calculate how many moles of NH3 form when each quantity of reactant completely reacts according to the equation:3N2H4 (l) → 4NH3(g) + N2(g)2.5 mol N2H4
You may want to reference (Pages 141 - 145) Section 4.2 while completing this problem.Calculate how many moles of NH3 form when each quantity of reactant completely reacts according to the equation:3N2H4 (l) → 4NH3(g) + N2(g)3.80 mol N2H4
You may want to reference (Pages 141 - 145) Section 4.2 while completing this problem.Calculate how many moles of NH3 form when each quantity of reactant completely reacts according to the equation:3N2H4 (l) → 4NH3(g) + N2(g)63.8 g N2H4
You may want to reference (Pages 141 - 145) Section 4.2 while completing this problem.Calculate how many moles of NH3 form when each quantity of reactant completely reacts according to the equation:3N2H4 (l) → 4NH3(g) + N2(g)4.76 kg N2H4
You may want to reference (Pages 141 - 145) section 4.2 while completing this problem.Sulfuric acid dissolves aluminum metal according to the following reaction:2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g)Suppose you wanted to dissolve an aluminum block with a mass of 15.2 g .What minimum mass of H2SO4 would you need?
When Heated, KClO3 decomposes into KCl and O2. 2KClO3 → 2KCl+3O2 If this reaction produced 25.8 g of KCl, how much O2 was produced? (in grams)  
Nitroglycerine decomposes violently according to the chemical equation below. What mass of carbon dioxide gas is produced from the decomposition of 5.00 g C3H5(NO3)3?__C3H5(NO3)3 (l) → __CO2 (g) + __N2 (g) + __H2O (g) + __O2 (g)
One way to synthesize ethylamine (CH 3CH2NH2) is from the reaction of ammonia (NH3) with chloroethane (CH 3CH2Cl). (1)   NH3 + CH3CH2Cl → CH3CH2NH2 + HCl One problem with this synthesis route is that the above reaction is not very selective, and ammonia may react with two chloroethane molecules to form diethylamine ( (CH3CH2)2NH ). (2)   NH3 + 2 CH3CH2Cl → (CH3CH2)2NH + 2 HCl A mixture of 0.475 mol NH3/mol, 0.475 mol CH3CH2Cl/mol and the remainder inerts is fed into a reactor. Within the reactor, the fractional conversion of CH3CH2Cl is 0.840 and the fractional yield of CH3CH2NH2 is 0.390. Assume a 100 mol basis for the feed stream, and calculate the number of moles of each component entering the reactor and leaving in the product stream.
The reaction of chlorine gas with solid phosphorus produces solid phosphorus pentachloride. How many grams of PCl5 are produced from 3.5 g of Cl 2?5Cl2(g) + 2P(s) → 2PCl(s)
In an experiment in which 36.04 g of liquid water is decomposed into hydrogen gas and oxygen gas, the total mass of the products isa. 0 gb. 18.02 gc. 36.04 gd. uncertain 
When heated, KClO3 decomposes into KCl and O2.2 KClO3 → 2KCl + 3O2If this reaction produced 62.1 grams of KCl, how much O2 was produced (in grams)? 
Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. a. Write the balanced chemical equation for this reaction.b. How many grams of aluminum hydroxide are obtained from 16.2 of aluminum sulfide?
Determine the minimum volume of 3.8 M HI required to completely dissolve sample of 2.30 g of Al. 
In the reaction of ammonia, NH3, with oxygen, O2, below, balance the equation and answer the questions a and b.NH3 + 5O2 → NO + H2Oa. How many moles of oxygen are needed to react with 5.0 moles of ammonia?b. In the above reaction, how many moles of water can be produced from 256 grams of oxygen?
Carborundum is silicon carbide, SiC, a very hard material used as an abrasive on sandpaper and in other applications. It is prepared by the reaction of pure sand, SiO2, with carbon at high temperature. Carbon monoxide, CO, is the other product of this reaction. Write the balanced equation for the reaction, and calculate how much SiO2 is required to produce 3.00 kg of SiC.
In an accident, a solution containing 2.5 kg of nitric acid was spilled. Two kilograms of Na2CO3 was quickly spread on the area and CO2 was released by the reaction. Was sufficient Na2CO3 used to neutralize all of the acid?
A compact car gets 37.5 miles per gallon on the highway. If gasoline contains 84.2% carbon by mass and has a density of 0.8205 g/mL, determine the mass of carbon dioxide produced during a 500-mile trip (3.785 liters per gallon).
The human body excretes nitrogen in the form of urea, NH 2CONH2. The key step in its biochemical formation is the reaction of water with arginine to produce urea and ornithine:(b) How many grams of nitrogen can be excreted as urea when 135.2 g of ornithine is produced?
Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following:(a) The number of moles and the mass of chlorine, Cl 2, required to react with 10.0 g of sodium metal, Na, to produce sodium chloride, NaCl.
Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following:(b) The number of moles and the mass of oxygen formed by the decomposition of 1.252 g of mercury(II) oxide.
Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following:(c) The number of moles and the mass of sodium nitrate, NaNO 3, required to produce 128 g of oxygen. (NaNO2 is the other product.)
Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following:(d) The number of moles and the mass of carbon dioxide formed by the combustion of 20.0 kg of carbon in an excess of oxygen.
Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following:(e) The number of moles and the mass of copper(II) carbonate needed to produce 1.500 kg of copper(II) oxide. (CO2 is the other product.)
Calculate the mass (g) of each product formed when 174 g of silver sulfide reacts with excess hydrochloric acid: Ag2S(s) + HCl(aq) ⟶AgCl(s) + H2S(g) [unbalanced]
Determine the number of moles and the mass requested for each reaction in each of the following:(a) The number of moles and the mass of chlorine, Cl 2, required to react with 10.0 g of sodium metal, Na, to produce sodium chloride, NaCl.
Elemental phosphorus occurs as tetratomic molecules, P4. What mass (g) of chlorine gas is needed to react completely with 455 g of phosphorus to form phosphorus pentachloride?
Determine the number of moles and the mass requested for each reaction in each of the following:(b) The number of moles and the mass of oxygen formed by the decomposition of 1.252 g of mercury(II) oxide.
Elemental sulfur occurs as octatomic molecules, S 8. What mass (g) of fluorine gas is needed to react completely with 17.8 g of sulfur to form sulfur hexafluoride?
Determine the number of moles and the mass requested for each reaction in each of the following:(c) The number of moles and the mass of sodium nitrate, NaNO 3, required to produce 128 g of oxygen. (NaNO2 is the other product.)
Hydroxyapatite, Ca5(PO4)3(OH), is the main mineral component of dental enamel, dentin, and bone. Coating the compound on metallic implants (such as titanium alloys and stainless steels) helps the body accept the implant. When placed in bone voids, the powder encourages natural bone to grow into the void. Hydroxyapatite is prepared by adding aqueous phosphoric acid to a dilute slurry of calcium hydroxide.b) What mass (g) of hydroxyapatite could form from 100. g of 85% phosphoric acid and 100. g of calcium hydroxide?
Determine the number of moles and the mass requested for each reaction in each of the following:(d) The number of moles and the mass of carbon dioxide formed by the combustion of 20.0 kg of carbon in an excess of oxygen.
Solid iodine trichloride is prepared in two steps: first, a reaction between solid iodine and gaseous chlorine to form solid iodine monochloride; second, treatment of the solid with more chlorine gas. (c) How many grams of iodine are needed to prepare 2.45 kg of final product?
Determine the number of moles and the mass requested for each reaction in each of the following:(e) The number of moles and the mass of copper(II) carbonate needed to produce 1.500 kg of copper(II) oxide. (CO2 is the other product.)
Consider the unbalanced equation for the combustion of hexane:C6H14(g) + O2(g) → CO2(g) + H2O(g)Determine how many moles of O2 are required to react completely with 6.1 moles C6 H14.
Consider the unbalanced equation for the neutralization of acetic acid:HC2H3O2(aq) + Ba(OH)2(aq) → H2O(l) + Ba(C2H3O2)2(aq)Determine how many moles of Ba(OH)2 are required to completely neutralize 0.451 mole of HC2H3O2.
Lead can be prepared from galena [lead(II) sulfide] by first roasting the galena in oxygen gas to form lead(II) oxide and sulfur dioxide. Heating the metal oxide with more galena forms the molten metal and more sulfur dioxide.(c) How many metric tons of sulfur dioxide form for every metric ton of lead obtained?
Determine the number of moles and the mass requested for each reaction in each of the following:(f) 
Various nitrogen oxides, as well as sulfur oxides, contribute to acidic rainfall through complex reaction sequences. Nitrogen and oxygen combine during the high-temperature combustion of fuels in air to form nitrogen monoxide gas, which reacts with more oxygen to form nitrogen dioxide gas. In contact with water vapor, nitrogen dioxide forms queous nitric acid and more nitrogen monoxide. (c) How many metric tons (t) of nitric acid form when 1350 t of atmospheric nitrogen is consumed (1 t = 1000 kg)?
For the reaction between solid tetraphosphorus trisulfide and oxygen gas to form solid tetraphosphorus decoxide and sulfur dioxide gas, write a balanced equation. Show the equation from the following table in terms of moles.
There are two binary compounds of mercury and oxygen. Heating either of them results in the decomposition of the compound, with oxygen gas escaping into the atmosphere while leaving a residue of pure mercury. Heating 0.6498 g of one of the compounds leaves a residue of 0.6018 g. Heating 0.4172 g of the other compound results in a mass loss of 0.016 g. Determine the empirical formula of each compound.
The zinc in a 1.343-g sample of a foot powder was precipitated as ZnNH  4PO4. Strong heating of the precipitate yielded 0.4089 g Zn2P2O7. Calculate the mass percent of zinc in the sample of foot powder.
The following scene represent a chemical reaction between AB 2 and B2:(c) How many moles of product can be made from 3.0 mol of B 2 and 5.0 mol of AB 2?
Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following:(b) The number of moles and the mass of oxygen formed by the decomposition of 1.252 g of silver(I) oxide.
Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following:(c) The number of moles and the mass of magnesium carbonate, MgCO 3, required to produce    283 g of carbon dioxide. (MgO is the other product.)
For the reaction between solid tetraphosphorus trisulfide and oxygen gas to form solid tetraphosphorus decoxide and sulfur dioxide gas, write a balanced equation. Show the equation from the following table in terms of grams.
Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following:(d) The number of moles and the mass of water formed by the combustion of 20.0 kg of acetylene, C2H2, in an excess of oxygen.
A 0.755-g sample of hydrated copper(II) sulfateCuSO4 • x H2Owas heated carefully until it had changed completely to anhydrous copper(II) sulfate (CuSO 4) with a mass of 0.483 g. Determine the value of x. [This number is called the number of waters of hydration of copper(II) sulfate. It specifies the number of water molecules per formula unit of CuSO4 in the hydrated crystal.]
Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following:(e) The number of moles and the mass of barium peroxide, BaO 2, needed to produce 2.500 kg of barium oxide, BaO (O2 is the other product.)
The multistep smelting of ferric oxide to form elemental iron occurs at high temperatures in a blast furnace. In the first step, ferric oxide reacts with carbon monoxide to form Fe3O4. This substance reacts with more carbon monoxide to form iron(II) oxide, which reacts with still more carbon monoxide to form molten iron. Carbon dioxide is also produced in each step.(b) How many grams of carbon monoxide are required to form 45.0 metric tons of iron from ferric oxide?
One of the compound used to increase the octane rating of gasoline is toluene (ball-and-stick model is shown). Suppose 20.0 mL of toluene (d = 0.867 g/mL) is consumed when a sample of gasoline burns in air. (a) How many grams of oxygen are needed for complete combustion of the toluene?
One of the compound used to increase the octane rating of gasoline is toluene (ball-and-stick model is shown). Suppose 20.0 mL of toluene (d = 0.867 g/mL) is consumed when a sample of gasoline burns in air. (b) How many total moles of gaseous products form?
One of the compounds used to increase the octane rating of gasoline is toluene (ball-and-stick model is shown). Suppose 20.0 mL of toluene (d = 0.867 g/mL) is consumed when a sample of gasoline burns in air.(c) How many molecules of water vapor form?
Determine the number of moles and the mass requested for each reaction in each of the following:(a) The number of moles and the mass of Mg required to react with 5.00 g of HCl and produce MgCl2 and H2.
Determine the number of moles and the mass requested for each reaction in each of the following:(b) The number of moles and the mass of oxygen formed by the decomposition of 1.252 g of silver(I) oxide.
Determine the number of moles and the mass requested for each reaction in each of the following:(c) The number of moles and the mass of magnesium carbonate, MgCO 3, required to produce    283 g of carbon dioxide. (MgO is the other product.)
Determine the number of moles and the mass requested for each reaction in each of the following:(d) The number of moles and the mass of water formed by the combustion of 20.0 kg of acetylene, C2H2, in an excess of oxygen.
Determine the number of moles and the mass requested for each reaction in each of the following:(e) The number of moles and the mass of barium peroxide, BaO 2, needed to produce 2.500 kg of barium oxide, BaO (O2 is the other product.)
Determine the number of moles and the mass requested for each reaction in each of the following:(f) 
The world burns approximately 3.7 x 1012 kg of fossil fuel per year.Use the combustion of octane as the representative reaction and determine the mass of carbon dioxide (the most significant greenhouse gas) formed per year. The current concentration of carbon dioxide in the atmosphere is approximately 399 ppm (by volume).
a. How many moles of NH3 can be produced from 16.5 mol of H 2 and excess N2?b. How many grams of NH3 can be produced from 3.78 mol of N 2 and excess H2.c. How many grams of H 2 are needed to produce 11.05 g of NH3 ?d. How many molecules (not moles) of NH3 are produced from 2.92 × 10−4 g of H2?
Lead (II) oxide, PbO, reacts with ammonia, NH 3, as follows:3PbO + 2NH3 → 3Pb + N 2 + 3H2OHow many grams of Pb are formed when 0.105 g NH 3 react?
The reaction of coal and water at a high temperature produces a mixture of hydrogen and carbon monoxide gases. This mixture is known as synthesis gas (or syngas). What mass of water is required for the formation of 175 grams of carbon monoxide? C(s) + H2O(g) → H2(g) + CO(g)
Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. a. Write a balanced equation for this reaction. b. How many grams of aluminum hydroxide can be obtained from 5.50 g of aluminum sulfide?
What is the concentration of alcohol, in terms of molarity, in blood if the BAC is 0.08?
Elemental S reacts with O2 to form SO3 according to the reaction:2S + 3O2 → 2SO3a. How many O2 molecules are needed to react with 5.69 g of S? Express your answer numerically in units of molecules.b. What is the theoretical yield of SO3 produced by the quantities described in part a? Express your answer numerically in grams. 
Propane, C3H8, is commonly used as a fuel in gas grills. It reacts with oxygen according toC3H8 + 5O2 → 3CO2 + 4H2OHow many grams of propane can be burned by 24 g of O 2?
Iodine is prepared both in the laboratory and commercially by adding Cl2(g) to an aqueous solution containing sodium iodide:2Nal(aq) + CI2(g) --> l2(s) + 2 NaCl(aq)How many grams of sodium iodide, Nal, must be used to produce 45.8 g of iodine, I2?
Sulfuric acid dissolves aluminum metal according to the following reaction: 2 Al(s) + 3H2SO4 (aq) --> Al2(SO4)3 (aq) + 3H2 (g)Suppose you wanted to dissolve an aluminum block with a mass of 14.3 g. What minimum mass of H2SO4 would you need? Express your answer in grams.What mass of H2 gas would be produced by the complete reaction of the aluminum block? Express your answer in grams.
Green plants use light from the Sun to drive photosynthesis. Photosynthesis is a chemical reaction in which water (H2O) and carbon dioxide (CO2) chemically react to form the simple sugar glucose (C6H12O6) and oxygen gas (O2). What mass of simple sugar glucose is produced by the reaction of 8.14 g of carbon dioxide? Be sure your answer has the correct number of significant digits.
How many grams of H2 are needed to produce 11.73 g of NH3? Express your answer numerically in grams. How many molecules (not moles) of NH3 are produced from 8.42 times 10^-4 g of H2? Express your answer numerically as the number of molecules.
Calculate the mass of water (in grams) present in 9.41 g of CaCl_2 2 H_2O. Select one. a. 1.53 g b. 3.06 g c. 2.31 g d. 1.15 g
How many moles of N2 are needed to react with 7.96 mol of O2? How many moles of NO can be formed when 6.16 mol of N2 reacts?
If there are 1.50 mol of H, how many moles of each of the following compounds are present?
Ammonium perchlorate (NH4ClO4) is the solid rodent fuel used by the U.S. Space Shuttle. It reacts with itself to produce nitrogen gas (N2) chlorine gas (Cl2) oxygen gas (O2) water (H2O) and a great deal of energy. What mass of chlorine gas is produced by the reaction of 4.5 g of ammonium perchlorate? Round your answer to 2 significant digits.
A sample of sodium reacts completely with 0.284 kg of chlorine, forming 468 g of sodium chloride. What mass of sodium reacted? Express your answer to three significant figures and include the appropriate units.
The fuel used in many disposable lighters is liquid butane, C4H10. How many carbon atoms are in 4.00 g of butane?Express your answer numerically in atoms.
Sulfuric acid dissolves aluminum metal according to the reaction:2 Al(s) + 3H2SO4(aq) ---> Al2(SO4)3(aq) + 3 H(g)Suppose you wanted to dissolve an aluminum block with a mass of 11.2 g. What minimum mass of H2SO4 (in g) would you need? What mass of H2, gas (in g) would be produced by the complete reaction of the aluminum block? 
What mass of oxygen is required to react with calcium to produce 44.8 g calcium oxide? 25 6 g, 51.1 g, 0.399 g, 6.39 g, 12.8 g
Ammonium phosphate ((NH4)3PO4) is an important ingredient in many fertilizers. It can be made by reacting phosphoric acid (H3PO4) with ammonia (NH3).What mass of ammonium phosphate is produced by the reaction of 6.88 g of phosphoric acid? Be sure your answer has the correct number of significant digits.
A flask contains 0.380 mol of liquid bromine. Br2. Determine the number of bromine molecules present in the flask. Express your answer numerically in molecules.Calculate the mass of 1.00 times 10^24 (a septillion) molecules of water. Express the answer numerically in grams. Express the answer numerically in grams.
Ammonia and oxygen react to form nitrogen and water.4NH3(g) +3O2 (g) --> 2N2(g) +6H2O(g)How many grams of N2 can be produced when 6.10 of O2 reacts?How many grams of water are formed from the reaction of 35.0 g of NH2?
If 0,356 moles of zinc reacts with excess lead(V) sulfate, how many grams of zinc sulfate would be produced in the following reaction? Pb(SO4)2 + 2Zn → 2ZnSO4 + Pb 
How many GRAMS of nitrogen are present in 2.65 moles of dinitrogen tetrafluoride? How many MOLES of fluorine are present in 1.28 grams of dinitrogen tetrafluoride?
Calculate the number of moles of aluminum and silicon required to produce 143 g of chromium based on the following equations: Cr2O3 + 2 Al → 2 Cr + Al 2O3 2Cr2O3 + 3 Si → 4 Cr + 3 SiO 2 Moles of aluminum: Moles of silicon:
According to the following reaction, how many grams of water are necessary to form 0.417 moles zinc hydroxide?zinc oxide (s) + water (l) → zinc hydroxide (aq)
In the following reaction, how many grams of sodium chromate, Na2CrO4, will be needed to react with 36.1 g of silver nitrate, AgNO3?2 AgNO3 + Na2CrO4 → Ag2CrO4 + 2NaNO3
CH4 and O2 react to form CO2 and H2O. Determine the amount of O2 needed to react with 9.25 g of CH4 to produce 25.44 g of CO2 and 20.83 g of H2O.
Butane gas is compressed and used as a liquid fuel in disposable cigarette lighters and lightweight camping stoves. Suppose a lighter contains 5.82 mL of butane (d = 0.579 g mL). (a) How many grams of oxygen are needed to burn the butane completely? (b) How many moles of H2O form when all the butane burns? (c) How many total molecules of gas form when the butane burns completely? 
Enter your answer in the provided box.Use the balanced equation to answer the question. 2C2H6 (g) + 5O2 (g) → 4CO (g) + 6H2O (g) How many moles of O2 are needed to react completely with 3.0 moles of C 2H6?
Be sure to answer all parts. Calculate the mass of each product formed when 127 g of silver sulfide reacts with excess hydrochloric acid: Ag2S (s) + HCl (aq) → AgCl (s) + H2S (s) [unbalanced] Mass of AgCl:Mass of H2S:
According to the following reaction, how many grams of iodine are necessary to form 0.544 moles hydrogen iodide? hydrogen (g) + iodine (s) → hydrogen iodide (g).
 If 0.376 moles of zinc reacts with excess lead(v) sulfate, how many grams of zinc sulfate would b produced in the following reaction? 
How many grams of oxygen gas must react to give 2.10 g of ZnO?2Zn(s) + O2(g) → 2 ZnO(s)Express your answer with the appropriate units.
For many years the extraction of gold-that is, the separation of gold from other materials-involved the use of potassium cyanide:4Au + SKCN + O2 + 2H2O → 4KAu(CN)2 + 4KOHWhat is the minimum amount of KCN in moles needed to extract 32.8 g of gold?
For the reaction Cl2 + 2KBr → 2KCl + Br2, how many moles of potassium chloride are produced from 85.4 g of potassium bromide? Select one: a. 0.718 b. 1.02e4 c. 1.44. d. 1.79
Enter your answer in the provided box.How many grams of phosphine (PH 3) can form when 23.8 g of phosphorus and 88.2 L of hydrogen gas react at STP? P4(s) + H2(g) → PH3(g)       [Unbalanced] 
Portland cement is a mixture of the oxides of calcium, aluminum, and silicon. The raw material for its calcium oxide is calcium carbonate, which occurs as the chief component of a natural rock, limestone. When calcium carbonate is strongly heated it decomposes. One product, carbon dioxide, is driven off to leave the desired calcium oxide as the only other product. Write the balanced chemical equation for the decomposition of calcium carbonate (include physical states of the compounds in your answer): A chemistry student is to prepare 1.50 x 102 g of calcium oxide in order to test a particular "recipe" for Portland cement. How many grams of carbon dioxide are produced?
Calculate the mass of hydrogen from the reaction of 2.70 g of aluminum metal and hydrochloric acid. Al (s) + HCl (aq) → AlCl3 (aq) + H2 (g) (a) 0.606 g (b) none of these (c) 0.202 g (d) 0.303 g (e) 0.135 g
Balance the equation below and determine the mass in grams of N2 needed to produce 11.35g of NH3. H2 + N2 → ____NH3
Ammonia (NH3) chemically reacts with oxygen gas (O2) to produce nitric oxide (NO) and water (H2O). What mass of oxygen gas is consumed by the reaction of 5.43 g of ammonia? Be sure your answer has the correct number of significant digits.
According to the following reaction, how many moles of carbon dioxide will be formed upon the complete reaction of 25.1 grams of propane (C3H8) with excess oxygen gas? propane (C3H8) (g) + oxygen (g) → carbon dioxide (g) + water 
Iron (III) oxide reacts with aluminum metal powder to make aluminum oxide and iron metal (and a whole lotta heat!). Use the balanced chemical equation to calculate the number of moles of iron(lll) oxide needed to form 3.6 mol of iron. Report only your numerical answer with correct sig figs (but DO NOT type units in the answer).
According to the following reaction, how many grams of mercury(II) oxide are necessary to form 0.339 moles oxygen gas? mercury(II) oxide (s) → mercury (I) + oxygen (g) 
Part AHow many moles of NH3 can be produced from 15.0 mol of H2 and excess N2? Express your answer numerically in moles. Part BHow many grams of NH3 can be produced from 2.83 mol of N2 and excess H2. Express your answer numerically in grams.
According to the following reaction, how many moles of hydrogen iodide will be formed upon the complete reaction of 0.283 moles hydrogen gas with excess iodine? hydrogen (g) + iodine (s) → hydrogen iodide (g)
Be sure to answer all parts.Aspirin or acetyl salicylic acid is synthesized by reacting salicylic acid with acetic anhydride:C7H6O3          + C4H6O3                → C9H8O4  +  C2H4O2 salicylic acid    acetic anhydride        aspirin        acetic acid(a) How much salicylic acid is required to produce 0.450 g of aspirin, assuming acetic anhydride is  present in excess? (b) Calculate the amount of salicylic acid needed if only 72.8 percent of salicylic acid is converted to aspirin. 
The combustion of octane (C8H18) is represented by the following equation: 2C8H18 + 25O2 → 16CO2 + 18H2O How many grams of carbon dioxide (CO2) are formed from 0.563 g of octane? 
Use reaction stoichiometry to calculate amounts of reactants and products. The substances magnesium nitride and water react to form magnesium hydroxide and ammonia. Unbalanced equation: Mg3N2 (s) + H2O (I) → Mg(OH)2 (aq) + NH3 (aq) In one reaction, 72.4 g of NH3 is produced. What amount (in mol) of H2O was consumed? What mass (in grams) of Mg(OH)2 is produced? 
According to the following reaction, how many grams of hydrobromic acid are necessary to form 0.424 moles bromine? hydrobromic acid (aq) → hydrogen (g) + bromine (l) 
A 1.560 - g sample of the alcohol CH3CHOHCH2CH3 is burned in an excess of oxygen. Part AWhat mass of CO2 should be obtained? Express your answer using four significant figures. Part BWhat mass of H2O should be obtained? Express your answer using four significant figures.
How many moles of NaOH will react with 1 mole of H2SO4 in the below unbalanced reaction? NaOH + H2SO4 → H2O + Na2SO4 
2.0 g of hydrogen reacts with enough nitrogen to make 11.4 g of ammonia, how much nitrogen was used in this reaction? (i) 13.4 g (ii) 9.4 g (iii) 11.4 g (iv) 2.0 g
The uranium minerals found in nature must be refined and enriched in  235U before the uranium can be used as a fuel in nuclear reactors. One procedure for enriching uranium begins with the reaction of natural UO2 with HF to form UF4, which is then converted into UF6 by reaction with fluorine: UO2 (g) + 4 HF (g) → UF4 (g) + 2H2O (l) UF4 (g) + F2 (g) → UF6 (g) a. How many kilograms of HF are needed to completely react with 2.25 kg of UO  2? b. How much UF6 can be produced from 830 g of UO2?
If 7.65 moles of C5H12 reacts with excess O2, how many moles of CO2 will be produced in the following combustion reaction? C5H12 + 8O2 → 6H2O + 5CO2
Part BWhat is the maximum amount in moles of P2O5 that can theoretically be made from 272 g of O2 and excess phosphorus? Express your answer to three significant figures and include the appropriate units.
The common pain relievers - aspirin (C9H8O4), acetaminophen (C8H9NO2), and naproxen sodium (C14H13O3Na) - are available in tablets containing 375 mg of the active ingredient. How many molecules of the active ingredient are present in each tablet? 375 mg aspirin = 375 mg acetaminophen = 375 mg naproxen sodium =
According to the following reaction, how many moles of nitrogen gas will be formed upon the complete reaction of 29.4 grams of ammonium nitrite?ammonium nitrite (aq) → nitrogen (g) + water (l)
When hydrogen sulfide reacts with oxygen, water and sulfur dioxide are produced. The balanced equation for this reaction is: 2H2S (g) + 3O2 (g) → 2H2O (l) + 2SO2 (g) If 9 moles of oxygen react, The reaction consumes _______ moles of hydrogen sulfide. The reaction produces _______ moles of water _______and moles of sulfur dioxide.
Potassium metal (K) reacts violently when added to water according to the balanced equation: 2K(s) + 2 H2O(l) → 2 KOH(aq) + H2(g). How many moles of H2O are needed to react completely with 754 mol of K? a. 2 mol of H2O b. 7.54 mol of H2O c. 15.1 mol of H2O d. 3.77 mol of H2O
Consider the following imbalanced equation: MnO2 (s) + Al (s) →How many grams of Al are required to completely react with 56.2 g of MnO2? How many moles of Al are required to completely react with 0.646 mol MnO2? 3MnO2 (s) + 4Al (s) → 3Mn (s) + 2Al2O3 (s) 
When heated, KCIO3 decomposes into KCI and O2. 2KCIO3 → 2KCI + 3O2 If this reaction produced 60.3 g of KCI, how much O2 was produced (in grams)?
Be sure to answer all parts.How many grams of chloride gas can be produced from the electrolyte decomposition of 185 g of calcium chloride? Select the name of the other product and enter the mass of the other product produced. hydrogen oxygen water calcium 
Pb(OH)Cl, one of the lead compounds used in ancient Egyptian cosmetics, was prepared from PbO according to the following ancient recipe: PbO + NaCl + H2O → Pb(OH)Cl + NaOH How many grams of PbO and how many grams of NaCl would be required to produce 10.0 g of Pb(OH)Cl? Mass of PbO required = Mass of NaCl required =
For the reaction, calculate how many moles of the product form when 0.021 mol of O2 completely reacts. Assume that there is more than enough of the other reactant. 2Ca(s) + O2 (g) → 2CaO(s) Express your answer using two significant figures. Part BFor the reaction, calculate how many moles of the product form when 0.048 mol of O2 completely reacts. Assume that there is more than enough of the other reactant. 4 Fe (s) + 3O2 (g) → 2Fe2O3 (s) Express your answer using two significant figures.
Use balanced chemical equations to relate amounts of reactants and products. The unbalanced equation for the reaction between carbon dioxide and potassium hydroxide is shown below. Balance the equation (enter the smallest integer possible in each box, including the integer "1" when needed) and determine the amount of KOH consumed and the amounts of K2CO3 and H2O produced when 0.816 mol of CO2 reacts. _CO2 (g) + _KOH (aq) → _K2CO3 (aq) + _H2O (l) mol 
Be sure to answer all parts. Calculate the mass of each product formed when 506 g of silver sulfide reacts with excess hydrochlorie acid: Ag2S (s) + HCI (aq) → AgCI (s) + H2S (g) [unbalanced] Mass of AgCl: Mass of H2S:
According to the following reaction, how many grams of sulfuric acid are necessary to form 0.309 moles aluminum sulfate? aluminum oxide (s) + sulfuric acid (aq) → aluminum sulfate (aq) + water (l)
In the combustion of hydrogen gas, hydrogen reacts with oxygen from the air to form water vapor. hydrogen + oxygen → water If you bun 27.8 g of hydrogen and produce 249 g of water, how much oxygen reacted?
According to the following reaction, how many moles of water are necessary to form 0.445 moles zinc hydroxide? zinc oxide (s) + water (1) → zinc hydroxide (aq)
According to the following reaction, how many grams of water are necessary to form 0.650 moles hydrofluoric acid? silicon tetrafluoride (s) + water (I) → hydrofluoric acid (aq) + silicon dioxide (s) 
Use the balanced equation for the reaction of N 2 and O2 to form NO to answer the question. N2 (g) + O2 (g) → 2NO (g) How many moles of NO are formed from 1.1 moles of N 2? 
When copper(II) sulfate pentahydrate (CuSO4•5H2O) is heated, it decomposes to the dehydrated form. The waters of hydration are released from the solid crystal and form water vapor.The hydrated form is medium blue, and the dehydrated solid is light blue. The balanced equation is: CuSO4•5H2O(s) heat→ CuSO4(s) + 5H2O(g)If 3.63g CuSO4•5H2O is decomposed to CuSO4, predict the mass of the remaining light blue solid. 
The combustion of octane (C8H18) is represented by the following equation: 2C 8H18 + 25O2 → 16CO2 + 18H2O How many grams of carbon dioxide (CO2) are formed from 0.221 g of octane?  
Balance the following reaction. Pb(NO3)3 + KI → KNO3 +PbI2Based on the balanced chemical equation above, determine the moles of KI needed to produce 3.00 moles of Pbl2 in the reaction.
A) The reaction between iron (ll) oxide and carbon monoxide produces iron and carbon dioxide. How many moles of iron can be obtained when 1.25 mol FeO reacts with an excess of CO? FeO + CO → Fe + CO2 B) The reaction between hydrochloric acid and aluminum produces hydrogen gas and aluminum chloride. The balanced reaction equation is given below. How many moles of H2 can be obtained when 6.00 mol HCl reacts with an excess of Al? 6HCl + 2A → 3H2 + 2AlCl3
According to the following reaction, how many moles of nitrogen gas will be formed upon the complete reaction of 0.741 moles ammonium nitrite? ammonium nitrite (aq) → nitrogen (g) + water (l)
Part 1Use the following balanced equation: 2H2 + O2 → 2H2O If you start with 24 molecules of hydrogen gas, how marry molecules of oxygen gas do you need?Part 2How many molecules of water are made from the amount of starting materials described above? 
According to the following reaction, how many moles of sodium hydroxide will be formed upon the complete reaction of 29.6 grams of sodium with excess water? sodium (s) + water (l) → sodium hydroxide (aq) + hydrogen (g) 
How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 65.1 moles of water vapor?
How many moles of H2O(g) are produced when 4.3 grams O2(g) are consumed? C4H6(g) + O2(g) → CO2(g) + H2O(g) (not balanced)a. 75 b. 0.073c. 0.25d. 0.72e. 140 
2 NH4NO3 → N2 + O2 + 4 H2OPart BDetermine how much oxygen in grams is produced by the complete reaction of 3.27 kg of ammonium nitrate.
If 0.184 mole of I2 reacts with K according to the equation 2 K + I 2 → 2 KI, how many moles of KI will form? Select one:a. 0.184 moleb. 0.0920 molc. 0.736 mold. 0.368 mol 
In the reaction below, how many grams of calcium carbonate are required to produce 30.50 g of carbon dioxide?
The manufacture of aluminum includes the production of cryolite (Na3AlF6) from the following reaction: 6HF + 3NaAlO2 → Na3AlF6 + 3H2O + Al2O3. How much NaAlO2 (sodium aluminate) is required to produce 4.60 kg of Na3AlF6? 
The combustion of ethane (C2H6) produces carbon dioxide and steam: 2C2H6 (g) + 7O2 (g) → 4CO2 (g) + 6H2O (g)How many moles of CO2 are produced when 5.85 mol of ethane are burned in an excess of oxygen?
For the balanced reaction 4NH3 + 3O2 → 2N2 + 6H2O (Atomic weights: H = 1.0 g/mol: N = 14.0 g/mol: O = 16.0 g/mol), the mass of oxygen needed to react with 75.0 g of ammonia is (a) 188 g (b) 106 g (c) 141 g (d) 53.0 g
For the reaction 2C2H5OH + 2Na2Cr2O7 + 16HCI → 3CH3COOH + 4CrCl3 + 4NaCl + 11H2O the yield (called a theoretical yield) of CrCl3 we can get from the reaction of 14.0 mol of C2H5OH, 10.0 mol of Na2Cr2O7 and 50.0 mol of HCI would be (a) 20.0 mol (b) 28.0 mol (c) 10.0 mol (d) 12.5 mol
Write the balanced equation for the reaction of aqueous Pb(CIO 3)2 with aqueous Nal. Include phases. What mass of precipitate will form if 1.50 L of highly concentrated Pb(CIO 3)2 is mixed with 0.700 L of 0.190 M Nal? Assume the reaction goes to completion.
A sample of a substance with the empirical formula XBr2 weighs 0.5675 g. When it is dissolved in water and all its bromine is converted to insoluble AgBr by addition of an excess of silver nitrate, the mass of the resulting AgBr is found to be 0.9465 g. The chemical reaction is XBr2 + 2AgNO3 → 2AgBr + X(NO3)2 (a) Calculate the formula mass of XBr2.  (b) Calculate the atomic mass of X.  
Be sure to answer all parts.Potassium nitrate decomposes on heating, producing potassium oxide and gaseous nitrogen and oxygen: 4KNO3 (s) → 2K2O (s) + 2N2 (g) + SO2 (g) To produce 76.3 kg of O2, how many (a) moles of KNO3 must be heated? (b) grams of KNO3 must be heated? 
How many grams of hydrogen peroxide would you need to get 24.7 g of water? Express your answer with the appropriate units. How many grams of hydrogen peroxide would you need to get 24.1 g of O 2? Express your answer with the appropriate units.
Consider the following unbalanced equation: MnO2 (s) + Al (s) →Mn (s) + Al2O3 (s) How many grams of Al are required to completely react with 56.2 g of MnO2? 
When hydrochloric acid reacts with iron(III) oxide, water and iron(III) chloride are produced. The balanced equation for this reaction is: 6HCl (aq) + Fe2O3 (s) → 3H2O (l) + 2FeCl3 (aq) If 12 moles of hydrochloric acid react, (a) The reaction consumes _________ moles of iron(III) oxide. (b) The reaction produces _________ moles of water and moles of iron(III) chloride.
When 123.8 g of ethylene (C2H4) burns in oxygen to give carbon dioxide and water, how many grams of CO2 are formed? a. 388.5 gb. 4.41 g c. 97.1 g d. 159.0 g e. 194.2 g
According to the following reaction, how many grams of dichloromethane (CH2Cl2) will be formed upon the complete reaction of 29.4 grams of carbon tetrachloride with excess methane (CH4) ? methane (CH4) (g) + carbon tetrachloride (g) → dichloromethane (CH2Cl2) (g) 
Green plants use light from the Sun to drive photosynthesis. Photosynthesis is a chemical reaction in which water (H2O) and carbon dioxide (CO2) chemically react to form the simple sugar glucose(C6H12O6) and oxygen gas (O2).What mass of oxygen gas is produced by the reaction of 2.64 g of water? Round your answer to 3 significant digits.
How many atoms of titanium are there in 0.300 mole of each of the following?a. ilmenite, FeTiO3 b. titanium (IV) chloride c. Ti2O3 d. Ti3O5
How many calcium ions are there in 3.73 g of CaCO3?
What mass of the second-listed reactant in each of the following reactions is needed to react completely with 2.014 g of the first-listed reactant? SiO2 + 3C → 2CO + SiC 3NO2+ H2O → 2HNO3 + NO
Iron reacts with 48.0 g of oxygen to make 159.6 g of rust (Fe2O3); how much iron reacted? (a) 111.6 g (b) 48.0 g (c) 207.6 g (d) 55.8 g
How many molecules (not moles) of NH3 are produced from 4.95 x 10-4 g of H2? Express your answer numerically as the number of molecules.
Here is the combustion reaction for octane (C8H18), which is a primary component of gasoline. 2C8H18 + 25O2 → 16CO2 + 18H2O How many moles of CO2 are emitted into the atmosphere when 14.6 g of C8H18 is burned?
Chromium metal can be produced from the high temperature reaction of Cr2O3 [chromium(III) oxide] with silicon or aluminum by each of the following reactions: Cr2O3 + 2Al → 2Cr + Al2O3 2Cr2O3 + 3Si →  4Cr + 3SiO2 Calculate the number of grams of aluminum required to prepare 133 g of chromium metal by the first reaction. Calculate the number of grams of silicon required to prepare 133 g of chromium metal by the second reaction.
7.65 moles of C5H12 reacts with excess O2, how many moles of CO2 will be produced in the following reaction? C5H12 + 8O2 → 6H2O + 5CO2
Nitrogen monoxide is produced by combustion in an automobile engine. According to the following r reaction, how many moles of nitrogen dioxide will be formed upon the complete reaction of 0.318 moles nitrogen monoxide with excess oxygen gas? nitrogen monoxide (g) + oxygen (g) → nitrogen dioxide (g)
The combustion of 987.0 g of methane in the presence of excess oxygen produces 1.543 kg of carbon dioxide. What is the percent yield? (a) 56.8% (b) 38.1% (c) 0.568% (d) 50.0%
Part AHow many moles of methane are produced when 36.6 moles of carbon dioxide gas read with excess hydrogen gas? Express your answer with the appropriate units. For example, write the unit moles as mol. Part BHow many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 65.1 moles of water vapor? Express your answer with the appropriate units. For example, write the unit moles as mol.
The combustion of propane may be described by the chemical equation, C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g) How many grams of O2(g) are needed to completely burn 97.1 g of C3H8(g)?
According to the following reaction, how many moles of ammonium nitrate are necessary to form 0.888 moles water? ammonium nitrate (aq) → dinitrogen monoxide (g) + water (1) moles ammonium nitrate 
When sulfuric acid reacts with calcium hydroxide, calcium sulfate and water are produced. The balanced equation for this reaction is: H2SO4 (aq) + Ca(OH)2 (s) → CaSO4 (s) + 2H2O(1) If 3 moles of calcium hydroxide react.. (a) The reaction consumes ________ moles of sulfuric acid. (b) The reaction produces ________ moles of calcium sulfate and moles of water.
In the reaction of aluminum metal and oxygen to make aluminum oxide, how many grams of oxygen gas will react with 2.2 moles aluminum metal?a. 94b. 53c. 44d. 26e. 1.7 
When 1.0 mol of Fe reacts with Cl2 forming FeCl3, how many moles of Cl2 are required to react with all of the iron?a. none of theseb. 0.7 molc. 0.3 mold. 1.0 mole. 1.5 mol 
Aluminum, silicon, and oxygen form minerals known as aluminosilicates. How many moles of aluminum are in: a. 0.60 moles of pyrophyllite, Al 2Si4O10(OH)2 b. 3.20 moles of mica, KAl 3Si3O10(OH)2 
Hydrazine, N2H4, a substance used as rocket fuel with oxygen as follows:N2H4 (l) + O2 (g) → NO2 (g) + H2O (g) Part ABalance the equaton.Part BHow many moles of oxygen are needed to react with 155 g of hydrazine? Part CHow many grams of oxygen are needed to react with 155 g of hydrazine? Express your answer as a chemical equations. Identify all of the phases in your answer.
Part CHow many grams of H2 are needed to produce 10.16 g of NH 3? Express your answer numerically in grams. Part DHow many molecules (not moles) of NH3 are produced from 3.09 x 10 -4 g of H2? Express your answer numerically as the number of molecules.
What is the theoretical yield of aluminum oxide if 3.60 mol of aluminum metal is exposed to 3.00 mol of oxygen Express your answer with the appropriate units. 
For the following redox reaction, balance the chemical equation, and determine the number of grams of MgO that are needed to produce 3.33 g of Fe2O3. _____ MgO (s) + _____ Fe (s) → _____ Fe2O3 (s) + _____ Mg (s) (i) 7.57 g (ii) 2.52 g (iii) 0.841 g (iv) 0.312 g
When heated, KCIO3 decomposes into KCI and O2. 2KCIO3 → 2KCI + 3O2 If this reaction produced 33.4 g of KCI, how much O2 was produced (in grams)?
Be sure to answer all parts.Iron reacts slowly with oxygen and water to form a compound commonly called rust (Fe2O3•4H3O). For 53.1 kg of rust, calculate the following quantities (a) The moles of compound: (b) The moles of Fe2O3: (c) The grams of iron:
H2 and O2 react to produce H2O. What is the mass of H2O produced when 0.73 g of H2 completely reacts with 3.28 g of O2? Multiple Choice A. 3.57 g B. 4.01g C. 4.25 g D. None of them
According to the following reaction, how many grams of chlorine gas are necessary to form 0.837 moles iron(HI) chloride? iron (s) + chlorine (g) → iron(III) chloride (s) 
Part CHow many grams of H2 are needed to produce 14.58 g of NH3? Express your answer numerically in grams. Part DHow many molecules (not moles) of NH3, are produced from 7.53 x 10-4 g of H2? Express your answer numerically as the number of molecules.
If 4.84 moles of C 5H12 reacts with excess O2, how many moles of CO2 will be produced in the following combustion reaction? C5H12 + 8O2 → 6H2O + 5CO2
Gaseous hydrogen and oxygen can be prepared in the laboratory from the decomposition of gaseous water. The equation for the reaction is 2H2O (g) → + 2H2 (g) + O2 (g) Calculate how many grams of O2(g) can be produced from 56.2 grams of H2O(g).
What is the mass in grams of Br in 1.88 moles of FeBr 3?
Nitrogen monoxide is produced by combustion in an automobile engine. According to the following reaction, how many grams of nitrogen dioxide will be formed upon the complete reaction of 23.4 grams of oxygen gas with excess nitrogen monoxide? nitrogen monoxide (g) + oxygen (g) → nitrogen dioxide (g)
Ammonia (NH3 chemically reacts with oxygen gas (O2) to produce nitric oxide (NO) and water (H2O). What mass of nitric oxide is produced by the reaction of 3.5 g of ammonia? Round your answer to 2 significant digits.
The thermite reaction is one of the most spectacular reactions with fames, sparks and glowing molten iron. Here aluminum reacts with iron (III) oxide to produce aluminum oxide and metallic iron. So much heat is generated that the iron forms in the liquid state Write the balanced chemical equation for this reaction (include physical states of the compounds in your answer): A certain welding operation requires at least 86.0 g of iron each time a weld is made. Calculate the mass of Al2O3 formed under the conditions specified.
The combustion of ethane (C2H6) produces carbon dioxide and steam:2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(g)How many moles of CO2 are produced when 5.65 mol of ethane are burned in an excess of oxygen? 
An automobile gasoline tank holds 22 kg of gasoline. When the gasoline burns, 86 kg of oxygen is consumed, and carbon dioxide and water are produced.You may want to reference (pages 48-51) section 2.3 when completing this problem.Part AWhat is the total combined mass of carbon dioxide and water that is produced? Express your answer with the appropriate units. 
How many atoms of iron are there in 2.20 moles of each of the following?
Coal power plants burn large amounts of coal, C(s), in an O2(g) atmosphere to generate electricity. The chemical reaction responsible for producing this energy is shown below: C(s) + O2(g) → CO2(g) Determine the volume of cop in liters produced when 100 metric ton of C(s) is completely burned in an O2 atmosphere. The density of CO2 is 1.98 kg/m3 (1 metric ton = 1000 kg; 1 m3 = 1000 L)
Under certain circumstances, carbon dioxide, CO2 (g) can be made to react with hydrogen gas, H2 (g) to produce methane, CH4 (g) and water vapour H2O (g).CO2 (g) + 4H2 (g) → CH4 (g) + 2H2O (g) Part AHow many moles of methane are produced when 36.6 moles of carbon dioxide gas react with excess hydrogen gas.Part BHow many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 30.6 moles of water.Express ye answer with the appropriate units.
A major component of gasoline is octane (C8H18). When octane is burned in air, it chemically reacts with oxygen gas (O2) to produce carbon dioxide (CO2)and water (H2O). What mass of octane is consumed by the reaction of 8.5 g of oxygen gas? Round your answer to 2 significant digits.
When NaHCO3 is heated above 270°C, it decomposes to Na2CO3, H2O, and CO2. Write a balanced chemical equation for the decomposition reaction. Calculate the mass of CO2 produced from the decomposition of 19.0 g of NaHCO3
When heated, KClO3 decomposes into KCI and O2. 2KClO3 → 2KCI + 3O2 If this reaction produced 45.8 g of KCl, how much O 2  was produced (in grams)  
The reaction for producing glucose in plants, called photosynthesis, is 6CO2 + H2O light→ C6H12O6 + 6O2If a plant produces 9.36 mol of  C6H12O6, how many moles of CO2 are needed?
If 5.93 moles of C5H12 reacts with excess O2, how many moles of CO2 will be produced in the following combustion reaction? C5H12 + 8O2 → 6H2O + 5CO2
How much NaNO3 is formed in the reaction of 220 grams of sodium chloride with excess lead nitrate in the reaction shown below? 2Nacl + Pb(NO3)2 → 2NaNO3 + PbCl2 a. 161 grams b. 220 grams c. 322 grams d. 644 grams
According to the following reaction, how many grams of oxygen gas are required for the complete reaction of 23.5 grams of hydrochloric acid? hydrochloric acid (aq) + oxygen (g) → water (l) + chlorine (g) 
How many molecules (not moles) of NH3 are produced from 6.33 x 10-4 g of H2? Express your answer numerically as the number of molecules.
 How many moles of N are in 0.175 g of N2O? 
Calculate the mass (in g) of O2 consumed in the complete combustion of 41.6 g sample of C4H8O. (Hint, write the balanced equation.)
To find the answer to the problem below, complete the set up by filling in the correct numbers (units in set are already provided):How many moles of CO2 will form if 5.00 mol O2 react? 2C2H6 + 7O2 → 6H2O + 4CO2 
When silver nitrate reacts with copper(II) chloride, silver chloride and copper(II) nitrate are produced. The balanced equation for this reaction is: 2AgNO3 (aq) + CuCl2 (s) → 2AgCl(s) + Cu(NO3)2(aq) If 6 moles of silver nitrate react, (a) The reaction consumes _______ moles of copper(II) chloride. (b) The reaction produces ________ moles of silver chloride and moles of copper(II) nitrate.
Consider the reaction: 2CO (g) + O2 (g) → 2CO2 (g) Given an initial mass of 17.48 g CO, an excess of O2, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of CO2 produced by the reaction.
When barium chloride reacts with potassium sulfate, barium sulfate and potassium chloride arc produced. The balanced equation for this reaction is: BaCl2 (aq) + K2SO4 (aq) → BaSO4 (s) + 2KCl (aq) If 2 moles of potassium sulfate react, The reaction consumes _______ moles of barium chloride. The reaction produces _______ moles of barium sulfate and _______ moles of potassium chloride.
Aluminum and oxygen react according to the following equation: 4Al(s) + 3O2(g) 2Al2O3(s) What mass of Al2O3, in grams, can be made by reacting 4.6 g Al with excess oxygen?a. 35b. 8.7c. 1.2d. 17e. 2.4 
What is the maximum amount in moles of P2O5 that can theoretically be made from 240 g of O2 and excess phosphorus?
According to the following reaction, bow many grains of phosphoric acid will be formed upon the complete reaction of 27.3 grams of tetraphosphorus with excess perchloric acid (HCIO4)? 12HCIO4 (aq) + P4O10 (s) → 4H3PO4 (aq) + 6CI2O7 (I) 
Consider the balanced equation: 2A + 5B <—> 3C + D (A) 8 mol A are mixed with 18 mol B at an elevated temperature. After 6 mol of A have reacted, how much B is left? (B) 0.31 mol A are mixed with 1.37 mol B at an elevated temperature. After 0.22 mol of A are left, how much B is left? (C) 0.30 mol A are mixed with 1.00 mol B at an elevated temperature. If, at the end of the reaction, 0.00 mol of A are left, how much C is produced?
According to the following reaction, how many grams of water are needed to form 25.4 grams of oxygen gas? water (l) → hydrogen (g) + oxygen (g) 
The manufacture of aluminum includes the production of cryolite (Na 3AlF6) from the following reaction: 6 HF + 3 NaAlO2 → Na3AlF6 + 3 H2O + Al2O3 How much NaAlO2 (sodium aluminate) is required to produce 2.80 kg of Na 3AlF6?
How many total atoms are in 0.420 g of P2O5?
When FeBr3 dissolves in water, how many particles are present in solution? (Number of ions per FeBr3 unit). 
How many oxygen atoms are present in 5.207 x 10-20 g of HClO4? Note, HClO4 Molar Mass: 100.46. 
Given the following balanced chemical reaction equation calculate the number of moles of Ca3(PO4)2 that can be made from 263. g of Ca(OH)2 and an unlimited amount of H3PO4. Note, Ca(OH)2 molar mass: 74.093 g/mol. 3 Ca (OH)2 + 2H3PO4 → 6H2O + Ca3(PO4)2. 
The tungsten metal used for filaments in light bulbs is made by reaction of tungsten trioxide with hydrogen: WO3 (s) + 3H2 (g) → W(s) + 3H2O(g) How many grams of tungsten trioxide must you start with to prepare 1.30 g of tungsten? (For WO3, MW = 231.8 amu.) How many grams of hydrogen must you start with to prepare 1.30 g of tungsten?
Lithium and nitrogen react to produce lithium nitride:6Li(s) + N2(g) → 2Li3N(s)How many moles of N2 are needed to react with 0.500 mol of lithium?a. 0.500b. 3.00c. 0.167d. 0.0833e. 1.50 
For the reaction N2 + 3H2 → 2NH3, how many moles of nitrogen are required to produce 14.94 mol of ammonia? a. 7.5 b. 30 c. 5.0 d. 45
Write the balanced chemical equation for the Haber-Bosch process, that is, the combination of nitrogen and hydrogen to form ammonia, NH3 Phase symbols are optional. 
How many molecules are present in 3.25 mol of C2H6O? 3.25 1.85 x 1023 46.0 1.96 x 1024 6.02 x 1023
The combustion of propane may be described by the chemical equation, C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O (g) w many grams of O2(g) are needed to completely burn 12.7 g of C3H8(g)?
When heated, KClO3 decomposes into KCl and O2. 2KClO3 → 2KCl + 3O2 If this reaction produced 70.4 g of KCl, how much O2 was produced (in grams)?