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
When 1.187 of a metallic oxide is reduced with excess hydrogen, 1.054 g of the metal is produced. What is the metallic oxide? a) Ag2O b) Cu2O c) K2O d)TI2O
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)
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 ?
How many grams of Cr are found in 1.00 × 10  2 g of K 2Cr2O7? A) 33.8 g       B) 24.3 g       C) 12.2 g       D) 48.6 g       E) 35.4 g
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.
Determine the mass of oxygen in a 7.2 g sample of Al 2(SO4)3.
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
Silver chloride, often used in silver plating, contains 75.27% Ag. Calculate the mass of silver chloride in grams required to make 6.0 g of silver plating.
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
You drank 100.0 g of water. This quantity of water contains hydrogen that is equivalent to (x) moles of hydrogen (H2).
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
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.    
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.
Consider the general chemical equation: 2A + B → 3C. Assume that you start with 100.0 g of substance A and you eventually isolate 500g of substance C. If you know that the molar mass of A is 20 g mol-1 and the molar mass of C is 72 g mol -1, find the actual yield, the theoretical yield and the % yield of the reaction that is represented by the above general chemical equation.
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
How many grams of chlorine are there in 22.7 g of zinc chloride?A) 5.90 gB) 0.17 gC) 10.9 gD) 14.7 gE) 11.81 g
Sodium and nitrogen combine to form sodium nitride;6Na(s)+N2(g) → 2Na3N(s)a) if 80.0 g of sodium is mixed with 20.0 g of nitrogen gas, what mass sodium nitride forms?b) If the reaction in part "a)" has a percent yield 75.0%, how much sodium nitride is actually produced?
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. 
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?
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
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?
 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] 
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
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.
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).
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)
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? 
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 =
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) 
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.
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)
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)
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? 
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
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
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.
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
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?
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
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
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)?
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?
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 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? 
How many atoms of iron are there in 2.20 moles of each of the following?
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)  
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
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? 
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) 
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