Ch.3 - Chemical ReactionsWorksheetSee 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
Additional Problems
Zinc (II) sulfide reacts with oxygen according to the reaction: 2 ZnS(s) + 3 O2(g)  → 2 ZnO(s) + 2 SO2(g) A reaction mixture initially contains 4.2 mol ZnS and 6.8 mol O2. Once the reaction has occured as completely as possible, what amount (in moles) of the excess reactant is left? A. 1.5 mol B. 0.5 mol C. 6.3 mol D. 0 mol
The limiting reagent in a particular reaction can be recognized because it is the reagent that   a) has the smallest coefficient in the balanced equation. b) has the smallest mass in the reaction mixture. c) is present in the smallest molar quantity. d) would be used up first.
Titanium metal and chlorine gas react in a combination type reaction to form titanium (IV) chloride. How many grams of titanium (IV) chloride can be formed when 3.00 g of Ti reacts with 9.50 g of Cl2? a) 11.9 b) 18.5 c) 19.7 d) 12.7 e) 3.81
For the reaction  ? Sb2S3 + ? HCl ⇌ ? SbCl 3 + ? H2S, how many grams of SbCl3 (228.1 g/mol) could be formed from 16.6 grams of Sb 2S3 (339.6 g/mol) and 12.1 grams of HCl (36.5 g/mol)? 1. 21.0 2. 23.07 3. 23.64 4. 26.14 5. 21.75 6. 19.97 7. 25.22 8. 20.18 9. 22.34 10. 22.69
Ammonia can be prepared by the Haber process, shown in this equation. N2 + 3 H2 ⇌ 2 NH3 If 2 mol of N2 and 3 mol of H2 are combined, the amount of NH 3 that would be formed if all of the limiting reactant were used up is known as the a) limited yield. b) percent yield. c) product yield. d) theoretical yield.
A “dozen” refers to a collection of 12 items. Working in a grocery store, you are asked to pack small packages, each containing 6 apples, 4 bananas, 3 peaches, and 2 pears. You have access to 30 dozen apples, 18 dozen bananas, 20 dozen peaches, and 12 dozen pears. Which one is in shortage? a. apple b. peach c. banana d. pear e. nothing left, no shortage
Determine the theoretical yield of CO 2 and the limiting reactant when 3.00 g of HCl reacts with 10.0 g of CaCO3 according to the reaction equation:   CaCO3 + 2 HCl → CaCl 2 + CO2 + H2O   a. The theoretical yield of CO 2 is 1.81 g and the limiting reactant is HCl. b. The theoretical yield of CO 2 is 3.61 g and the limiting reactant is HCl. c. The theoretical yield of CO 2 is 4.39 g and the limiting reactant is CaCO 3. d. The theoretical yield of CO 2 is 0.09 mol and the limiting reactant is CaCO 3. e. The theoretical yield of CO 2 is 0.08 mol and the limiting reactant is CaCO 3.
We cannot use the reactant in excess in a given reaction to determine the theoretical yield of a product because:   a. The reaction stops when the limiting reactant is totally consumed. b. The reaction stops when the reactant in excess is totally consumed. c. The theoretical yield is always greater than the actual yield. d. The theoretical yield is always less than the actual yield. e. This is an incorrect statement and the reactant in excess is used to determine the theoretical yield of the product.
In the chemical reaction: 2 H 2 (g) + O2 (g) → 2 H2O (g), with 8 grams of H 2 (2 grams/mole) and 16 grams of O2 (32 grams/mole) and the reaction goes to completion, what is the excess reactant and how much of that would remain?   A) 6 grams of H 2 B) 7 grams of H 2 C) 8 grams of O 2 D) 12 grams of O 2 E) 14 grams of O 2
In the combustion of C3H8O, if 5.00 g C3H8O (MW: 60.1 g/mol) combined with 9.12 g O2 (MW: 32.0 g/mol) what is the theoretical yield of aqueous product?
Consider the reaction: 2 NO(g) + 5 H 2(g) → 2 NH3(g) + 2 H2O(g) A reaction mixture initially contains 5 moles of NO and 10 moles of H 2. Which set of amounts best represents the mixture after the reactants have reacted as completely as possible?   A) 1 mol NO, 0 mol H2, 4 mol NH3, 4 mol H2O B) 0 mol NO, 0 mol H2, 4 mol NH3, 4 mol H2O C) 3 mol NO, 5 mol H2, 2 mol NH3, 2 mol H2O D) 0 mol NO, 1 mol H2, 5 mol NH3, 5 mol H2O E) 3 mol NO, 0 mol H2, 4 mol NH3, 2 mol H2O
A mixture of 34.0 g of ammonia and 40.0 g of oxygen gas reacts according to the equation 4 NH3 + 3 O2      →      2 N2 + 6 H2O Under these conditions, how many grams of H2O would be produced? a) 40.2 b) 53.6 c) 51.1 d) 45.0 e) none of the given answers is close i.e. within 5% of the correct answer
Ammonia (NH3) is prepared commercially by the reaction:  N2   +   3 H 2   →   2 NH 3  If 4.00 moles of N 2 and 8.0 moles of H 2 are mixed together and allowed to react, what is the limiting reagent and how many moles of the other reactant will remain after all of the limiting reagent has reacted?   A. N2 is the limiting reagent and 0.67 moles of H 2 will remain B. H2 is the limiting reagent and 1.0 moles of N 2 will remain C. N2 is the limiting reagent and 6.0 moles of H 2 will remain D. H2 is the limiting reagent and 1.33 moles of N 2 will remain E. H2 is the limiting reagent and 0.67 moles of N 2 will remain 
For the reaction:   ______ C6H6 + ______ O2 → ______ CO2 + ______ H2O   48.3 grams of C 6H6 are mixed with 166.2 grams of O 2 and allowed to react. How much CO 2 could be produced by this reaction?   1. 253.1 g 2. 91.4 g 3. 204 g 4. 308.6 g 5. 116.6 g 6. 342.9 g 7. 130.6 g 8. 217.2 g 9. 145.8 g  10. 182.9 g 11. 163.288 g
If you react 66.3 ml of CS2 with 156.2 g of Cl2 how many grams of CCl4 will be produced? (Note: The density of CS2 is 1.261 g/ml)   
For the reaction: CaCO3(s) + 2HCl(aq) → CaCl2(aq) + CO 2(g) + H 2O(l) 68.1 g solid CaCO3 is mixed with 51.6 g HCl. If 15 grams of CO 2 were produced, which is the limiting reagent?   a) CaCO3 b) CO2 c) both will produce only 15 g of CO 2 d) HCl e) neither will produce 15 g of CO 2 
Consider the following reaction: 3 NO2 (g) + H2O (l) → 2 HNO3 (l) + NO (g) How many moles of NO2(g) are required to react with 1.50 moles of water to produce 4.00 moles of nitric acid? a) Not enough water is available to produce 4.00 moles of nitric acid. b) 8.00 mol c) 3.00 mol d) 6.00 mol e) 1.33 mol 
If you react 66.3 ml of CS2 with 156.2 g of Cl2 how many grams of CCl4 will be produced? (Note: The density of CS2 is 1.261 g/ml)   CS2 (g) + 3 Cl2      →       (g) S2Cl2 (g) + CCl4 (g)
What is the maximum mass of CO2 which could be produced from the combustion of 2.63 g of propane with 2.79 g of O2 ? 1. 2.5829 2. 7.36912 3. 3.23482 4. 1.84022 5. 3.5484 6. 6.17256 7. 5.75171 8. 2.30233 9. 5.25658 10. 5.37211
Trinitrotoluene (TNT) is manufactured by reaction of toluene with nitric acid. C7 H8  (s) + 3 HNO3 (l) → C7 H5 N3 O6 (s) + 3 H2 O(g) Given 100 moles of each reactant, which is the limiting reactant? 1. C7 H8 2. HNO3 3. H2 O 4. C7 H5 N3 O6
If you have 5 grams of carbon and 6 grams of hydrogen and you want to make methane, what is reaction limiting? 1. hydrogen 2. None of these is limiting. 3. methane 4. carbon
Consider the reaction of hydrogen gas (H2) and nitrogen gas (N2) to make ammonia (NH3). How many moles of ammonia will be made when 3 moles of hydrogen gas react with 3 moles of nitrogen gas? (A) 2 (B) 3 (C) 5 (D) 6 (E) 8
A 15-g sample of lithium is reacted with 15 g of fluorine to form lithium fluoride: 2 Li + F2 ➔ 2 LiF After the reaction is complete, what will be present? a) 2.16 moles lithium fluoride only b) 0.789 moles lithium fluoride only c) 2.16 moles lithium fluoride and 0.395 moles fluorine d) 0.789 moles lithium fluoride and 1.37 moles lithium e) none of these answers is correct
The limiting reagent in a particular reaction can be recognized because it is the reagent that ______.  A. has the smallest coeffcient in the balanced equation B. has the smallest mass in the reaction mixture C. is present in the smallest molar quantity D. would be used up first
What mass of potassium can be produced by the reaction of 175.0 g of Na with 175.0 g of KCl? Na + KCl → NaCl + K  A. 183.5 g B. 148.4 g C. 296.7 g D. 91.78 g
A mixture of 45.2 g of PbO (molar mass 223.2 g/mol) and 35.4 g PbS ( molar mass 239.3 g/mol) are allowed to react. Identify the limiting  reagent and determine the maximum mass of lead (molar mass 207.2 g/mol) that can be obtained by the reaction. 2PbO(s) + PbS(s) → 3Pb(s) + SO2(g) A) PbS limiting; 30.65 g Pb obtained. B) PbS limiting; 91.95 g Pb obtained. C) PbO limiting; 63.0 g Pb obtained. D) PbO limiting; 42.0 g Pb obtained.
In molten salt nuclear reactors, the fuel is dissolved as fluoride compounds. One of the ideas being investigated is to use these reactors as “breeder” reactors, which make more nuclear fuel as an isotope of uranium. The uranium is produced as UF4, but a small amount of UF3 to prevent corrosion which leaches chromium from the walls of the reactor. For this reason, the properties of UF3 compound are currently being investigated (Inorg. Chem., 2011, 50, 10102–10106).  UF3 can be prepared from UF4 according to the following reaction:  3UF4 + Al → 3UF3 + AlF3 Supposed you started with 35 g of UF4 and 3.5 g of Al.  What is the limiting reagent? And what is the amount of UF3 that can be formed in grams?
In the reaction of 1.80 moles NH 3(g) and 2.00 moles O2(g) 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(l), which is the limiting reactant? 1. O2 limiting; 1.6 mol NH3 left over 2. O2 limiting; 0.4 mol NH3 left over 3. O2 limiting; 1.8 mol NH3 left over 4. NH3 limiting; 0.25 mol O2 left over 5. NH3 limiting; 2.00 mol O2 left over 6. NH3 limiting; 0.2 mol O2 left over 7. NH3 limiting; 0.4 mol O2 left over 8. O2 limiting; 0.2 mol NH3 left over
If we mix together 100.0 grams of TiCl 4 and 5.00 grams of H2, TiCl4 + 2 H2 → Ti + 4 HCl what is the maximum amount of HCl that can be produced? 1. 91 grams 2. 19 grams 3. 45 grams 4. 77 grams  5. 181 grams
Zinc (II) sulfide reacts with oxygen according to the reaction: 2 ZnS (s) + 3 O 2 (g)      →       2 ZnO (s) + 2 SO 2 (g) A reaction mixture initially contains 4.2 mol ZnS and 6.8 mol O 2. Once the reaction has occurred as completely as possible, what amount (in grams) of the excess reactant is left?  A. 5.28 g ZnS B. 7.04 g O2 C. 14.08 g O2 D. 15.84 g O2
Nitrogen (N2) and hydrogen (H2) react to form ammonia (NH3). Consider the mixture of N2 and H2 shown in the accompanying diagram. The blue spheres represent N, and the white ones represent H. How many N2 molecules are left over?
Nitrogen monoxide and oxygen react to form nitrogen dioxide. Consider the mixture of NO and O2 shown in the accompanying diagram. The blue spheres represent N, and the red ones represent O. If the actual yield of the reaction was 75% instead of 100%, how many molecules of NO would be present after the reaction was over?
Nitrogen monoxide and oxygen react to form nitrogen dioxide. Consider the mixture of NO and O2 shown in the accompanying diagram. The blue spheres represent N, and the red ones represent O. If the actual yield of the reaction was 75% instead of 100%, how many molecules of O2 would be present after the reaction was over?
When a mixture of 13.0 g of acetylene (C2H2) and 13.0 g of oxygen (O2) is ignited, the resultant combustion reaction produces CO2 and H2O.How many grams of C2 H2 are present after the reaction is complete?
When a mixture of 13.0 g of acetylene (C2H2) and 13.0 g of oxygen (O2) is ignited, the resultant combustion reaction produces CO2 and H2O.How many grams of O2 are present after the reaction is complete?
Imagine you mix 16.05 g of methane (CH4) gas and 96.00 g of oxygen (O2) gas and then ignite the mixture. After a bright flash and a loud bang, some water droplets form on the inside of the reaction vessel.Will anything be left over? What? How much?
Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 3.60 g of sodium carbonate is mixed with one containing 5.14 g of silver nitrate.How many grams of sodium carbonate are present after the reaction is complete?
Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 3.60 g of sodium carbonate is mixed with one containing 5.14 g of silver nitrate.How many grams of silver nitrate are present after the reaction is complete?
The combustion of liquid ethanol (C2 H5 OH) produces carbon dioxide and water. After 4.63 mL of ethanol (density = 0.789/ml) was allowed to burn in the presence of 15.60 g of oxygen gas, 3.73 mL of water (density = 1.00/ml) was collected.Determine the theoretical yield of H2 O for the reaction.
Nitrogen monoxide and oxygen react to form nitrogen dioxide. Consider the mixture of NO and O2 shown in the accompanying diagram. The blue spheres represent N, and the red ones represent O. How many molecules of NO2 can be formed, assuming the reaction goes to completion?
Nitrogen monoxide and oxygen react to form nitrogen dioxide. Consider the mixture of NO and O2 shown in the accompanying diagram. The blue spheres represent N, and the red ones represent O. If the actual yield of the reaction was 75% instead of 100%, how many molecules of NO2 would be present after the reaction was over?
Consider the mixture of ethanol, C2H5OH, and O2 shown in the accompanying diagram. How many molecules of CO2, H2O, C2H5OH, and O2 will be present if the reaction goes to completion?
What is the the theoretical yield?
The semiconductor gallium arsenide, GaAs, is used in highspeed integrated circuits, light-emitting diodes, and solar cells. Its density is 5.32 g/cm3. It can be made by reacting trimethylgallium, Ga(CH3)3, with arsine gas, AsH3. The other product of the reaction is methane, CH4.If you reacted 600 g of trimethylgallium with 400 g of arsine, what mass of GaAs could you make?
Nitrogen (N2) and hydrogen (H2) react to form ammonia (NH3). Consider the mixture of N2 and H2 shown in the accompanying diagram. The blue spheres represent N, and the white ones represent H. What is the limiting reactant in this case?
The combustion of liquid ethanol (C2 H5 OH) produces carbon dioxide and water. After 4.63 mL of ethanol (density = 0.789/ml) was allowed to burn in the presence of 15.60 g of oxygen gas, 3.73 mL of water (density = 1.00/ml) was collected.Determine the limiting reactant for the reaction. (Hint: Write a balanced equation for the combustion of ethanol.)
Nitrogen (N2) and hydrogen (H2) react to form ammonia (NH3). Consider the mixture of N2 and H2 shown in the accompanying diagram. The blue spheres represent N, and the white ones represent H. Are any reactant molecules left over, based on the diagram?
Nitrogen monoxide and oxygen react to form nitrogen dioxide. Consider the mixture of NO and O2 shown in the accompanying diagram. The blue spheres represent N, and the red ones represent O. What is the limiting reactant in this case?
Consider the mixture of ethanol, C2H5OH, and O2 shown in the accompanying diagram. Which reactant is the limiting reactant?
When a mixture of 13.0 g of acetylene (C2H2) and 13.0 g of oxygen (O2) is ignited, the resultant combustion reaction produces CO2 and H2O.Which is the limiting reactant?
In a chemical reaction, what is the limiting reactant?
What do we mean when we say a reactant is in excess?
Imagine you mix 16.05 g of methane (CH4) gas and 96.00 g of oxygen (O2) gas and then ignite the mixture. After a bright flash and a loud bang, some water droplets form on the inside of the reaction vessel.Identify the limiting reagent.
Imagine you mix 16.05 g of methane (CH4) gas and 96.00 g of oxygen (O2) gas and then ignite the mixture. After a bright flash and a loud bang, some water droplets form on the inside of the reaction vessel.Identify the excess reagent.
When a mixture of 13.0 g of acetylene (C2H2) and 13.0 g of oxygen (O2) is ignited, the resultant combustion reaction produces CO2 and H2O.How many grams of CO2 are present after the reaction is complete?
When a mixture of 13.0 g of acetylene (C2H2) and 13.0 g of oxygen (O2) is ignited, the resultant combustion reaction produces CO2 and H2O.How many grams of H2 O are present after the reaction is complete?
Metallic aluminum reacts with MnO2 at elevated temperatures to form manganese metal and aluminum oxide. A mixture of the two reactants is 67.2% mole percent Al.Find the theoretical yield (in grams) of manganese from the reaction of 230 g of this mixture.
A mixture of 56.0 g of S and 1.06×102 g of Cl2 reacts completely to form S2 Cl2 and SCl2.Find the mass of S2 Cl2 formed.
A mixture of 21.2 g of P and 79.2 g of Cl2 reacts completely to form PCl3 and PCl5 as the only products.Find the mass of PCl3 that forms.
Imagine you mix 16.05 g of methane (CH4) gas and 96.00 g of oxygen (O2) gas and then ignite the mixture. After a bright flash and a loud bang, some water droplets form on the inside of the reaction vessel.How many moles of water can you make?
Imagine you mix 16.05 g of methane (CH4) gas and 96.00 g of oxygen (O2) gas and then ignite the mixture. After a bright flash and a loud bang, some water droplets form on the inside of the reaction vessel.How many moles of carbon dioxide can you make?
Imagine you mix 16.05 g of methane (CH4) gas and 96.00 g of oxygen (O2) gas and then ignite the mixture. After a bright flash and a loud bang, some water droplets form on the inside of the reaction vessel.Identify the theoretical yields.
Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 3.60 g of sodium carbonate is mixed with one containing 5.14 g of silver nitrate.How many grams of silver carbonate are present after the reaction is complete?
Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 3.60 g of sodium carbonate is mixed with one containing 5.14 g of silver nitrate.How many grams of sodium nitrate are present after the reaction is complete?
When ethane (C2H6) reacts with chlorine (Cl2), the main product is C2H5Cl; but other products containing Cl, such as C2H4Cl2, are also obtained in small quantities. The formation of these other products reduces the yield of C2H5Cl.Calculate the theoretical yield of C2H5Cl when 121 g of C2H6 reacts with 226 g of Cl2, assuming that C2H6 and Cl2 react only to form C2H5Cl and HCl.
Consider the general chemical equation below: A + 2B → 3C 10.0 g of A react with 20.0 g of B. The molar mass of A is 30.0 g/mol and for B is 50.0 g/mol. Predict the limiting reactant.
Lithium hydroxide absorbs carbon dioxide forming lithium carbonate and water.2LiOH + CO2 → Li2CO3 + H2OIf a reaction vessel contains 0.15 moles of LiOH and 0.08 moles CO 2, which compound is the limiting reagent?
Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia.N2(g)+3H2(g) → 2NH3(g)Assume 4 molecules of nitrogen and 9 molecules of hydrogen are present.a. After complete reaction, how many molecules of ammonia are produced?b. How many molecules of H2 remain?c. How many molecules of N2 remain?d. What is the limiting reactant, Hydrogen or Nitrogen? 
When calcium carbonate is added to hydrochloric acid, calcium chloride, carbon dioxide, and water are produced. CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g). How many grams of calcium chloride will be produced when 28.0 g of calcium carbonate are combined with 14.0 g of hydrochloric acid?_____ g CaCl2Which reactant is in excess and how many grams of this reactant will remain after the reaction is complete?______g of CaCO3 or HCl
Aluminum reacts with oxygen gas to produce aluminum oxide, Al 2O3. Determine the mass, in grams, of aluminum needed to produce 6.58 g of aluminum oxide in excess oxygen.A) 1.74 gB) 4.74 gC) 2.37 gD) 3.48 gE) 0.87 g
NH3 + O2 → NO + H2O   (Unbalanced) If at the beginning of the reaction you used 6.89 g NH3 and 15.76 g O2, what is the theoretical yield (in grams) of NO (you will need to find the limiting reagent and then the theoretical yield of NO from this reagent)?
The octane rating of gasoline is a relationship of the burning efficiency of the given gasoline mixture to the burning efficiency of octane (C8H18). Like most hydrocarbons, octane reacts with oxygen gas to produce carbon dioxide and water.The unbalanced equation for this reaction is: C8H18 (g) + O2 (g) → CO2 (g) + H2O (g)0.310 mol of octane is allowed to react with 0.870 mol of oxygen.a. How many moles of water are produced in this reaction?b. After the reaction, how much octane is left? 
Consider this reaction used for the production of lead.2 PbO (s) + PbS (s) → 3 Pb (s) + SO2 (g)What is the maximum mass of lead that can be obtained by the reaction of 57.33 g PbO and 33.80 g of PbS?a) 43.48 gb) 72.75 gc) 79.83 gd) 87.80 g
A known amount of gaseous ammonia and gaseous oxygen were mixed in a closed container according to the following reaction:    4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (g) It was experimentally determined that oxygen was the limiting reagent and was completely used up during the course of the reaction. If you started the process with 45.37 grams of ammonia (NH3) and you have 19.27 grams of ammonia left over at the end of the reaction, how much gaseous oxygen was actually consumed during the experiment? A) 34.50 g B) 61.27 g C) 45.23 g D) 106.5 g E) 39.21 g
When FeCl3 is ignited in an atmosphere of pure oxygen, this reaction takes place.4FeCl3(s) + 3O2(g) → 2Fe2O3(s) + 6Cl2(g)If 3.00 mol of FeCl3 are ignited in the presence of 2.00 mol of O 2 gas, how much of which reagent is present in excess and therefore remains unreacted?a) 0.33 mol FeCl3 remains unreactedb) 0.67 mol FeCl3 remains unreactedc) 0.25 mol O2 remains unreactedd) 0.50 mol O2 remains unreacted
Consider the reaction:2SO2(g) + O2(g) → 2SO3(g)If 276.2 mL of SO2 is allowed to react with 172.8 mL of O 2 (both measured at STP), what is the theoretical yield of SO3?
If the reaction of 1.00 mole NH3 (g) and 1.00 mole O2 (g)4 NH3 (g) + 5 O2 (g) → 4 NO(g) + 6 H2 O(l)is carried out to completion,1. all of the O2 is consumed and 1.5 mol of NO(g) is produced.2. all of the O2 is consumed and 4.0 mol of NO(g) is produced.3. all of the O2 is consumed and 1.5 mol of H2 O is produced.4. all of the NH3 is consumed.5. 1.5 mol of H2 O is produced.6. None of the other answers is correct.7. all of the NH3 is consumed and 4.0 mol of NO(g) is produced.8. all of the NH3 is consumed and 1.5 mol of H2 O is produced.9. 4.0 mol of NO(g) is produced and 1.5 mol of H2O is produced.10. all of the O2 is consumed.
A 14.01 g sample of N2 reacts with 3.02 g of H2 to form ammonia (NH3). If ammonia is the only product, what mass of ammonia is formed?A) 17.03 gB) 1.10 gC) 14.01 gD) 3.02 gE) 23.07 g
2 Al(NO3)3 + 3 Na 2CO3 → Al2(CO3)3 + 6 NaNO3 If 2.00 grams of aluminum nitrate is reacted with 3.50 grams of sodium carbonate, what is the theoretical yield in grams of aluminum carbonate?
Aluminum sulfite reacts with sodium hydroxide to form sodium sulfite and aluminum hydroxide according to the following equation.Al2(SO3)3 + 6 NaOH → 3 Na 2SO3 + 2 Al(OH)3a) Determine the number of moles and mass of Na 2SO3 produced from 20 g of Al2(SO3)3 and 20 g of NaOH.     b) Determine the grams of excess reagent left over in the reaction.
Consider the reaction2 H2 + O2 → 2 H2O .How much water will be formed when 32 grams of hydrogen and 32 grams of oxygen are mixed and allowed to react?1. 64 g2. 36 g 3. 18 g4. 2.0 g
Aluminum sulfite reacts with sodium hydroxide to form sodium sulfite and aluminum hydroxide according to the following equation.Al2(SO3)3 + 6 NaOH → 3 Na 2SO3 + 2 Al(OH)3a) Determine the limiting reactant if 20.0 g of Al 2(SO3)3 reacts with 20.0 g of NaOH.     b) Determine the number of moles and mass of Al(OH) 3 produced. 
Lithium metal is the only member of Group 1 that reacts directly with nitrogen gas to produce a nitride according to:6 Li (s)+ N2 (g)      →       2 Li 3N(s) What mass of lithium nitride can form 48.0 g of Lithium and 7.50 x 10  23 molecules of N 2?a) 56.8b) 80.3c) 96.1d) 101e) 115
What mass of H 2 is produced when 60.0 g of aluminum reacts with excess HCl?  Al(s)    +    HCl(aq)    →    AlCl 3(aq)    +    H 2(g) A. 6.73 g          B. 12.1 g          C. 4.49 gD. 2.22 g          E. 2.99 g
Consider the mixture of ethanol, C 2H5OH, and O2. How many molecules of CO 2, H2O, C2H5OH, and O2 will be present if the reaction goes to completion?
When magnesium metal is burned in air, two products are produced. One is magnesium oxide, MgO. The other is the product of the reaction of  Mg with molecular nitrogen, magnesium nitride. When water is added to magnesium nitride, it reacts to form magnesium oxide and ammonia gas.Magnesium nitride can also be formed by reaction of the metal with ammonia at high temperature. Write a balanced equation for this reaction. If a 6.9 g Mg ribbon reacts with 2.49 g NH3 (g) and the reaction goes to completion, which component is the limiting reactant?
Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas.        2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H2(g)What mass of H2(g) is produced from the reaction of 0.75 g Al(s) with excess hydrochloric acid?a. 0.056 gb. 0.084 gc. 0.17 gd. 1.1 ge. 2.3 g 
0.240 mol of octane is allowed to react with 0.700 mol of oxygen. Which is the limiting reactant?a. Octaneb. Oxygen
How many grams of Ca(NO 3)2 can be produced by reacting excess HNO3 with 7.40 g of Ca(OH)2?a) 10.2 gb) 16.4 gc) 32.8 gd) 8.22 ge) 7.40 g
The gasoline tank of an automobile contains 83 kg of gasoline. The gasoline combines with 332.0 kg of oxygen. What is the total combined mass of the carbon dioxide and water produced by combustion in the engine?
How many grams NO and of H 2O form when 150g of NH 3 reacts with 2.75g of O 2?
Phosphine, an extremely poisonous and highly reactive gas, will react with oxygen to form tetraphosphorus decaoxide and water. PH3(g) + O2(g) → P4O10(s) + H2O(g) Calculate the mass of P4O10(s) formed when 225 g of PH3 reacts with excess oxygen.A)  1880 g           B)  940. g            C)  900. g            D)  470 g             E)  56.3 g
What is the maximum mass of S 8 that can be produced by combining 90.0 g of each reactant?8SO2 + 16H2S → 3S8 + 16H2O  
Calculate the mass of excess reagent remaining at the end of the reaction in which 90.0 g of SO2 are mixed with 100.0 g of O 2.                2 SO2 + O2 → 2 SO3A)  11.5 g            B)  22.5 g            C)  67.5 g            D)  77.5 g            E)  400 g
a) What is the molar mass of butane, C 4H10 ?    b) Calculate the mass of water produced when 8.80 g of butane reacts with excess oxygen.     c) Calculate the mass of butane needed to produce 76.2 g of carbon dioxide.
What is the limiting reactant when 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide, and how many grams of calcium oxide are produced?A)  Calcium is the limiting reactant and 47.1 g of calcium oxide are produced.B)  Oxygen is the limiting reactant and 24.4 g of calcium oxide are produced.C)  Calcium is the limiting reactant and 47.1 g of calcium dioxide are produced.D)  Oxygen is the limiting reactant and 48.7 g of calcium oxide are produced.E)  Calcium is the limiting reactant and 23.6 g of calcium oxide are produced.
For each of the given situations, indicate whether S or O 2 is the limiting reactant.a. 3 mol Sulfur, 4 mol Oxygenb. 3 mol Sulfur, 5 mol Oxygenc. 3 mol Sulfur, 3 mol Oxygen
A mixture contains only NaCl and Fe(NO 3)3. A 0.456-g sample of the mixture is dissolved in water, and an excess of NaOH is added, producing a precipitate of Fe(OH)3. The precipitate is filtered, dried, and weighed. Its mass is 0.107 g. Calculate the following. a. the mass of iron in the sample
A mixture contains only NaCl and Fe(NO 3)3. A 0.456-g sample of the mixture is dissolved in water, and an excess of NaOH is added, producing a precipitate of Fe(OH)3. The precipitate is filtered, dried, and weighed. Its mass is 0.107 g. Calculate the following. b. the mass of Fe(NO 3)3 in the sample
Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g/mol, HNO3 = 63.02 g/mol. 3 NO2 (g) + H2O (l) → 2 HNO3 (aq) + NO (g)A) 38.0 g H2OB) 26.5 g H2OC) 10.9 g H2OD) 21.7 g H2OE) 43.4 g H2O
Consider the following balanced reaction. What mass (in g) of CO 2 can be formed from 288 mg of O2? Assume that there is excess C3H7SH present. C3H7SH (l) + 6 O2 (g) → 3 CO2 (g) + SO2 (g) + 4 H2O (g)A) 0.396 g CO2B) 0.209 g CO2C) 0.126 g CO2D) 0.198 g CO2E) 0.792 g CO2
Iron metal reacts with bromine as follows: Fe(s) + Br2(g) → FeBr3(s)How many moles of FeBr3 are obtained when 4.6 mol of Br2 reacts with excess Fe?(A) 2.30 mol(B) 3.07 mol(C) 4.60 mol(D) 6.90 mol(E) 9.2 mol
How many grams of CO are needed to react with an excess of Fe  2O3 to produce 209.7g Fe?Fe2O3(s) + 3CO(g) → 3CO2(g) + 2Fe(s) 
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 + HIO3 + 5 HClA) 6.09 × 1025 molecules HClB) 2.78 × 1024 molecules HClC) 3.65 × 1024 molecules HClD) 1.67 × 1024 molecules HClE) 5.02 × 1025 molecules HCl
A mixture of 50.0 g of S and 1.00 X 10 2 g of Cl2 reacts completely to form S2CI2 and SCI2. Find the mass of S2CI2 formed. 
Balance the following chemical equation: CH4 + O2 → CO2 + H2O Given 10.0 g of CH4 and unlimited supply of O2, determine the mass (grams) of H 2O that will result from the mixture.
What is the maximum number of moles H 2 that can be produced by the reaction of 3.00 mol of Ni with 4.50 mol of HCl according to the equation: Ni + 2HCl → NiCl 2 + H2a. 4.50 molb. 2.25 molc. 9.00 mold. 3.00 mol 
What is the maximum mass of S8 that can be produced by combining 80.0 g of each reactant?8SO2 + 16H2S → 3S8 + 16H2O
Consider the following balanced reaction. What mass (in g) of CO 2 can be formed from 288 mg of O2? Assume that there is excess C3H7SH present. C3H7SH(l) + 6O2(g) → 3CO2(g) + SO2(g) + 4H2O (g)A) 0.396 g CO2B) 0.209 g CO2C) 0.198 g CO2D) 0.792 g CO2E) 0.126 g CO2
How many molecules of H2S are required to form 79.0 g of sulfur according to the following reaction? Assume excess SO2. 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(l)A) 1.48 × 1024 molecules H2SB) 2.44 × 1023 molecules H2SC) 5.06 × 1025 molecules H2SD) 3.17 × 1025 molecules H2SE) 9.89 × 1023 molecules H2S
What is the maximum mass of aluminum chloride that could be obtained from 6.00 mol of barium chloride and excess aluminum sulfate? This is the balanced equation for the reaction?Al2(SO4)3 + 3 BaCl2 → 3 BaSO4 + 2 AlCl3a) 1250 gb) 801 gc) 534 gd) 134 g
Ammonia can be formed by the following reaction.N2 + 3H2 → 2NH3If 2 mol of N2 and 3 mol of H2 are combined, the amount of NH 3 that would be formed if all of the limiting reactant were used up is known as the _____.A. limited yieldB. percent yieldC. product yieldD. theoretical yield
50g O2 is available for the combustion of 25.0 grams of C. Is this an adequate amount of O2? If so what is the excess O2, If not what is the excess C?  
The reaction between potassium chlorate and red phosphorus takes place when you strike a match on a matchbox. If you were to react 52.9 g of potassium chlorate (KClO3) with excess red phosphorus, what mass of tetraphosphorus decaoxide (P4O10) would be produced?KClO3(s) + P4(s) → P4O10(s) + KCl(s) (unbalanced)
How many moles of NH3 can be produced from 18.0 mol of H 2 and excess N2?
Aluminum oxide forms when aluminum reacts with oxygen.4Al(s) + 3O2(g) => 2Al2O3(s)If a mixture of 41.25g of aluminum and 58.83g of oxygen reacts, what mass of aluminum oxide can be formed? 
Consider the reaction of Na 2CO3 with excess of Ca(OH)2. How many formula units of NaOH will be obtained by reacting 10.5 g of Na2CO3?
Hydrogen peroxide is used as a cleaning agent in the treatment of cuts and abrasions for several reasons. It is an oxidizing agent that can directly kill many microorganisms; it decomposes upon contact with blood, releasing elemental oxygen gas (which inhibits the growth of anaerobic microorganisms); and it foams upon contact with blood, which provides a cleansing action. In the laboratory, small quantities of hydrogen peroxide can be prepared by the action of an acid on an alkaline earth metal peroxide, such as barium peroxide:BaO2(s) + 2HCl(aq) → H2O2(aq) + BaCl2(aq)What mass of hydrogen peroxide should result when 1.50 g of barium peroxide is treated with 25.0 mL of hydrochloric acid solution containing 0.0272 g of HCl per mL? What mass of which reagent is left unreacted? 
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction:     2C 6H5Cl      +    C 2HOCl3     →    C14H9Cl5    +   H2Ochlorobenzene         chloral                   DDT In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral.a. What mass of DDT is formed? 
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction:     2C 6H5Cl      +    C 2HOCl3     →    C14H9Cl5    +   H2Ochlorobenzene         chloral                   DDT In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral.b. Which reactant is limiting? Which is in excess?
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction:     2C 6H5Cl      +    C 2HOCl3     →    C14H9Cl5    +   H2Ochlorobenzene         chloral                   DDT In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral.c. What mass of the excess reactant is left over?
Magnesium nitride (Mg3N2) is formed by the reaction of magnesium metal (Mg) with nitrogen gas (N2). No other products are produced. (A) How many grams of magnesium nitride can be made in the reaction of 35.00 g of magnesium and 15.00 g of nitrogen gas? (B) How many grams of excess reactant remain after the reaction? (Be sure to identify the excess reactant!)
Consider the general chemical equation below: 3A + 2B + 5C →D If 6 moles of A react with 1 mole of B and 2 moles of C, what is the limiting reactant?  
How many molecules of carbon dioxide will be formed if 4.89 g of propane, C 3H8, is burned with excess oxygen?a. 8.83 × 1024 moleculesb. 6.68 × 1022 moleculesc. 2.67 × 1023 moleculesd. 2.00 × 1023 moleculese. 3.34 × 1023 molecules
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 Cl 2 in each container.
Sulfur and fluorine react to form sulfur hexafluoride:S(s) + 3 F2(g) → SF6(g)If 50.0 g S is allowed to react as completely as possible with 105.0 g F2(g), what mass of the excess reactant is left?
Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation:N2 (g) + 3 H 2 (g) → 2 NH 3 (g)Given a mixture of 1.00 x 10 3 g N2 and 5.00 x 10 2 g H2, what mass of which starting material would remain unreacted?
Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation:3 NO2(g) + H2O(l) → 2 HNO3(l) + NO(g)Suppose that 5 mol NO2 and 1 mol H2O combine and react completely. How many moles of the reactant in excess are present after the reaction has completed?
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction:2 C6H5Cl + C2HOCl3 → C14H9Cl5 + H2O  chlorobenzene          chloral                        DDTIn a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. What mass of the excess reactant is left over?
The following quantities are placed in a container: 1.5 × 10 24 atoms of hydrogen, 1.0 mol of sulfur, and 88.0 g of diatomic oxygen.(d) How many atoms of each remaining element would remain unreacted in the change described in (c)?
In a combination reaction, 1.62 g of lithium is mixed with 6.50 g of oxygen.After reaction, how many grams of each reactant and product are present?
Zinc sulfide reacts with oxygen according to the reaction: 2 ZnS(s) + 3 O2(g) → 2 ZnO(s) + 2 SO2(g) A reaction mixture initially contains 4.2 mol ZnS and 8.7 mol O2.Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?
In a combination reaction, 2.22 g of magnesium is heated with 3.75 g of nitrogen.After reaction, how many grams of each reactant and product are present?
Iron(II) sulfide reacts with hydrochloric acid according to the reaction:FeS(s) + 2 HCl(aq) → FeCl2(s) + H2S(g)A reaction mixture initially contains 0.226 mol FeS and 0.656 mol HCl.Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?
Iron(III) oxide reacts with carbon monoxide according to the equation:Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2 (g)A reaction mixture initially contains 22.55 g Fe2O3 and 14.00 g CO.Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?
Elemental phosphorus reacts with chlorine gas according to the equation:P4(s) + 6 Cl2(g) → 4 PCl3(l)A reaction mixture initially contains 45.53 g P4 and 131.1 g Cl2.Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?
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?(d) How many moles of excess reactant remain after the reaction in part (c)?
Calculate the maximum numbers of moles and grams of iodic acid (HIO 3) that can form when 635 g of iodine trichloridereacts with 118.5 g of water: ICl3 + H2O ⟶ICl + HIO 3 + HCl [unbalanced]How many grams of the excess reactant remain?
Calculate the maximum numbers of moles and grams of H2S that can form when 158 g of aluminum sulfide reacts with 131 g of water: Al2S3 + H2O ⟶Al(OH)3 + H2S [unbalanced]How many grams of the excess reactant remain?
When 0.100 mol of carbon is burned in a closed vessel with 8.00 g of oxygen, how many grams of carbon dioxide can form? Which reactant is in excess, and how many grams of it remain after the reaction?
Solutions of sulfuric acid and lead(II) acetate react to form solid lead(II) sulfate and a solution of acetic acid. 5.50 g of sulfuric acid and 5.50 g of lead(II) acetate are mixed.Calculate the number of grams of sulfuric acid present in the mixture after the reaction is complete.
A mixture of 0.0375 g of hydrogen and 0.0185 mol of oxygen in a closed container is sparked to initiate a reaction.How many grams of water can form? Which reactant is in excess, and how many grams of it remain after the reaction?
The semiconductor gallium arsenide, GaAs, is used in highspeed integrated circuits, light-emitting diodes, and solar cells. Its density is 5.32 g/cm3. It can be made by reacting trimethylgallium, Ga(CH3)3, with arsine gas, AsH3. The other product of the reaction is methane, CH4.Which reactant, if any, would be left over?
The semiconductor gallium arsenide, GaAs, is used in highspeed integrated circuits, light-emitting diodes, and solar cells. Its density is 5.32 g/cm3. It can be made by reacting trimethylgallium, Ga(CH3)3, with arsine gas, AsH3. The other product of the reaction is methane, CH4.How many moles of the Ga(CH3)3 would remain?
Aspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form aspirin (C9H8O4) and acetic acid (C2H4O2). The balanced equation isC4H6O3 + C7H6O3 → C9H8O4 + C2H4O2In a laboratory synthesis, a student begins with 3.00 mL of acetic anhydride (density = 1.08/ml) and 1.26 g of salicylic acid. Once the reaction is complete, the student collects 1.23 g of aspirin.Determine the theoretical yield of aspirin for the reaction.
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 50.0 g of sodium is used.
Consider the mixture of propane, C3H8, and O2 shown below.How many molecules of CO2,H2O,C3H8, and O2 will be present if the reaction goes to completion?
The reaction between potassium chlorate and red phosphorus takes place when you strike a match on a matchbox. If you were to react 52.9 g of potassium chlorate (KClO3) with excess red phosphorus, what mass of tetraphosphorus decaoxide (P4O10) could be produced?KClO3 (s) + P4 (s) → P4O10 (s) + KCl (s) (unbalanced)
Physicians who specialize in sports medicine routinely treat athletes and dancers. Ethyl chloride, a local anesthetic commonly used for simple injuries, is the product of the combination of ethylene with hydrogen chloride:C2H4(g) + HCl(g) ⟶ C2H5Cl(g) Assume that 0.100 kg of C2H4 and 0.100 kg of HCl react.How many molecules of gas (reactants plus products) are present when the reaction is complete?
Consider the following reaction:4K(s) + O2 (g) → 2K2O(s)The molar mass of K is 39.09 g/mol and that of O2 is 32.00 g/mol.Without doing any calculations, pick the conditions under which potassium is the limiting reactant
Phosphorus can be prepared from calcium phosphate by the following reaction:2 Ca 3(PO4)2 (s) + 6 SiO2 (s) + 10 C (s) → 6 CaSiO3 (s) + P4 (s) + 10 CO (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.
Coke is an impure form of carbon that is often used in the industrial production of metals from their oxides. If a sample of coke is 95% carbon by mass, determine the mass of coke needed to react completely with 1.0 ton of copper(II) oxide.2 CuO (s) + C (s) → 2 Cu (s) + CO2 (g)
Consider the following reaction: 2 NO(g) + 5 H2(g) → 2 NH3(g) + 2 H2O(g). A reaction mixture initially contains 5 moles of NO and 10 moles of H2. Without doing any calculations, determine which of the following best represents the mixture after the reactants have reacted as completely as possible.a. 1 mol NO, 0 mol H2, 4 mol NH3, 4 mol H2Ob. 0 mol NO, 1 mol H2, 5 mol NH3, 5 mol H2Oc. 3 mol NO, 5 mol H2, 2 mol NH3, 2 mol H2Od. 0 mol NO, 0 mol H2, 4 mol NH3, 4 mol H2O
Consider the following reaction: 2N2H4 (g) + N2O4 (g) → 3N2(g) + 4H2O(g) Consider the following representation of an initial mixture of N2H4 and N2O4 : Which of the following best represents the reaction mixture after the reactants have reacted as completely as possible?
Sodium and chlorine react to form sodium chloride:2 Na(s) + Cl2(g) → 2NaCl(s)What is the theoretical yield of sodium chloride for the reaction of 55.0 g Na with 67.2 g Cl2?
Consider the following reaction:4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g)If a container were to have 10 molecules of O 2 and 10 molecules of NH 3 initially, how many total molecules (reactants plus products) would be present in the container after this reaction goes to completion?
Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation:N2 (g) + 3 H 2 (g) → 2 NH 3 (g)What is the maximum mass of ammonia that can be produced from a mixture of 1.00 x 10  3 g N2 and 5.00 x 102 g H2?
Consider the following unbalanced equation:Ca3(PO4)2 (s) + H2SO4 (aq) → CaSO4 (s) + H3PO4 (aq)What masses of calcium sulfate and phosphoric acid can be produced from the reaction of 1.0 kg calcium phosphate with 1.0 kg concentrated sulfuric acid (98% H2SO4 by mass)?
Hydrogen peroxide is used as a cleansing agent in the treatment of cuts and abrasions for several reasons. It is an oxidizing agent that can directly kill many microorganisms; it decomposes on contact with blood, releasing elemental oxygen gas (which inhibits the growth of anaerobic microorganisms); and it foams on contact with blood, which provides a cleansing action. In the laboratory, small quantities of hydrogen peroxide can be prepared by the action of an acid on an alkaline earth metal peroxide, such as barium peroxide:BaO2 (s) + 2 HCl (aq) → H2O2 (aq) + BaCl2 (aq)What mass of hydrogen peroxide should result when 1.50 g barium peroxide is treated with 25.0 mL hydrochloric acid solution containing 0.0272 g HCl per mL? What mass of which reagent is left unreacted?
Silver sulfadiazine burn-treating cream creates a barrier against bacterial invasion and releases antimicrobial agents directly into the wound. If 25.0 g Ag2O is reacted with 50.0 g C10H10N4SO2, what mass of silver sulfadiazine, AgC10H9N4SO2, can be produced, assuming 100% yield?Ag2O (s) + 2 C10H10N4SO2 (s) → 2 AgC10H9N4SO2 (s) + H2O (l)
Hydrogen cyanide is produced industrially from the reaction of gaseous ammonia, oxygen, and methane:2 NH3 (g) + 3 O2 (g) + 2 CH4 (g) → 2 HCN (g) + 6 H2O (g)If 5.00 x 103 kg each of NH3, O2, and CH4 are reacted, what mass of HCN and of H 2O will be produced, assuming 100% yield?
Acrylonitrile (C3H3N) is the starting material for many synthetic carpets and fabrics. It is produced by the following reaction:2 C3H6 (g) + 2 NH 3 (g) + 3 O2 (g) → 2 C3H3N (g) + 6 H2O (g)If 15.0 g C3H6, 10.0 g O 2, and 5.00 g NH 3 are reacted, what mass of acrylonitrile can be produced, assuming 100% yield?
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction:2 C6H5Cl + C2HOCl3 → C14H9Cl5 + H2O  chlorobenzene          chloral                        DDTIn a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. What mass of DDT is formed, assuming 100% yield?
Ammonia can also be synthesized by the reaction:3H2(g) + N2(g) → 2NH3(g)What is the theoretical yield of ammonia, in kilograms, that we can synthesize from 5.39 kg of H2 and 33.5 kg of N2?
Nitrogen and hydrogen gas react to form ammonia according to the reaction:N2(g) + 3H2(g) → 2NH3(g)If a flask contains a mixture of reactants represented by the image at the far left, which image below best represents the mixture in the flask after the reactants have reacted as completely as possible?
Because H2 is completely consumed, it is the limiting reactant. Because some O2 is left over after the reaction is complete, it is the excess reactant. The amount of H2O formed depends on the amount of limiting reactant, H2. If the amount of H2 is doubled, how many moles of H2O would have formed?
The scene below represents a mixture of A2 (blue) and B2 (green) before they react to form AB.(b) How many molecules of product can form?
Consider the reaction:4 HCl(g) + O2(g) → 2 H2O(g) + 2 Cl2(g)Each molecular diagrams represents an initial mixture of the reactants.How many molecules of Cl2 would be formed from the reaction mixture that produces the greatest amount of products?
In a combination reaction, 1.62 g of lithium is mixed with 6.50 g of oxygen.How many moles of product are formed?
Consider the reaction:4 HCl(g) + O2(g) → 2 H2O(g) + 2 Cl2(g)Each molecular diagrams represents an initial mixture of the reactants.Which mixture produces the greatest amount of products?
Consider the reaction:2 CH3OH(g) + 3 O2(g) → 2 CO2(g) + 4 H2O(g)Each of the molecular diagrams represents an initial mixture of the reactants.How many CO2 molecules form from the reaction mixture that produces the greatest amount of products?
Consider the reaction:2 CH3OH(g) + 3 O2(g) → 2 CO2(g) + 4 H2O(g)Each of the molecular diagrams represents an initial mixture of the reactants.Which reaction mixture produces the greatest amount of products?
In a combination reaction, 2.22 g of magnesium is heated with 3.75 g of nitrogen.How many moles of product are formed?
For the reaction shown, compute the theoretical yield of the product (in moles) for each of the following initial amounts of reactants.Ti(s) + 2Cl2(g) → TiCl4(s)6 mol Ti, 6 mol Cl2
For the reaction shown, compute the theoretical yield of the product (in moles) for each of the following initial amounts of reactants.Ti(s) + 2Cl2(g) → TiCl4(s)8 mol Ti, 19 mol Cl2
For the reaction shown, compute the theoretical yield of the product (in moles) for each of the following initial amounts of reactants.Ti(s) + 2Cl2(g) → TiCl4(s)12.6 mol Ti, 18.8 mol Cl2
For the reactionMn(s) + O2(g) → MnO2(s)compute the theoretical yield of product (in moles) for each of the following initial amounts of reactants.5 mol Mn and 9 mol O2
For the reactionMn(s) + O2(g) → MnO2(s)compute the theoretical yield of product (in moles) for each of the following initial amounts of reactants.You may want to reference (Pages 146 - 151) Section 4.3 while completing this problem.28.0 mol Mn and 44.0 mol O2
For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants.2Al(s) + 3Cl2(g) → 2AlCl3(s)2.5 g Al, 2.5 g Cl2
For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants.2Al(s) + 3Cl2(g) → 2AlCl3(s)7.6 g Al, 25.0 g Cl2
For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants.2Al(s) + 3Cl2(g) → 2AlCl3(s)0.235 g Al, 1.15 g Cl2
For the reactionTi(s) + 2F2 → TiF4compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants.6.0 g Ti, 6.0 g F2
For the reactionTi(s) + 2F2 → TiF4compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants.0.234 g Ti, 0.289 g F2
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 O 2.(d) How many grams of CaO can be produced?
Urea (CH4N2O) is a common fertilizer that can be synthesized by the reaction of ammonia (NH3) with carbon dioxide as follows: 2NH3(aq) + CO2(aq) → CH4N2O(aq) + H2O(l). In an industrial synthesis of urea, a chemist combines 133.0 kg of ammonia with 211.4 kg of carbon dioxide and obtains 173.0 kg of urea.Determine the theoretical yield of urea
Mining companies use this reaction to obtain iron from iron ore:Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)The reaction of 182 g of Fe2O3 with 84.1 g of CO produces 73.1 g of Fe.Calculate the theoretical yield of solid iron.
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.(d) How many grams of H2 can be produced?
Methane (CH4) is the main component of marsh gas. Heating methane in the presence of sulfur produces carbon disulfide and hydrogen sulfide as the only products. Calculate the theoretical yield of carbon disulfide when 120. g of methane is reacted with an equal mass of sulfur.
A potential fuel for rockets is a combination of B 5H9 and O 2. The two react according to the following balanced equation:2 B5H9 (l) + 12 O 2 (g) → 5 B 2O3 (s) + 9 H2O (g)If one tank in a rocket holds 126 g B  5H9 and another tank holds 192 g O 2, what mass of water can be produced when the entire contents of each tank react together?
Ammonia, NH3(g), and hydrogen chloride, HCl(g), react to form solid ammonium chloride, NH4Cl(s):NH3(g) + HCl(g) → NH4Cl(s)Two 2.50 L flasks at 30.0 oC are connected by a stopcock, as shown in the drawingOne flask contains 5.60g NH3(g), and the other contains 4.60 g  HCl(g). When the stopcock is opened, the gases react until one is completely consumed.What mass of ammonium chloride will be formed?
Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. The balanced equation for the reaction is2Mg(s) + O2(g) → 2MgO(s)When 10.1 g Mg is allowed to react with 10.5 g O2, 12.0 g MgO is collected.Determine the theoretical yield for the reaction.
The semiconductor gallium arsenide, GaAs, is used in highspeed integrated circuits, light-emitting diodes, and solar cells. Its density is 5.32 g/cm3. It can be made by reacting trimethylgallium, Ga(CH3)3, with arsine gas, AsH3. The other product of the reaction is methane, CH4.One application of GaAs uses it as a thin film. If you take the mass of GaAs from part A and make a 40-nm thin film from it, what area, in cm2, would it cover? Recall that 1 nm = 1 x 10–9 m.
A 27.6-mL sample of a 1.62 M potassium chloride solution is mixed with 14.6 mL of a 0.890 M lead(II) nitrate solution and this precipitation reaction occurs:2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)The solid PbCl2 is collected, dried, and found to have a mass of 2.56 g. Determine the limiting reactant, the theoretical yield, and the percent yield.Determine the theoretical yield.
Iron reacts rapidly with chlorine gas to form a reddish-brown, ionic compound (A), which contains iron in the higher of its two common oxidation states. Strong heating decomposes compound A to compound B, another ionic compound, which contains iron in the lower of its two oxidation states. When compound A is formed by the reaction of 50.6 g of Fe and 83.8 g of Cl2 and then heated, how much compound B forms?
Aspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form aspirin (C9H8O4) and acetic acid (C2H4O2). The balanced equation isC4H6O3 + C7H6O3 → C9H8O4 + C2H4O2In a laboratory synthesis, a student begins with 3.00 mL of acetic anhydride (density = 1.08/ml) and 1.26 g of salicylic acid. Once the reaction is complete, the student collects 1.23 g of aspirin.Determine the limiting reactant for the reaction.
Is the following statement true or false? Correct any that are false.(c) A limiting-reactant problem is being stated when the available quantity of one of the reactants is given in moles.
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.Answer the following questions:a. Explain the shape of the graph.b. Calculate the mass of NaCl formed when 20.0 g of sodium is used.c. Calculate the mass of Cl2 in each container.d. Calculate the mass of NaCl formed when 50.0 g of sodium is used.e. Identify the leftover reactant, and determine its mass for parts b and d above.
Consider the mixture of propane, C3H8, and O2 shown below.Which reactant is the limiting reactant?        
Treatment of gold metal with BrF3 and KF produces Br2 and KAuF4, a salt of gold. Which is the limiting reactant when a 73.5-g mixture of equal masses of all three reactants is prepared?
When barium (Ba) reacts with sulfur (S) to form barium sulfide (BaS), each Ba atom reacts with an S atom. If 2.50 cm3 of Ba reacts with 1.75 cm3 of S, are there enough Ba atoms to react with the S atoms (d of Ba = 3.51 g/cm3; d of S = 2.07 g/cm3)?
Aspirin (C9H8O4) is synthesized by reacting salicylic acid (C7H6O3) with acetic anhydride (C4H6O3). The balanced equation isC7H6O3 + C4H6O3 → C9H8O4 + HC2H3O2a. What mass of acetic anhydride is needed to completely consume 1.00 X 102 g salicylic acid?b. What is the maximum mass of aspirin (the theoretical yield) that could be produced in this reaction?
Consider the reaction between NO (g) and O2 (g) represented below.What is the balanced equation for this reaction, and what is the limiting reactant?
Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation:3NO2(g) + H2O(l) → 2HNO3(l) + NO(g)Suppose that 4.4 mol NO2 and 0.80 mol H2O combine and react completely. Which reactant is in excess?
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction:2 C6H5Cl + C2HOCl3 → C14H9Cl5 + H2O  chlorobenzene          chloral                        DDTIn a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. Which reactant is limiting? Which is in excess?
The following quantities are placed in a container: 1.5 × 10 24 atoms of hydrogen, 1.0 mol of sulfur, and 88.0 g of diatomic oxygen.(c) If the mixture of the three elements formed a compound with molecules that contain two hydrogen atoms, one sulfur atom, and four oxygen atoms, which substance is consumed first?
What is the limiting reactant in a reaction that produces sodium chloride from 8 g of sodium and 8 g of diatomic chlorine?
Outline the steps needed to determine the limiting reactant when 30.0 g of propane, C3H8, is burned with 75.0 g of oxygen.Determine the limiting reactant.
Outline the steps needed to determine the limiting reactant when 0.50 mol of Cr and 0.75 mol of H3PO4 react according to the following chemical equation.2Cr + 2H3PO4 ⟶ 2CrPO4 + 3H2Determine the limiting reactant.
Nitrogen and hydrogen gas react to form ammonia according to the reaction:N2(g) + 3H2(g) → 2NH3(g)What is the limiting reactant?
What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following unbalanced equation?Li + N2 ⟶ Li3N
Nitrogen and hydrogen gas react to form ammonia according to the reaction:N2(g) + 3H2(g) → 2NH3(g)Which reactant is in excess?
The phosphorus pentoxide used to produce phosphoric acid for cola soft drinks is prepared by burning phosphorus in oxygen.(a) What is the limiting reactant when 0.200 mol of P4 and 0.200 mol of O2 react according to P4 + 5O2 ⟶ P4O10
Aspirin (acetylsalicylic acid, C9H8O4) is made by reacting salicylic acid (C 7H6O3) with acetic anhydride [(CH3CO)2O]: C7H6O3(s) + (CH3CO)2O(l) ⟶C9H8O4(s) + CH3COOH(l) In one preparation, 3.077 g of salicylic acid and 5.50 mL of acetic anhydride react to form 3.281 g of aspirin. (a) Which is the limiting reactant (the density of acetic anhydride is 1.080 g/mL)?
For the reaction shown, find the limiting reactant for each of the following initial amounts of reactants.2Na(s) + Br2(g) → 2NaBr(s)4 mol Na, 4 mol Br2
For the reaction shown, find the limiting reactant for each of the following initial amounts of reactants.2Na(s) + Br2(g) → 2NaBr(s)2.2 mol Na, 1.8 mol Br2
For the reaction shown, find the limiting reactant for each of the following initial amounts of reactants.2Na(s) + Br2(g) → 2NaBr(s)2.5 mol Na, 1 mol Br2
The scene below represents a mixture of A2 (blue) and B2 (green) before they react to form AB.(a) What is the limiting reactant?
For the reaction shown, find the limiting reactant for each of the following initial amounts of reactants.2Na(s) + Br2(g) → 2NaBr(s)12.1 mol Na, 6.9 mol Br2
In a combination reaction, 1.62 g of lithium is mixed with 6.50 g of oxygen.Which reactant is present in excess?
The following scene shows a mixture of nitrogen (dark blue) and hydrogen (light blue) before they react to produce ammonia,NH3. What is the limiting reactant? Draw a scene that shows the number of reactant and product molecules present after reaction.
In a combination reaction, 2.22 g of magnesium is heated with 3.75 g of nitrogen.Which reactant is present in excess?
The following scene represent a chemical reaction between AB 2 and B2:(b) What is the limiting reactant?
Sodium bicarbonate reacts with hydrochloric acid in a gas-forming reaction to produce aqueous sodium chloride, water, and carbon dioxide gas:NaHCO3(s) + HCl(aq) → NaCl(aq) + H2O(l) + CO2(g)Determine the mass of CO2 gas produced when 8.67 g of NaHCO3 is added to a solution that contains 5.65 g of HCl.
For the reactionMn(s) + O2(g) → MnO2(s)compute the theoretical yield of product (in moles) for each of the following initial amounts of reactants.5 mol Mn and 5 mol O2
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 O 2.(c) Which is the limiting reactant?
For the reactionTi(s) + 2F2 → TiF4compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants.2.5 g Ti, 1.7 g F2
Urea (CH4N2O) is a common fertilizer that can be synthesized by the reaction of ammonia (NH3) with carbon dioxide as follows: 2NH3(aq) + CO2(aq) → CH4N2O(aq) + H2O(l). In an industrial synthesis of urea, a chemist combines 133.0 kg of ammonia with 211.4 kg of carbon dioxide and obtains 173.0 kg of urea.Determine the limiting reactant.
Mining companies use this reaction to obtain iron from iron ore:Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)The reaction of 182 g of Fe2O3 with 84.1 g of CO produces 73.1 g of Fe.Identify the limiting reactant.
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.(c) Which is the limiting reactant?
The methane molecule, CH4, has the geometry shown in following figure. Imagine a hypothetical process in which the methane molecule is "expanded," by simultaneously extending all four C–H bonds to infinity. We then have the process CH4(g) → C(g) + 4 H(g)Suppose that 3.70 g CH4(g) is reacted with 1.13 g F2(g), forming CF4(g) and HF(g) as sole products. What is the limiting reagent in this reaction?
Ammonia, NH3(g), and hydrogen chloride, HCl(g), react to form solid ammonium chloride, NH4Cl(s):NH3(g) + HCl(g) → NH4Cl(s)Two 2.50 L flasks at 30.0 oC are connected by a stopcock, as shown in the drawingOne flask contains 5.60g NH3(g), and the other contains 4.60 g  HCl(g). When the stopcock is opened, the gases react until one is completely consumed.Which gas will remain in the system after the reaction is complete?
High-temperature superconducting oxides hold great promise in the utility, transportation, and computer industries. (b) Another common superconducting oxide is made by heating a mixture of barium carbonate, copper(II) oxide, and yttrium(III) oxide, followed by further heating in O2: 4BaCO3(s) + 6CuO(s) + Y2O3(s) ⟶ 2YBa2Cu3O6.5(s) + 4CO2(g) 2YBa2Cu3O6.5(s) + 1/2 O2(g) ⟶2YBa2Cu3O7(s) When equal masses of the three reactants are heated, which reactant is limiting?
For the reaction shown, find the limiting reactant for each of the following initial amounts of reactants: 4 Al(s) + 3 O2(g) → 2 Al2O3(s)a. 1 mol Al, 1 mol O2b. 4 mol Al, 2.6 mol O2c. 16 mol Al, 13 mol O2d. 7.4 mol Al, 6.5 mol O2
Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. The balanced equation for the reaction is2Mg(s) + O2(g) → 2MgO(s)When 10.1 g Mg is allowed to react with 10.5 g O2, 12.0 g MgO is collected.Determine the limiting reactant for the reaction.
Many computer chips are manufactured from silicon, which occurs in nature as SiO2. When SiO2 is heated to melting, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 155.9 kg of SiO2 is allowed to react with 78.4 kg of carbon to produce 66.2 kg of silicon.Determine the limiting reactant for the reaction.
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.Explain the shape of the graph.
The combustion of octane (C 8H18) in oxygen proceeds as follows 2C8H18(g) + 25O2(g) → 16CO2 (g) + 18 H2O(l) How many moles of CO2 are produced when 5.0 moles of octane, C 8H18, is burned in 5.0 moles of oxygen?
For the reaction shown below, what is the chemical formula for the limiting reactant? Write the balanced chemical equation for the reaction, using lowest whole-number coefficients.
Cyanogen, (CN)2, has been observed in the atmosphere of Titan, Saturn’s largest moon, and in the gases of interstellar nebulas.On Earth, it is used as a welding gas and a fumigant. In its reaction with fluorine gas, carbon tetrafluoride and nitrogen trifluoride gases are produced. What mass (g) of carbon tetrafluoride forms when 60.0 g of each reactant is used?
Sulfur dioxide gas reacts with sodium hydroxide to form sodium sulfite and water. The unbalanced chemical equation for this reaction is given below:SO2 (g) + NaOH (s) → Na2SO3 (s) + H2O (l)Assuming you react 38.3 g sulfur dioxide with 32.8 g sodium hydroxide and assuming that the reaction goes to completion, calculate the mass of each product formed.
An intermediate step in the production of nitric acid involves the reaction of ammonia with oxygen gas to form nitrogen monoxide and water. How many grams of nitrogen monoxide can form in the reaction of 485 g of ammonia with 792 g of oxygen?
When magnesium metal is burned in air, two products are produced. One is magnesium oxide, MgO. The other is the product of the reaction of Mg with molecular nitrogen, magnesium nitride. When water is added to magnesium nitride, it reacts to form magnesium oxide and ammonia gas.Magnesium nitride can also be formed by reaction of the metal with ammonia at high temperature. Write a balanced equation for this reaction. If a 6.3-g Mg ribbon reacts with 2.57 g NH3(g) and the reaction goes to completion, what mass of H2(g) is formed in the reaction?
Many computer chips are manufactured from silicon, which occurs in nature as SiO2. When SiO2 is heated to melting, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 155.9 kg of SiO2 is allowed to react with 78.4 kg of carbon to produce 66.2 kg of silicon.Determine the theoretical yield for the reaction.
Aluminum nitrite and ammonium chloride react to form aluminum chloride, nitrogen, and water. How many grams of each substance are present after 72.5 g of aluminum nitrite and 58.6 g of ammonium chloride react completely?
Calcium nitrate and ammonium fluoride react to form calcium fluoride, dinitrogen monoxide, and water vapor. How many grams of each substance are present after 16.8 g of calcium nitrate and 17.50 g of ammonium fluoride react completely?
Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas.2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2(g)What mass of H2(g) is required from the reaction of 0.75 g of Al(s) with excess hydrochloric acid?
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation3H2(g)+N2(g) → 2NH3(g) Use molar masses expressed to five significant figures throughout.a. How many moles of NH3 can be produced from 12.0mol of H2 and excess N2?Express your answer numerically in moles.b. How many grams of NH3 can be produced from 4.10mol of N2 and excess H2. Express your answer numerically in grams.c. How many grams of H2 are needed to produce 11.35g of NH3? Express your answer numerically in grams. 
In the combustion of hydrogen gas, hydrogen reacts with oxygen from the air to form water vapor. If you burn 33.5 g of hydrogen and produce 299 g of water, how much oxygen in grams reacted?hydrogen + oxygen → water
What is the maximum mass of S that can be produced by combining 92.0 g of each reactant?8SO2 + 16H2S <--> 3S8 + 16H20
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.
3H2(g) + N2(g) → 2NH3(g)How many moles of NH3 can be produced from 24.0 mol of H 2 and excess N2?
2C8H18 + 25O2 → 16CO2 + 18H2O0.660 mol of octane is allowed to react with .780 mol of oxygen. Oxygen is the limiting reactant. After the reaction, how much octane is left?
AgNO3 (aq) + KCl (aq) → KNO3 (aq) + AgCl (s) Given the above reaction equation, if 0.50 moles of AgNO3 and 0.25 moles of KCI react together, what is the theoretical yield (in grams) of AgCI (molar mass of 143.3 grams/mole)? (a) 35.8 grams (b) 71.7 grams (c) 573.2 grams (d) 286.6 grams
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H2O that can be produced by combining 82.3 g of each reactant? 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)
When calcium carbonate is added to hydrochloric acid, calcium chloride, carbon dioxide, and water produced. CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g)How many grams of calcium chloride wll be produced when 28.0 g of calcium carbonate are combined with 11.0 g of hydrochloric acid? Which reactant is in excess and how many grams of this reactant will remain after the reaction is complete? 
A reaction vessel contains 7.70 g of CO and 7.70 g of O2. How many grams of CO2 could be produced according to the following reaction? 2CO + O2 → 2CO2
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H 2O that can be produced by combining 75.9 g of each reactant? 4NH3(g) + 5O2(g) → 4NO(g) + 6H 2O(g)
An intermediate step in the industrial production of nitric acid involves the reaction of ammonia with oxygen gas to form nitrogen monoxide and water. How many grams of nitrogen monoxide can form by the reaction of 538 g of ammonia and 993 g of oxygen?
Identify limiting reactants (mole ratio method). Identify the limiting reactant in the reaction of nitrogen and oxygen to form NO, if 8.35 g of N2 and 5.02 g of O2 are combined. Determine the amount (in grams) of excess reactant that remains after the reaction is complete. Formula of limiting reactant = Amount of excess reactant remaining = 
Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia.N2 (g) + 3H2 (g) → 2NH3 (g) Assume 0.250 mol of N2 and 0.805 mol of H2 are present initially. After complete reaction, how many moles of ammonia are produced? How many moles of H2 remain? How many moles of N2 remain? What is the limiting reactant?
Liquid hexane (CH3(CH2)4CH3) reacts with gaseous oxygen gas (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). What is the theoretical yield of water formed from the reaction of 7.76 g of hexane and 17.2 g of oxygen gas? Be sure your answer has the correct number of significant digits in it.
Combining 0.326 mol of Fe2O3 with excess carbon produced 13.7 g of Fe. Fe2O3 + 3C → 2Fe + 3CO What is the actual yield of iron in moles? What was the theoretical yield of iron in moles? What was the percent yield?
Be sure to answer all parts. Metal hydrides react with water to form hydrogen gas and metal hydroxide. For example, SrH2(s) + 2H2O(l) → Sr(OH)2(s) + 2H2(g) You wish to calculate the mass of hydrogen gas that can be prepared from 4.02 g of SrH2 and 3.35 g of H2O. (a) How many moles of H2 can be produced from the given mass of SrH2? (b) How many moles of H2 can be produced from the given mass of H2O? (c) Which is the limiting reactant?                           • H2O                           • SrH2 (d) How many grams of H2 can be produced?
Aqueous sulfuric acid (H2SO4) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium sulfate (Na2SO4) and liquid water (H2O). What is the theoretical yield of water formed from the reaction of 7.8 g of sulfuric acid and 3.7 g of sodium hydroxide? Be sure your answer has the correct number of significant digits in it.
For the following reaction, 0.446 moles of carbon dioxide are mixed with 0.252 moles of potassium hydroxide.carbon dioxide (g) + potassium hydroxide (aq) → potassium carbonate (aq) + water (l) What is the FORMULA for the limiting reagent? What is the maximum amount of potassium carbonate that can be produced?
Gaseous methane (CH 4) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). Suppose 15. g of methane is mixed with 100. g of oxygen. Calculate the maximum mass of water that could be produced by the chemical reaction. Round your answer to 2 significant digits.
What is the maximum mass of S 8 that can be produced by combining 86.0 g of each reactant? 8SO2 + 16H2S → 3S8 + 16H2O
Be sure to answer all parts. Calculate the maximum numbers of moles and grams of H2S that can form when 138.7 g of aluminum sulfide reacts with 143.0 g of water: Al2S3 + H2O → Al(OH)3 + H2S [unbalanced] What mass of the excess reactant remains? 
Metal hydrides react with water to form hydrogen gas and metal hydroxide. For example, SrH2 (s) + 2H2O (l) → Sr(OH)2 (s) + 2H2 (g) You wish to calculate the mass of hydrogen gas that can be prepared from 7.27 g of SrH  2  and 6.06 g of H2O. (a) How many moles of H2 can be produced from the given mass of SrH 2? (b) How many moles of H2 can be produced from the given mass of H 2O?  (c) Which is the limiting reactant? (d) How many grams of H2 can be produced? 
Aqueous sulfuric acid (H2SO4) will react with solid sodium hydroxide (NaOH) to produce aqueous sodium sulfate (Na2SO4) and liquid water (H2O). Suppose 93 g of sulfuric acid is mixed with 128 g of sodium hydroxide. Calculate the maximum mass of water that could be produced by the chemical reaction. Round your answer to 2 significant digits.
Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia. N2 (g) + 3H2 (g) → 2NH3 (g) Assume 0.230 mol of N2 and 0.741 mol of H2 are present initially. a) After complete reaction, how many moles of ammonia are produced?b) How many moles of H2 remain? c) How many moles of N2 remain? d) What is the limiting reactant?
If 1176 grams of FeS2 is allowed to react with 704 grams of O2 according to the following equation, how many grams of Fe2O3 are produced?FeS2 + O2 → Fe2O3 + SO2
Be sure to answer all parts. A mixture of 0.0723 g of hydrogen and 0.0358 mol of oxygen in a closed container is sparked to initiate a reaction.How many grams of water can form? Which reactant is in excess, and how many grams of it remain after the reaction?                                 (i) oxygen                                 (ii) hydrogen 
When calcium carbonate is added to hydrochloric acid, calcium chloride, carbon dioxide, and water are produced.CaCO3 (s) + 2HCl (aq) → CaCI2 (aq) + H2O (l) + CO2 (g) How many grams of calcium chloride will be produced when 29.0 g of calcium carbonate are combined with 11.0 g of hydrochloric acid? Which reactant is in excess and how many grams of this reactant will remain after the reaction is complete?
Liquid octane (CH3(CH2)6CH3) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). Suppose 2.28 g of octane is mixed with 4.5 g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Round your answer to 2 significant digits.
What is the maximum mass of S8 that can be produced by combining 86.0 g of each reactant? 8SO2 + 16H2S → 3S8 + 16H2O 
For the following reaction, 5.67 grams of carbon (graphite) are mixed with excess oxygen gas. The reaction yields 19.4 grams of carbon dioxide. carbon (graphite) (s) + oxygen (g) → carbon dioxide (g) What is the theoretical yield of carbon dioxide? What is the percent yield for this reaction? 
Nitrogen monoxide is produced by combustion in an automobile engine. For the following reaction, 0.250 moles of nitrogen monoxide are mixed with 0.514 moles of oxygen gas nitrogen monoxide (g) + oxygen (g) → nitrogen dioxide (g) What is the FORMULA for the limiting regent? What is the maximum amount of nitrogen dioxide that can be formed?
If a solution containing 41.17 g of mercury(II) nitrate is allowed to react completely with a solution containing 7.410 g of sodium sulfide, how many grams of solid precipitate will be formed?How many grams of the reactant in excess will remain after the reaction?
For the following reaction, 0.180 moles of carbon monoxide are mixed with 0.352 moles of oxygen gas. carbon monoxide (g) + oxygen (g) → carbon dioxide (g) What is the formula for the limiting reagent? What is the maximum amount of carbon dioxide that can be produced?
For the following reaction, 17.4 grams of iron are allowed to react with 8.61 grams of oxygen gas.iron (s) + oxygen (g) → iron (II) oxide(s) What is the maximum mass of iron(II) oxide that can be formed? What is the FORMULA for the limiting reagent? What mass of the excess reagent remains after the reaction is complete? 
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce niítric oxide and water What is the maximum mass of H2O that can be produced by combining 57.9 g of each reactant?4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (g) 
Iron(II) sulfide reacts with hydrochloric acid according to the reaction FeS (s) + 2HCl (aq) → FeCl2 (s) + H2S (g) A reaction mixture initially contains 0.223 mol FeS and 0.665 mol HCl. Part A Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?Express your answer to three significant figures.
For the following reaction, 20.1 grams of iron are allowed to react with 42.3 grams of chlorine gas.iron (s) + chlorine (g) → iron(III) chloride(s) What is the maximum mass of iron(III) chloride that can be formed? What is the FORMULA for the limiting reagent? What mass of the excess reagent remains after the reaction is complete? 
For the following reaction, 20.1 grams of iron are allowed to react with 42.3 grams of chlorine gas.iron (s) + chlorine (g) → iron(III) chloride (s) What is the maximum amount of iron(III) chloride that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? 
For the following reaction, 5.41 grams of hydrogen gas are allowed to react with 10.4 grams of ethylene (C2H4).hydrogen (g) + ethylene (C2H4) (g) → ethane (C2H6) (g)What is the maximum amount of ethane (C2H6) that can be formed?What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete?
SO2 reacts with H2S as follows: 2H2S + SO2 → 3S + 2H2O When 7.50 g of H2S reacts with 12.75 g of SO2, which statement applies? A) 6.38 g of sulfur are formedB) 10.6 g of sulfur are formedC) 0.0216 moles of H2S remainD) 1.13 g of H2S remainE) SO2 is the limiting reagent
Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide.4HCl(aq) + MnO2(s) → MnCl2(aq) + 2H2O(l) + Cl2(g) You add 35.5 g of MnO2 to a solution containing 42.5 g of HCI. (a) What is the limiting reactant?  (b) What is the theoretical yield of Cl 2 in grams? (c) If the yield of the reaction is 71.1%, what is the actual yield (grams) of chlorine?
For the following reaction, 16.5 grams of chlorine gas are allowed to react with 7.40 grams of water. chlorine (g) + water (l) → hydrochloric acid (aq) + chloric acid (HCIO3) (aq) What is the maximum amount of hydrochloric acid that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete?
For the following reaction, 60.6 grams of silver nitrate are allowed to react with 22.7 grams of copper(II) chloride.silver nitrate( aq) + copper(II) chloride (s) → silver chloride (s) + copper(II) nitrate( aq) What is the maximum amount of silver chloride that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? 
The reaction of Cr2O3 with silicon metal at high temperatures will make chromium metal. 2Cr2O3 (s) +3Si(s) → 4Cr(l) + 3SiO2 (s) The reaction is begun with 182.00 g of Si and 140.00 g of Cr 2O3. How many grams of the excess reactant are left after the reaction is complete? 
Consider this reaction 2H2 + O2 → 2H2O If 5.91 grams of hydrogen (H2) reacts with 74.22 grams of oxygen (O2), how many grams of the excess reactant remain? Use precise masses from the periodic table (all digits) and round your answer at the end of your calculations to two decimal places. 
Consider the reaction between HCl and O2: 4HCl (g) + O2 (g) → 2H2O (l) + 2Cl2 (g) When 63.1 g of HCl are allowed to react with 17.2 g of O2, 56.5 g of Cl2 are collected. Part ADetermine the limiting reactant for the reaction. Express your answer as a chemical formula. Part BDetermine the theoretical yield of Cl2 for the reaction.
When 0.2250 g of magnesium is heated with 0.5331 g of nitrogen in a closed container, the magnesium is completely converted to 0.3114 g of magnesium nitride. What mass of unreacted nitrogen must remain?
For the following reaction, 0.266 moles of hydrogen gas are mixed with 0.452 moles of iodine. hydrogen (g) + iodine (s) → hydrogen iodide (g) What is the formula for the limiting reagent? What is the maximum amount of hydrogen iodide that can be produced? 
Na2SO3 reacts with HCIO4 according to the reaction Na2SO3(aq) + 2HCIO4(aq) → 2NaClO4(aq) + H2O(l) + SO2(g) You wish to provide a 50% excess of 4.61 wt% aqueous HCIO4 to react with 50.0 mL of 0.0732 M Na2SO3. Calculate the mass of the 4.61 wt% aqueous HCIO4 solution required to provide the 50% excess.
Consider the following reaction between sulfur trioxide and water: SO3 (g) + H2O (l) → H2SO4 (aq) A chemist allows 61.5 g of SO3 and 11.2 g of H2O to react When the reaction is finished: the chemist collects 54.4 g of H2SO4. Part ADetermine the limiting reactant for the reaction. Express your answer as a chemical formula. Part BDetermine the theoretical yield for the reaction.
Identify limiting reactants (maximum product method). Consider the reaction of ruthenium(III) iodide with carbon dioxide and silver. RuI3 (s) + 5CO (g) + 3Ag (s) → Ru(CO)5 (s) + 3AgI (s) Determine the limiting reactant in a mixture containing 114 g of RuI3, 38.6 g of CO, and 114 g of Ag. Calculate the maximum mass (in grams) of ruthenium pentacarbonyl, Ru(CO)5, that can he produced in the reaction. The limiting reactant is: (a) CO (b) Ag (c) RuI3 Amount of Ru(CO)5 formed - 
A sealed chamber contains 6.00 g CH4 and 13.00 g O2. The mixture is ignited. How many grams of CO2 are produced?
For the following reaction, 29.0 grams of hydrochloric acid are allowed to react with 59.3 grams of barium hydroxide.hydrochloric acid (aq) + barium hydroxide (aq) → barium chloride (aq) + water (l) What is the maximum amount of barium chloride that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete?
A reaction vessel contains 6.3 g of CO and 6.3 g of O 2. How many grams of CO 2 could be produced according to the following reaction? 2CO + O2 → 2CO2
For the following reaction, 0.182 moles of aluminum oxide are mixed with 0.268 moles of sulfuric acid. aluminum oxide (s) + sulfuric acid (aq) → aluminum sulfate (aq) + water(l) What is the formula for the limiting reagent? What is the maximum amount of aluminum sulfate that can be produced?
For the following reaction, 0.486 moles of calcium hydroxide are mixed with 0.285 moles of hydrochloric acid.calcium hydroxide(aq) + hydrochloric acid(aq) → calcium chloride(aq) + water(l) What is the FORMULA for the limiting reagent? What is the maximum amount of calcium chloride that can be produced?
If a solution containing 22.34 g of mercury(lI) acetate is allowed to react completely with a solution containing 6.256 g of sodium dichromate, how many grams of solid precipitate will be formed? How many grams of the reactant in excess will remain after the reaction? 
The following reaction is unbalanced. HF + SiO2 → H2SiF6 + H2O Write the balanced reaction in the space below. How much H2SiF6 can be produced from 3.00 moles of HF? If 3.00 moles of HF reacts with SiO2, and 1.50 moles of SiO2 were initially present, what is the fractional excess of SiO2? What is the percent excess of SiO2?
For the following reaction, 25.2 grams of calcium hydroxide are allowed to react with 28.9 grams of hydrochloric acid. calcium hydroxide (aq) + hydrochloric acid (aq) → calcium chloride (aq) + water (l) What is the maximum amount of calcium chloride that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete?
Gaseous methane (CH4) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). Suppose 0.48 g of methane is mixed with 0.518 g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Round your answer to 3 significant digits.
For the following reaction, 3.67 grams of hydrogen gas are allowed to react with 43.9 grams of iodine. hydrogen (g) + iodine (s) → hydrogen iodide (g)What is the maximum amount of hydrogen iodide that can be formed?What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? 
The reaction of Cr2O3 with silicon metal at high temperatures will make chromium metal.2Cr2O3(s) + 3Si(s) → 4Cr(l) + 3SiO2(s) The reaction is begun with 107.00 g of Si and 149.00 g of Cr2O3. Part 1 (1 point) Select the limiting reactant. Choose one or more: (i) Cr (ii) Cr2O3(iii) SiO2 (iv) SiPart 2 (1 point) How many grams of the excess reactants are left after the reaction is completed?
Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s) + 3Cl2(g) → 2AlCl3(s) What is the maximum mass of aluminum chloride that can be formed when reacting 11.0 g of aluminum with 16.0 g of chlorine?
Mining companies use this reaction to obtain iron from iron ore: Fe2O3 (s) + 3CO (g) → 2Fe (s) + 3CO2 (g) The reaction of 182 g of Fe2O3 with 83.4 g of CO produces 72.5 g of Fe. Identify the limiting reactant. (i) Fe2O3 (ii) CO
Assume that you have 1.44 mol of H2 and 3.45 mol of N2. How many grams of ammonia (NH3) can you make, and how many grams of which reactant will be left over? 3H2 + N2 → 2NH3mNH3 = mH2 = mN2  =
Balance the following combustion reaction in order to answer the following questions. Use lowest whole-number coefficients C2H4 + O2 → CO2 + H2O Tip: If you need to clear your work and reset the equation, click the button that looks like two red arrows. You are given 9.5 moles of O2 to react with 145 g C2H4. Upon completion of the reaction, will there be any remaining C2H4?a. Yes, there will still be C2H4 remaining. b. No, all C2H4 will be used up in the reaction. 
For the following reaction, 0.340 moles of sodium chloride are mixed with 0.446 moles of silver nitrate.sodium chloride(aq) + silver nitrate(aq) → silver chloride(s) + sodium nitrate(aq) What is the FORMULA for the limiting reagent? What is the maximum amount of silver chloride that can be produced?
Under certain conditions, the substances iron and chlorine combine to form iron(III) chloride. If 25.4 grams of iron and 48.4 grams of chlorine combine to form iron(III) chloride, how many grams of iron(III) chloride must form? 
For the following reaction, 28.5 grams of hydrochloric acid are allowed to react with 70.9 grams of barium hydroxide.hydrochloric acid (aq) + barium hydroxide (aq) → barium chloride (aq) + water (l) What is the maximum amount of barium chloride that can be formed?What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete?
Cryolite, Na3AIF6 (s), an ore used in the production of aluminum, can be synthesized using aluminum oxide. Balance the equation.Al2O3 (s) + 6 NaOH(l) + 12 HF(g) → 2 Na3AlF6 + 9 H2O(g) If 13.9 kilograms of Al2O3 (s), 50.4 kilograms of NaOH(l), and 50.4 kilograms of HF(g) react completely, how many kilograms of cryolite will be produced?Which reactants will be in excess? What is the total mass of the excess reactants left over after the reaction is complete?
When 1.00 mol sodium chloride reacts with 0.500 mol silver nitrate, sodium chloride is the limiting reagent. a. True b. False
Aluminum and oxygen react to form aluminum oxide. 4 Al + 3 O2 -->2 Al2O3a. What is the limiting reactant if 15.0 g Al are reacted with 15.0 g of O2?b. What is the theoretical yield of Al2O3, in grams?c. If 8.8 g of Al2O3 are obtained, what is the percent yield?
What is the maximum mass of S8 that can be produced by combining 84.0 g of each reactant? 8SO2 + 16H2S → 3S8 + 16H2O
What mass of PCl 5 will be produced from the given masses of both reactants? 28.0 g of P4 and 59.0 g of Cl2,
The Ba3(PO4)2 (molar mass = 601.93 g/mol) precipitate that formed from a salt mixture has a mass of 0.667 g. Experimental tests revealed that Na3PO4 • 12H2O (molar mass = 380.12 g/mol) was the limiting reactant in the formation of the precipitate and the BaCl2 • 2H2O was the excess reactant in the salt mixture. Determine the mass of Na3PO4 • 12H2O in the salt mixture.