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Unit 5 Test Review 1. Consider the following balanced chemical equation: 2 Na + Cl2 2 NaCl How many molecules of NaCl will be produced from the reaction of 36 molecules of Cl2? a. 9 b. 18 c. 36 d. 72 e. 144 2. Consider the following balanced chemical equation: C5H12(l) + 8 O2(g) 5 CO2(g) + 6 H2O(g) How many moles of CO2 will be produced from the reaction of 31.6 moles of C5H12? a. 5.27 b. 6.32 c. 31.6 d. 158 e. 190 3. Consider the following balanced chemical equation: 2 Al + 3 CuCl2 2 AlCl3 + 3 Cu How many atoms of Cu will be produced from the reaction of 12 atoms of Al? a. 6 b. 8 c. 12 d. 18 4. e. 36 Consider the following unbalanced chemical equation: Al + O2 Al2O3 How many molecules of Al2O3 will be produced from the reaction of 6 atoms of Al? a. 2 b. 3 c. 6 d. 12 e. 18 5. Determine the number of molecules of H2O that can be produced by the combustion of 2 molecules of methane (CH4)? a. 1 b. 2 c. 3 d. 4 e. 8 6. Consider the synthesis of aluminum oxide from its elements. How many molecules of aluminum oxide are produced by the reaction of 24 atoms of aluminum? a. 6 b. 12 c. 16 d. 36 e. 48 7. Consider the following reaction. 4 Al + 3 O2 2 Al2O3 Pick two conversion factors that would be needed in order to determine the mass of Al that must react to produce 19.3 mole of Al2O3. Bubble in two answers. a. 8. b. c. d. e. Consider the following reaction. 4 Al + 3 O2 2 Al2O3 Pick two conversion factors that would be needed in order to determine the moles of Al that must react to produce 276 grams of Al2O3. Bubble in two answers. a. 9. b. c. d. e. Which method is correct for determining the mass of carbon dioxide that can be made by the combustion of 3.219 grams of ethanol with excess oxygen? C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l) a. b. c. d. e. 10. Suppose that a student wishes to solve a problem involving the determination of the mass of product produced if a given amount of moles of reactant was reacted. Which quantities would be essential in order to solve such a problem? Bubble in all that apply - but only those that are essential to this calculation. a. The molar mass of the reactant b. The molar mass of the product c. The coefficients of the balanced chemical equation d. The density of the reactant e. The density of the product 11. Which of the following statements best describes what a limiting reactant is for any given reaction? a. It is the reactant that is used up first while other reactants remain. b. It is the reactant that has the highest coefficient in the balanced chemical equation. c. It is the reactant that has the lowest coefficient in the balanced chemical equation. d. It is the reactant that is available with the least amount of mass. 12. The combustion of methane occurs according to the reaction CH4 + 2 O2 CO2 + 2 H2O Methane and oxygen are combined in a reaction vessel in amounts of 16 grams and 32 grams respectively. What amounts of reactants and products will be present in the reaction vessel once the reaction is complete? a. 0 grams CH4, 0 grams of O2, 44 grams of CO2, 36 grams of H2O b. 8 grams CH4, 0 grams of O2, 22 grams of CO2, 18 grams of H2O c. 0 grams CH4, 0 grams of O2, 44 grams of CO2, 18 grams of H2O d. 8 grams CH4, 0 grams of O2, 22 grams of CO2, 9 grams of H2O e. 0 grams CH4, 16 grams of O2, 22 grams of CO2, 10 grams of H2O 13. Consider the reaction for the combustion of benzene (C6H6). 2 C6H6 + 15 O2 ==> 12 CO2 + 6 H2O Suppose that 4 moles of benzene are mixed with 15 moles of oxygen. What amounts of reactants and products will be present in the reaction vessel once the reaction is complete? a. 0 moles C6H6, 15 moles of O2, 24 moles of CO2, 12 moles of H2O b. 0 moles C6H6, 15 moles of O2, 12 moles of CO2, 6 moles of H2O c. 2 moles C6H6, 0 moles of O2, 24 moles of CO2, 12 moles of H2O d. 2 moles C6H6, 0 moles of O2, 12 moles of CO2, 6 moles of H2O e. 2 moles C6H6, 15 moles of O2, 12 moles of CO2, 6 moles of H2O 14. Consider the reaction for the combustion of methane (CH4). CH4 + 2 O2 CO2 + 2 H2O Suppose that 4 moles of benzene are mixed with 10 moles of oxygen. Which one of the following statements is true? a. Methane is the limiting reactant and there is an excess of 1 mole of oxygen. b. Methane is the limiting reactant and there is an excess of 2 moles of oxygen. c. Oxygen is the limiting reactant and there is an excess of 1 moles of methane. d. Oxygen is the limiting reactant and there is an excess of 2 moles of methane. e. None of these statements are correct. 15. Nitrogen reacts with hydrogen to produce ammonia (NH3). In a certain reaction, a chemist found that 235 g of ammonia were produced. What other piece of information would be required to determine the percent yield? a. the density of ammonia b. the volume of ammonia c. the theoretical yield of ammonia d. the mass of excess reactant remaining 16. A lab group performs a four-step copper cycle lab. They begin with 0.31 grams of Cu. In the final step of the cycle, they produce 0.23 g of Cu. What percent yield has this lab group obtained? a. 26% b. 30.% c. 35% d. 74% e. 87% Two students perform a lab in order to experimentally determine the mole ratio of silver to copper in a single replacement reaction between copper and silver nitrate. A copper wire is massed and placed in a 100 mL beaker with a known amount of silver(I) nitrate. Once the reaction is complete, the mass of the silver product and the unreacted copper is determined. The following data was collected: 17. Experimental Data Mass of Cu Wire Before Reaction Mass of Empty 100 mL Beaker Mass of 100 mL Beaker + AgNO3 Mass of Empty 50 mL Beaker Mass of 50 mL Beaker + Ag Mass of Cu Wire After Reaction 1.86 g 52.85 g 59.08 g 31.92 g 35.74 g 0.71 g Determine the mass and the number of moles of copper that reacted in this experiment, accurate to three significant figures. PSYW Mass = 1.15 g Moles = 0.0181 mol 18. Determine the mass and the number of moles of silver produced by this reaction, accurate to three significant figures. PSYW Mass = 3.82 g Moles = 0.0354 mol 19. Determine the experimental mole ratio of silver to copper (mol Ag/mol Cu), accurate to at least two decimal places. PSYW Mole ratio = 1.96