Ch12 Test. Multiple Choice Identify the choice that best completes the statement or answers the question.

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1 h12 Test Multiple hoice Identify the choice that best completes the statement or answers the question. 1. Stoichiometry is based on the law of conservation of. a. charge. c. reactants. b. mass. d. volume. 2. In a balanced chemical equation, the numbers of individual particles and the numbers of moles of particles are represented by the. a. chemical symbols. c. molar masses. b. coefficients. d. subscripts. 3. Mole ratios for a reaction are obtained from the. a. balanced chemical equation. c. periodic table. b. molar masses. d. total mass of products. 4. In the decomposition reaction of compound into substances and, what is the number of mole ratios? a. 1 c. 6 b. 3 d alculating the mass of a reactant and product from the number of moles of another product or reactant in a chemical equation is an example of a. a. mass-to-mass conversion. c. mole-to-mass conversion. b. mass-to-mole conversion. d. mole-to-mole conversion. 6. Limiting a reactant is often accomplished by. a. producing excess product. c. slowing down a chemical reaction. b. overcoming conservation of mass. d. using an excess of another reactant. 7. In a reaction, substances and form substance. If the actual mole ratio of substance to substance is less than the balanced equation mole ratio of substance to substance, substance is the. a. actual yield. c. limiting reactant. b. excess reactant. d. product. 8. Percent yield of a product is a measure of a reaction s. a. efficiency. c. rate. b. heat production. d. spontaneity. 9. The actual yield of a product is. a. a negative value. c. the same as its theoretical yield. b. independent of the reactants. d. measured experimentally. 10. The most important industrial chemical in the world is. a. carbon dioxide. c. petroleum. b. oxygen. d. sulfuric acid. 11. How many moles of carbon dioxide is produced when 10.4 mol of propane gas is burned in excess oxygen? a mol c mol b mol d mol 12. How many grams of water are produced when 2.50 mol oxygen reacts with hydrogen? a g c g b g d g 13. What is the mass of potassium chloride when 2.50 g of potassium reacts with excess of chlorine gas? a g c g

2 b g d. 728 g 14. How many moles of carbon dioxide are produced when 8.30 mol of ethanol reacts with excess of oxygen? a mol c mol b mol d mol 15. alculate the mass of citric acid when 2.60 mol of sucrose gas reacts with oxygen. a g c. 999 g b g d. 499 g 16. Hydrofluoric acid reacts with 31.3 g of silica to produce hexafluorosilicic acid. etermine the percent yield of H 2 SiF 6 if the actual yield is 60.3 g. a % c. 31.8% b. 12.2% d. 81.8% 17. opper reacts with 36.7 g of silver nitrate to produce copper(ii) nitrate and silver. etermine the theoretical yield of u(no 3 ) 2 if the actual yield is g. a g c g b g d g ompletion omplete each statement. 18. When g of sulfur reacts with g of chlorine to produce disulfur dichloride, acts as the limiting reactant. 19. Nitrogen acts as a(n) reactant in the production of ammonia. Use the following terms to complete the statements. Some terms will be used more than once. actual yield percent yield stoichiometry excess reactant mole ratio theoretical yield limiting reactant 20. The reactant that limits the extent of the reaction is called the. 21. The amount of product actually produced by a chemical reaction is called the. 22. (n) is a ratio between the number of moles of any two substances in a balanced chemical equation. 23. (n) is a reactant that has a portion remaining after the reaction has stopped. 24. The is the maximum amount of product that can be produced from a given amount of reactant. 25. The study of the quantitative relationships among the amounts of reactants used and the amounts of products formed by a chemical reaction is called. 26. The ratio of the actual yield to the theoretical yield expressed as a percent is called the. 27. The amount of product formed during a reaction depends on the. 28. chemical reaction rarely produces the of the product. 29. hemists sometimes use to speed up a chemical reaction.

3 h13 Test Multiple hoice Identify the choice that best completes the statement or answers the question. 1. gas particle of mass kg has a velocity of m/s. What is the kinetic energy of the molecule? a kg m 2 /s 2 c kg m 2 /s 2 b kg m 2 /s 2 d kg m 2 /s 2 2. mixture of oxygen, hydrogen, and water vapor has a total pressure of 684 mm Hg. The partial pressure of oxygen is 380 mm Hg and that of hydrogen is atm. What is the partial pressure of water vapor? a. 304 mm Hg c. 684 mm Hg b. 228 mm Hg d. 690 mm Hg 3. Which of the following about an ice cube floating in a glass of water is correct? a. The temperature of the ice cube increases. b. The temperature of the ice cube decreases. c. The temperature of the ice cube remains constant. d. The temperature of the ice cube will fluctuate. 4. Pressure is defined as force per unit a. area. c. time. b. mass. d. volume. 5. What is an instrument designed to measure atmospheric pressure? a. barometer c. sphygmomanometer b. manometer d. thermometer 6. The height of the liquid in a barometer is affected by all of the following EXEPT the a. altitude. c. density of the liquid in the column. b. atmospheric pressure. d. diameter of the column tube. 7. The pressure of the gas in a manometer is directly related to which of the following quantities? a. height of the mercury column in the closed-end arm b. height of the mercury column in the open-end arm c. a + b d. a b 8. One atmosphere is equal to a pressure of a. 76 mm Hg. c. 147 psi. b kpa. d. 706 torr. 9. The partial pressure of a gas depends on all of the following EXEPT the a. concentration of the gas. c. size of the container. b. identity of the gas. d. temperature of the gas. 10. The pressure of a sample of air in a manometer is kpa. What is the partial pressure of nitrogen (N 2 ) in the sample if the combined partial pressures of the other gases is 22.4 kpa? a kpa c kpa. b kpa d kpa ompletion omplete each statement.

4 11. If the molar mass of ammonia is 17 g/mol, and that of hydrogen is 2 g/mol, gas diffuses more slowly than gas. 12. mixture consists of three gases,,, and. The partial pressure of is 5.1 Pa, of is 1.5 Pa, and of is 1.2 Pa. The total pressure of the mixture is Pa. 13. When a cellulose paper is dipped in water, the force existing between the particles of the cellulose paper and the water particles is a(n) force. 14. The surface tension of water is greater than the surface tension of cooking oil because the attractive forces between the molecules of cooking oil is than the attractive forces between the molecules of water. 15. Paper towels can absorb water to a large extent because the forces between the molecules of paper and water are greater than the forces among water molecules. 16. The smallest, repetitive parts of crystals such as fluorite and corundum are called. 17. rystal shapes differ based on the edge length and angle of intersection of their. 18. human body controls its temperature by the method of. 19. t boiling point, the pressure over a liquid equals the atmospheric pressure. 20. uring the deposition process by which atmospheric carbon dioxide undergoes a phase change to form solid carbon dioxide, energy is. 21. The kinetic molecular theory describes the behavior of gases in terms of particles in. The kinetic-molecular theory makes the following assumptions. 22. In a sample of a gas, the volume of the gas particles themselves is very compared to the volume of the sample. 23. ecause gas particles are far apart, there are no significant attractive or repulsive between gas particles. 24. Gas particles are in constant and motion. 25. The collisions between gas particles are ; that is, no energy is lost. 26. The kinetic energy of a particle is represented by the equation. 27. is a measure of the average kinetic energy of the particles in a sample of matter. Matching Match the terms below with their correct definitions. a. boiling point c. melting point b. freezing point 28. Temperature at which a liquid is converted into a crystalline solid 29. Temperature at which the forces holding a crystalline lattice together are broken

5 30. Temperature at which the vapor pressure of a liquid equals the external or atmospheric pressure Match the terms below with their correct definitions. a. barometer k. melting point b. alton s law of partial pressure l. Graham s law of effusion c. phase diagram m. amorphous solid d. pressure n. deposition e. surface tension o. boiling point f. temperature p. crystalline solid g. elastic collisions q. sublimation h. vapor pressure r. freezing point i. viscosity s. diffusion j. kinetic-molecular theory 31. measure of the resistance of a liquid to flow 32. The energy required to increase the surface area of a liquid by a given amount 33. Force per unit area 34. The model describing the behavior of gases in terms of particles in motion 35. n instrument used to measure atmospheric pressure 36. measure of the average kinetic energy of the particles in a sample of matter 37. States that the total pressure of a mixture of gases is equal to the sum of the pressures of each gas in the mixture 38. The temperature at which a crystalline solid becomes a liquid 39. The pressure exerted by a vapor over a liquid 40. graph that shows in which phase a substance exists under different conditions of temperature and pressure 41. ollisions between gas particles in which no kinetic energy is lost 42. The movement of one material through another 43. The process by which a substance changes from a gas or vapor to a solid without first becoming a liquid 44. solid whose atoms, ions, or molecules are arranged in an orderly, geometric, three-dimensional structure 45. Temperature at which a liquid becomes a crystalline solid 46. States that the rate of effusion for a gas is inversely proportional to the square root of its molar mass 47. Temperature at which the vapor pressure of a liquid equals the external or atmospheric pressure 48. The process by which a solid changes directly to a gas without first becoming a liquid 49. solid in which the particles are not arranged in a regular, repeating pattern

6 h12 Test nswer Section MULTIPLE HOIE 1. NS: 2. NS: 3. NS: 4. NS: 5. NS: 6. NS: 7. NS: 8. NS: 9. NS: 10. NS: 11. NS: The equation for the combustion of propane is. ivide the unknown moles of carbon dioxide by the known moles of propane. Multiply the known number of moles of propane by the mole ratio. alance the equation correctly. IF: 2 REF: Page 359 OJ: Use the steps to solve stoichiometric problems. NT: UP.1 UP.3.3 TOP: Use the steps to solve stoichiometric problems. KEY: Stoichiometric mole-to-mole conversion MS: NS: The balanced chemical equation is. Multiply the number of moles of water by the molar mass of water. Multiply the number of moles by the mole ratio. alance the equation correctly. IF: 3 REF: Page 360 OJ: Use the steps to solve stoichiometric problems. NT: UP.1 UP.3.3 TOP: Use the steps to solve stoichiometric problems. KEY: Stoichiometric mole-to-mass conversion MS: NS: The balanced chemical equation is. alculate the mass of Kl using the molar mass as a conversion factor.

7 alance the equation correctly. onvert the grams of Kl to moles using the inverse of molar mass as the conversion factor. IF: 3 REF: Page 361 OJ: Use the steps to solve stoichiometric problems. NT: UP.1 UP.3.3 TOP: Use the steps to solve stoichiometric problems. KEY: Stoichiometric mass-to-mass conversion MS: NS: The mole ratio of carbon dioxide to ethanol is 2:1. ivide the unknown moles by the known moles. Multiply the known number of moles by the mole ratio. alance the equation correctly. IF: 1 REF: Page 359 OJ: Use the steps to solve stoichiometric problems. NT: UP.1 UP.3.3 TOP: Use the steps to solve stoichiometric problems. KEY: Stoichiometric mole-to-mole conversion MS: NS: The molar mass of citric acid is g. ivide the unknown moles by the known moles. Multiply the known number of moles by the mole ratio and the molar mass. alance the equation correctly. IF: 2 REF: Page 360 OJ: Use the steps to solve stoichiometric problems. NT: UP.1 UP.3.3 TOP: Use the steps to solve stoichiometric problems. KEY: Stoichiometric mole-to-mass conversion MS: NS: Percent yield (actual yield/theoretical yield) 100 Multiply the yield by 100 to calculate the percent yield. ivide the actual yield by the theoretical yield. The molar mass is incorrect. IF: 3 REF: Page 371 OJ: etermine the percent yield for a chemical reaction. NT: UP.3.3 TOP: etermine the percent yield for a chemical reaction. KEY: Percent yield MS: NS: Percent yield (actual yield/theoretical yield) 100

8 Multiply the number of moles by the molar mass to obtain the theoretical yield. The mole ratio is incorrect. The molar mass is incorrect. IF: 3 REF: Page 371 OJ: etermine the percent yield for a chemical reaction. NT: UP.3.3 TOP: etermine the percent yield for a chemical reaction. KEY: Percent yield MS: 3 OMPLETION 18. NS: chlorine IF: 2 REF: Page 365 OJ: Identify the limiting reactant in a chemical equation. NT:.3 TOP: Identify the limiting reactant in a chemical equation. KEY: Limiting reactant MS: NS: excess IF: 2 REF: Page 365 OJ: Identify the excess reactant and calculate the amount remaining after the reaction is complete. NT: UP.3.3 TOP: Identify the excess reactant and calculate the amount remaining after the reaction is complete. KEY: Excess reactant MS: NS: limiting reactant 21. NS: actual yield 22. NS: mole ratio 23. NS: excess reactant 24. NS: theoretical yield 25. NS: stoichiometry 26. NS: percent yield

9 27. NS: limiting reactant 28. NS: theoretical yield 29. NS: excess reactant h13 Test nswer Section MULTIPLE HOIE 1. NS: The kinetic energy of a particle is. Instead of multiplying the mass and velocity, multiply the square of velocity by the mass. ivide the product of multiplication of mass and the square of velocity by 2. Instead of multiplying the product of mass and the square of velocity by 2, divide the product of multiplication of mass and square of velocity by 2. IF: 1 REF: Page 386 OJ: Use the kinetic-molecular theory to explain the behavior of gases. NT: UP TOP: Use the kinetic-molecular theory to explain the behavior of gases. KEY: Particle energy MS: 3 2. NS: p(total) p(o ) p(h ) p(h O) Instead of subtracting 380 mm by 684 mm, add 76 mm to 380 mm and then subtract the result from 684 mm. The total pressure of the system is 684 mm. The partial pressure of a component gas cannot exceed the total pressure of the system. IF: 3 REF: Page 388 OJ: Explain how gas pressure is measured and calculate the partial pressure of a gas. NT: UP.3.4 TOP: Explain how gas pressure is measured and calculate the partial pressure of a gas. KEY: Partial pressure MS: 3 3. NS: The heat flow from water to ice is used to break the hydrogen bonds of the ice crystal.

10 Ice remains at the same temperature. The temperature of water decreases as heat flows from water to ice. The temperature of ice does not depend on the temperature of water. IF: 1 REF: Page 404 OJ: Explain how the addition and removal of energy can cause a phase change. NT: UP TOP: Explain how the addition and removal of energy can cause a phase change. KEY: Phase change MS: 1 4. NS: 5. NS: 6. NS: 7. NS: 8. NS: 9. NS: 10. NS: OMPLETION 11. NS: ammonia, hydrogen IF: 1 REF: Page 387 OJ: escribe how mass affects the rates of diffusion and effusion. NT: UP.3.4 TOP: escribe how mass affects the rates of diffusion and effusion. KEY: Graham's law MS: NS: 7.8 IF: 1 REF: Page 391 OJ: Explain how gas pressure is measured and calculate the partial pressure of a gas. NT: UP.3.4 TOP: Explain how gas pressure is measured and calculate the partial pressure of a gas. KEY: Partial pressure MS: NS: intermolecular IF: 1 REF: Page 393 OJ: escribe and compare intramolecular and intermolecular forces. NT:.2.4 TOP: escribe and compare intramolecular and intermolecular forces. KEY: Intermolecular forces Intramolecular force MS: NS: less IF: 1 REF: Page 398 OJ: Relate properties such as viscosity, surface tension, and capillary action to intermolecular forces. NT:.2.4 TOP: Relate properties such as viscosity, surface tension, and capillary action to intermolecular forces. KEY: Surface tension MS: NS: adhesive, cohesive

11 IF: 1 REF: Page 399 OJ: Relate properties such as viscosity, surface tension, and capillary action to intermolecular forces. NT:.2.4 TOP: Relate properties such as viscosity, surface tension, and capillary action to intermolecular forces. KEY: apillary action MS: NS: unit cells IF: 1 REF: Page 400 OJ: ompare the structures and properties of different types of solids. NT:.2 TOP: ompare the structures and properties of different types of solids. KEY: Unit cell MS: NS: faces surfaces IF: 1 REF: Page 400 OJ: ompare the structures and properties of different types of solids. NT:.2 TOP: ompare the structures and properties of different types of solids. KEY: ubic crystal MS: NS: evaporation IF: 1 REF: Page 405 OJ: Explain how the addition and removal of energy can cause a phase change. NT: UP TOP: Explain how the addition and removal of energy can cause a phase change. KEY: Evaporation MS: NS: vapor IF: 1 REF: Page 406 OJ: Explain how the addition and removal of energy can cause a phase change. NT: UP TOP: Explain how the addition and removal of energy can cause a phase change. KEY: Vapor pressure MS: NS: released IF: 1 REF: Page 407 OJ: Explain how the addition and removal of energy can cause a phase change. NT: UP TOP: Explain how the addition and removal of energy can cause a phase change. KEY: ondensation MS: NS: motion 22. NS: small 23. NS: forces

12 24. NS: random 25. NS: elastic, kinetic 26. NS: KE = 1/2mv NS: Temperature MTHING 28. NS: 29. NS: 30. NS: 31. NS: I 32. NS: E 33. NS: 34. NS: J 35. NS: 36. NS: F 37. NS: 38. NS: K 39. NS: H 40. NS: 41. NS: G 42. NS: S 43. NS: N 44. NS: P 45. NS: R 46. NS: L 47. NS: O 48. NS: Q 49. NS: M