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

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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 AB into substances A and B, what is the number of mole ratios? a. 1 c. 6 b. 3 d. 9 5. Calculating 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 A and B form substance C. If the actual mole ratio of substance B to substance A is less than the balanced equation mole ratio of substance B to substance A, substance B 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. 0.288 mol c. 31.2 mol b. 3.46 mol d. 52.0 mol 12. How many grams of water are produced when 2.50 mol oxygen reacts with hydrogen? a. 0.277 g c. 45.0 g b. 22.5 g d. 90.0 g 13. What is the mass of potassium chloride when 2.50 g of potassium reacts with excess of chlorine gas? a. 4.77 g c. 9.52 g

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b. 8.57 g d. 728 g How many moles of carbon dioxide are produced when 8.30 mol of ethanol reacts with excess of oxygen? a. 0.241 mol c. 16.6 mol b. 4.15 mol d. 24.9 mol Calculate the mass of citric acid when 2.60 mol of sucrose gas reacts with oxygen. a. 0.769 g c. 999 g b. 1.30 g d. 499 g Hydrofluoric acid reacts with 31.3 g of silica to produce hexafluorosilicic acid. Determine the percent yield of H2SiF6 if the actual yield is 60.3 g. a. 0.818% c. 31.8% b. 12.2% d. 81.8% Copper reacts with 36.7 g of silver nitrate to produce copper(II) nitrate and silver. Determine the theoretical yield of Cu(NO3)2 if the actual yield is 31.29 g. a. 0.773 g c. 77.3 g b. 12.9 g d. 40.5 g

Completion Complete each statement. 18. When 200.2 g of sulfur reacts with 100.3 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. A(n) ____________________ is a ratio between the number of moles of any two substances in a balanced chemical equation. 23. A(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. A chemical reaction rarely produces the ____________________ of the product. 29. Chemists sometimes use ____________________ to speed up a chemical reaction.

Ch13 Test Multiple Choice Identify the choice that best completes the statement or answers the question. ____

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1. A gas particle of mass 5.31  10 kg has a velocity of 1.00 102 m/s. What is the kinetic energy of the molecule? a. 5.31  10 kg m2/s2 c. 2.65  10 kg m2/s2 b. 5.31  10 kg m2/s2 d. 10.6  10 kg m2/s2 2. A 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 0.100 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 EXCEPT 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. 101.3 kPa. d. 706 torr. 9. The partial pressure of a gas depends on all of the following EXCEPT 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 102.3 kPa. What is the partial pressure of nitrogen (N2) in the sample if the combined partial pressures of the other gases is 22.4 kPa? a. 62.4 kPa c. 102.3 kPa. b. 79.9 kPa d. 124.7 kPa

Completion Complete each statement.

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. A mixture consists of three gases, A, B, and C. The partial pressure of A is 5.1 Pa, of B is 1.5 Pa, and of C 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. Crystal shapes differ based on the edge length and angle of intersection of their ____________________. 18. A human body controls its temperature by the method of ____________________. 19. At boiling point, the ____________________ pressure over a liquid equals the atmospheric pressure. 20. During 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. Because 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

____ 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. Dalton’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 ____ ____ ____ ____ ____ ____ ____

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A measure of the resistance of a liquid to flow The energy required to increase the surface area of a liquid by a given amount Force per unit area The model describing the behavior of gases in terms of particles in motion An instrument used to measure atmospheric pressure A measure of the average kinetic energy of the particles in a sample of matter States that the total pressure of a mixture of gases is equal to the sum of the pressures of each gas in the mixture The temperature at which a crystalline solid becomes a liquid The pressure exerted by a vapor over a liquid A graph that shows in which phase a substance exists under different conditions of temperature and pressure Collisions between gas particles in which no kinetic energy is lost The movement of one material through another The process by which a substance changes from a gas or vapor to a solid without first becoming a liquid A solid whose atoms, ions, or molecules are arranged in an orderly, geometric, three-dimensional structure Temperature at which a liquid becomes a crystalline solid States that the rate of effusion for a gas is inversely proportional to the square root of its molar mass Temperature at which the vapor pressure of a liquid equals the external or atmospheric pressure The process by which a solid changes directly to a gas without first becoming a liquid A solid in which the particles are not arranged in a regular, repeating pattern

Ch12 Test Answer Section MULTIPLE CHOICE 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11.

ANS: B PTS: 1 ANS: B PTS: 1 ANS: A PTS: 1 ANS: C PTS: 1 ANS: C PTS: 1 ANS: D PTS: 1 ANS: C PTS: 1 ANS: A PTS: 1 ANS: D PTS: 1 ANS: D PTS: 1 ANS: C The equation for the combustion of propane is

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Feedback A B C D

Divide the unknown moles of carbon dioxide by the known moles of propane. Multiply the known number of moles of propane by the mole ratio. Correct! Balance the equation correctly.

PTS: 1 DIF: 2 REF: Page 359 OBJ: 12.2.2 Use the steps to solve stoichiometric problems. TOP: Use the steps to solve stoichiometric problems. KEY: Stoichiometric mole-to-mole conversion 12. ANS: D The balanced chemical equation is .

NAT: UCP.1 | UCP.3 | B.3 MSC: 3

Feedback A B C D

Multiply the number of moles of water by the molar mass of water. Multiply the number of moles by the mole ratio. Balance the equation correctly. Correct!

PTS: 1 DIF: 3 REF: Page 360 OBJ: 12.2.2 Use the steps to solve stoichiometric problems. TOP: Use the steps to solve stoichiometric problems. KEY: Stoichiometric mole-to-mass conversion 13. ANS: A The balanced chemical equation is .

NAT: UCP.1 | UCP.3 | B.3 MSC: 3

Feedback A B

Correct! Calculate the mass of KCl using the molar mass as a conversion factor.

C D

Balance the equation correctly. Convert the grams of KCl to moles using the inverse of molar mass as the conversion factor.

PTS: 1 DIF: 3 REF: Page 361 OBJ: 12.2.2 Use the steps to solve stoichiometric problems. TOP: Use the steps to solve stoichiometric problems. KEY: Stoichiometric mass-to-mass conversion 14. ANS: C The mole ratio of carbon dioxide to ethanol is 2:1.

NAT: UCP.1 | UCP.3 | B.3 MSC: 3

Feedback A B C D

Divide the unknown moles by the known moles. Multiply the known number of moles by the mole ratio. Correct! Balance the equation correctly.

PTS: 1 DIF: 1 REF: Page 359 OBJ: 12.2.2 Use the steps to solve stoichiometric problems. TOP: Use the steps to solve stoichiometric problems. KEY: Stoichiometric mole-to-mole conversion 15. ANS: D The molar mass of citric acid is 192.044 g.

NAT: UCP.1 | UCP.3 | B.3 MSC: 3

Feedback A B C D

Divide the unknown moles by the known moles. Multiply the known number of moles by the mole ratio and the molar mass. Balance the equation correctly. Correct!

PTS: 1 DIF: 2 REF: Page 360 OBJ: 12.2.2 Use the steps to solve stoichiometric problems. TOP: Use the steps to solve stoichiometric problems. KEY: Stoichiometric mole-to-mass conversion 16. ANS: D Percent yield (actual yield/theoretical yield)  100

NAT: UCP.1 | UCP.3 | B.3 MSC: 3

Feedback A B C D

Multiply the yield by 100 to calculate the percent yield. Divide the actual yield by the theoretical yield. The molar mass is incorrect. Correct!

PTS: 1 DIF: 3 REF: Page 371 OBJ: 12.4.2 Determine the percent yield for a chemical reaction. NAT: UCP.3 | B.3 TOP: Determine the percent yield for a chemical reaction. KEY: Percent yield MSC: 3 17. ANS: D Percent yield (actual yield/theoretical yield)  100

Feedback A B C D

Multiply the number of moles by the molar mass to obtain the theoretical yield. The mole ratio is incorrect. The molar mass is incorrect. Correct!

PTS: OBJ: NAT: KEY:

1 DIF: 3 REF: Page 371 12.4.2 Determine the percent yield for a chemical reaction. UCP.3 | B.3 TOP: Determine the percent yield for a chemical reaction. Percent yield MSC: 3

COMPLETION 18. ANS: chlorine PTS: OBJ: NAT: KEY: 19. ANS:

1 DIF: 2 REF: Page 365 12.3.1 Identify the limiting reactant in a chemical equation. B.3 TOP: Identify the limiting reactant in a chemical equation. Limiting reactant MSC: 3 excess

PTS: 1 DIF: 2 REF: Page 365 OBJ: 12.3.2 Identify the excess reactant and calculate the amount remaining after the reaction is complete. NAT: UCP.3 | B.3 TOP: Identify the excess reactant and calculate the amount remaining after the reaction is complete. KEY: Excess reactant MSC: 1 20. ANS: limiting reactant PTS: 1 21. ANS: actual yield PTS: 1 22. ANS: mole ratio PTS: 1 23. ANS: excess reactant PTS: 1 24. ANS: theoretical yield PTS: 1 25. ANS: stoichiometry PTS: 1 26. ANS: percent yield PTS: 1

27. ANS: limiting reactant PTS: 1 28. ANS: theoretical yield PTS: 1 29. ANS: excess reactant PTS: 1

Ch13 Test Answer Section MULTIPLE CHOICE 1. ANS: C The kinetic energy of a particle is

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Feedback A B C D

Instead of multiplying the mass and velocity, multiply the square of velocity by the mass. Divide the product of multiplication of mass and the square of velocity by 2. Correct! 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.

PTS: 1 DIF: 1 REF: Page 386 OBJ: 13.1.1 Use the kinetic-molecular theory to explain the behavior of gases. NAT: UCP.2 | B.2 | B.4 TOP: Use the kinetic-molecular theory to explain the behavior of gases. KEY: Particle energy MSC: 3 2. ANS: B p(total) p(O ) p(H ) p(H O) Feedback A B C D

Instead of subtracting 380 mm by 684 mm, add 76 mm to 380 mm and then subtract the result from 684 mm. Correct! The total pressure of the system is 684 mm. The partial pressure of a component gas cannot exceed the total pressure of the system.

PTS: 1 DIF: 3 REF: Page 388 OBJ: 13.1.3 Explain how gas pressure is measured and calculate the partial pressure of a gas. NAT: UCP.3 | B.4 TOP: Explain how gas pressure is measured and calculate the partial pressure of a gas. KEY: Partial pressure MSC: 3 3. ANS: C The heat flow from water to ice is used to break the hydrogen bonds of the ice crystal.

Feedback A B C D

4. 5. 6. 7. 8. 9. 10.

Ice remains at the same temperature. The temperature of water decreases as heat flows from water to ice. Correct! The temperature of ice does not depend on the temperature of water.

PTS: OBJ: NAT: TOP: KEY: ANS: ANS: ANS: ANS: ANS: ANS: ANS:

1 DIF: 1 REF: Page 404 13.4.1 Explain how the addition and removal of energy can cause a phase change. UCP.3 | B.2 | B.4 | B.6 Explain how the addition and removal of energy can cause a phase change. Phase change MSC: 1 A PTS: 1 A PTS: 1 D PTS: 1 D PTS: 1 B PTS: 1 B PTS: 1 B PTS: 1

COMPLETION 11. ANS: ammonia, hydrogen PTS: OBJ: NAT: KEY: 12. ANS:

1 DIF: 1 REF: Page 387 13.1.2 Describe how mass affects the rates of diffusion and effusion. UCP.3 | B.4 TOP: Describe how mass affects the rates of diffusion and effusion. Graham's law MSC: 2 7.8

PTS: OBJ: NAT: TOP: KEY: 13. ANS:

1 DIF: 1 REF: Page 391 13.1.3 Explain how gas pressure is measured and calculate the partial pressure of a gas. UCP.3 | B.4 Explain how gas pressure is measured and calculate the partial pressure of a gas. Partial pressure MSC: 2 intermolecular

PTS: OBJ: NAT: KEY: 14. ANS:

1 DIF: 1 REF: Page 393 13.2.1 Describe and compare intramolecular and intermolecular forces. B.2 | B.4 TOP: Describe and compare intramolecular and intermolecular forces. Intermolecular forces | Intramolecular force MSC: 1 less

PTS: 1 DIF: 1 REF: Page 398 OBJ: 13.3.2 Relate properties such as viscosity, surface tension, and capillary action to intermolecular forces. NAT: B.2 | B.4 TOP: Relate properties such as viscosity, surface tension, and capillary action to intermolecular forces. KEY: Surface tension MSC: 1 15. ANS: adhesive, cohesive

PTS: 1 DIF: 1 REF: Page 399 OBJ: 13.3.2 Relate properties such as viscosity, surface tension, and capillary action to intermolecular forces. NAT: B.2 | B.4 TOP: Relate properties such as viscosity, surface tension, and capillary action to intermolecular forces. KEY: Capillary action MSC: 1 16. ANS: unit cells PTS: 1 DIF: 1 REF: Page 400 OBJ: 13.3.3 Compare the structures and properties of different types of solids. NAT: B.2 TOP: Compare the structures and properties of different types of solids. KEY: Unit cell MSC: 1 17. ANS: faces surfaces PTS: OBJ: NAT: KEY: 18. ANS:

1 DIF: 1 REF: Page 400 13.3.3 Compare the structures and properties of different types of solids. B.2 TOP: Compare the structures and properties of different types of solids. Cubic crystal MSC: 1 evaporation

PTS: OBJ: NAT: TOP: KEY: 19. ANS:

1 DIF: 1 REF: Page 405 13.4.1 Explain how the addition and removal of energy can cause a phase change. UCP.3 | B.2 | B.4 | B.6 Explain how the addition and removal of energy can cause a phase change. Evaporation MSC: 1 vapor

PTS: OBJ: NAT: TOP: KEY: 20. ANS:

1 DIF: 1 REF: Page 406 13.4.1 Explain how the addition and removal of energy can cause a phase change. UCP.3 | B.2 | B.4 | B.6 Explain how the addition and removal of energy can cause a phase change. Vapor pressure MSC: 1 released

PTS: OBJ: NAT: TOP: KEY: 21. ANS:

1 DIF: 1 REF: Page 407 13.4.1 Explain how the addition and removal of energy can cause a phase change. UCP.3 | B.2 | B.4 | B.6 Explain how the addition and removal of energy can cause a phase change. Condensation MSC: 2 motion

PTS: 1 22. ANS: small PTS: 1 23. ANS: forces PTS: 1

24. ANS: random PTS: 1 25. ANS: elastic, kinetic PTS: 1 26. ANS: KE = 1/2mv2 PTS: 1 27. ANS: Temperature PTS: 1 MATCHING 28. ANS: B 29. ANS: C 30. ANS: A

PTS: 1 PTS: 1 PTS: 1

31. 32. 33. 34. 35. 36. 37. 38. 39. 40. 41. 42. 43. 44. 45. 46. 47. 48. 49.

PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS:

ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS:

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