2. If the volume of a container holding a gas is reduced, what will happen to the presure within the container?

Transcription

1 1. Which gas law states that the volume of a fixed mass of a gas is directly proportional to its Kelvin temperature if the pressure is kept constant? A. Boyle s law B. Charles law C. Dalton s law D. Gay-Lussac s law E. Ideal gas law 2. If the volume of a container holding a gas is reduced, what will happen to the presure within the container? A. The pressure will decrease B. The pressure will increase C. The pressure will not change 3. A gas occupies a volume of 0.7 L at 10.1 kpa. What volume will the gas occupy at 101 kpa? A. 7 L B L C. 0.7 L D. 4 L 4. Which of these changes would NOT cause an increase in the pressure of a gaseous system? A. Another gas is added to the container B. Additional amounts of the same gas are added to the container C. The temperature is increased D. The container is made larger 5. Generally, for a gas at a constant volume which of the following is true? A. The pressure of a gas is directly proportional to its temperature in Kelvin B. The volume of a gas is inversely proportional to its temperature in Kelvin C. The pressure of a gas is inversely proportional to its temperature in Kelvin D. The volume of a gas is directly proportional to its temperature in Kelvin 6. If a balloon containing L of gas at 50.0 C and 101 kpa rises to an altitude where the pressure is 50.5 kpa and the temperature is 10.0 C, what would the volume of the balloon be under these new conditions? A. 400 L B L C L D. 571 L

2 7. If oxygen is removed from the air in the process of rusting, what happens to the partial pressure of oxygen in the air A. It increases B. It decreases C. It stays the same 8. What is the tendency of molecules to move toward areas of lower concentration? A. Effusion B. Suffusion C. Suspension D. Diffusion 9. The gaseous product o a reaction is collected in a 25.0 L container at 27 C. The pressure in the container is kpa and the gas has a mass of 96.0g. What is the formula mass of the gas? 10. How many liters of chlorine gas can be produced when 0.98 L of HCl react with excess O 2 at STP? 4HCl + O 2 2 Cl H 2 O A g/mol B g/mol C g/mol D. 240 g/mol A L B L C. 3.9 L D. 2.0 L E L 11. Consider an iron ball and an aluminum ball. If the two balls were at the same temperature, how would the average kinetic energy of the iron atoms compare with the average kinetic energy of the aluminum atoms? A. The average kinetic energy of the iron atoms would be greater B. The average kinetic energy of the aluminum atoms would be greater C. There would be no difference in the average kinetic energies D. No determination can be made on the basis of the information given 12. What is the volume occupied by 2.20 mol of hydrogen at STP? A L B L C L D L E L

3 13. What is the number of grams of neon present in 78.4 L of neon at STP? A g B g C g D. 105 g E. 140 g 14. At what temperature does the motion of particles theoretically cease? A K B K C C D. 273 C 15. Why is it is possible for equal volumes of gases, at the same temperature and pressure, to contain equal numbers of particles? 16. If heat is added to a boiling liquid, what happens to the temperature of the liquid? A. It increases B. It decreases C. It does not change A. Gas particles are far apart B. Gas molecules are large C. The volume of a gas molecules is inversely proportional to its mass D. This is not actually possible 17. When the vapor pressure of a liquid is equal to the atmospheric pressure, what happens to the liquid? A. It condenses B. It freezes C. It boils D. No change is observed 18. How many joules are there in 148 calories? A J B J C. 148 J D. 619 J E J

4 19. How much heat does it take to warm 16.0g of pure water from 90.0 C to C (specific heat of water = J/g C 20. A piece of candy has 5 Calories. If it could be burned, leaving nothing by carbon dioxide and water, how much heat would it give off? A joules B. 669 joules C. 160 joules D joules A. 500 calories B calories C joules D. Not enough information is given 21. When cooking food with natural gas, from where does the energy come? A. Kinetic energy in the gas B. Chemical potential energy of the gas molecules C. The pressure of the gas D. The volume of the gas 22. How does a calorie relate to a joule? A. A calorie is smaller than a joule B. A calorie is larger than a joule C. A calorie is the same size as a joule 23. A process that absorbs heat is which type of process? A. Exothermic B. Endothermic C. Polythermic D. Ectothermic 24. When gasoline is burned in an automobile engine, what happens regarding energy A. Energy is created B. Heat energy is converted to chemical energy C. Energy is destroyed D. Potential energy is transformed into kinetic energy

5 25. Which of the following equations correctly represents an endothermic reaction? A. A + B C + D + heat B. A + B + heat C + D 26. What does the symbol H stand for? A. The specific heat of a substance B. The heat capacity of a substance C. The heat of reaction for a chemical reaction D. One Calorie given off by a reaction 27. During a phase change, what happens to the temperature of a substance? A. The temperature increases B. The temperature decreases C. The temperature remains constant D. The temperature may increase or decrease depending on the situation 28. How much heat does it take to make the water in a teakettle boil if the water starts at 44 C A. 44 calories B. 44 joules C. 44 Calories D. Not enough information given 29. Compared to a glass of ice water with ice in it, a glass of ice-cold water without ice will warm up. A. Faster B. Slower C. At the same rate 30. A chunk of ice whose temperature is C is added to an insulated cup filled with water at 0.00 C. What happens in the cup? A. The ice melts until it reaches the temperature of the water B. The water cools until it reaches the temperature of the ice C. Some of the water freezes, so the chunk of ice gets larger D. None of the above

6 31. The quantity of heat needed to raise the temperature of 1.00 g of water by 1.00 C is defined as which of the following? 32. The ratio of mass to volume for an object is defined as which of the following? A. Specific heat B. Matter C. Density D. Joule A. Calorie B. Joule C. Heat of fusion D. Heat of reaction E. Calorie 33. How much energy does it take to convert 0.75 kg of ice at 15.0 C to liquid water at 40.0 C (specific heats: ice = 0.53cal/g C; water = 1.00 cal/ g C heat of fusion 80.0 cal/g 34. For a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure. This describes which of the gas laws? A B C D A. Boyle s law B. Charles law C. Gay-Lussac s law D. Dalton s law E. Ideal gas law 35. What happens to the temperature of a gas when it is compressed? A. The temperature increases B. The temperature decreases C. The temperature does not change 36. A sample of gas occupies 40.0 ml at C. What volume does the sample occupy at 27.0 C? A. 182 ml B ml C ml D ml

7 37. If a balloon is rubbed vigorously, what happens to the volume of the air in the balloon if the pressure is constant? A. It stays the same B. It increases C. It decreases 38. What does the ideal gas law allow a scientist to calculate that the other laws do not? A. Energy B. Temperature C. Pressure D. Number of moles E. Volume 39. A breathing mixture used by deep-sea divers contains helium, oxygen and carbon dioxide. What is the partial pressure oxygen at 101 kpa if P he = 84.0 kpa and P CO2 = 0.10 kpa? 40. Which of the following gases will effuse the most rapidly A. Chlorine B. Hydrogen C. Ammonia D. Bromine E. Argon A. 80% B kpa C kpa D kpa 41. Identify the limiting reagent and the volume of product formed when 11.0 L CS 2 reacts with 18.0 L O 2 to produce CO 2 and SO 2 at STP. CS 2 + 3O 2 CO 2 + 2SO How many liters of NH 3, at STP, will react with 5.3 g O 2 to form NO 2 and water? A L B L C L D L E L A. CS 2 ; 5.5 L CO 2 B. O 2 ; 2.0 L CO 2 C. CS 2 ; 11 L CO 2 D. O 2 ; 27 L SO 2 E. O 2 ; 54 L CO 2

8 43. What instrument is normally used to measure atmospheric pressure? A. Thermistor B. Barometer C. Hydrometer D. Spectrometer 44. What is the number of moles of gas in 20.0 L of oxygen at STP? A mol B mol C mol D mol E mol 45. The average kinetic energy of water molecules is greatest in which of the following? A. Steam at C B. Water at 90.0 C C. Water at 373 K D. Ice at 0.00 C 46. What is the pressure of one standard atmosphere? A kpa B kpa C. 101 kpa D kpa 47. Which states of matter can flow? A. Gases only B. Liquids only C. Gases and liquids only D. Gases liquids and solids 48. The first particles to evaporate from a liquid are those with which of the following? A. The lowest kinetic energy B. The highest kinetic energy C. The farthest from the surface of the liquid

9 49. Water could be made to boil at 105 C rather than 100 C by doing which of the following? A. Applying a great deal of heat B. Increasing the air pressure on the water C. Decreasing the pressure on the water D. Decreasing the air pressure above the water 50. What is the amount of heat required to raise the temperature of g of aluminum by 10.0 C (specific heat of aluminum = cal/g C ) A x 10 2 cal B x 10 3 cal C x 10 4 cal D x 10 5 cal E. None of the above 51. As the temperature of a sample of matter is increased, what happens to the average kinetic energy of the particles in the sample? 52. The specific heat capacity of silver is 0.24 J/g C. How many joules of enery are needed to warm f od silver from 25.0 C to 27.5 C A. It decreases B. It increases C. It does not change A J B J C. 3.24J D J 53. What happens to the energy produced by burning gasoline in a car engine? A. It is lost as heat in the exhaust B. It is transformed into work to move the car C. It heats the parts of the engine D. All of the above 54. In an exothermic reaction, which of the following is true regarding the energy stored in the chemical bonds of the reactants? A. It is equal to the energy stored in the bonks of the products B. It is greater than the energy stored in the bonds of the products C. It is less that the energy stored in the bonds of the products D. If is less than the heat released E. It is less than the heat absorbed

10 55. If you were to touch the flask in which an endothermic reaction were occurring, which of the following would be true? A. The flask would probably feel cooler than before the reaction started B. The flask would probably feel warmer than before the reaction started C. The flask would feel the same as before the reaction started D. None of the above 56. When energy is changed from one form to another which of the following is true? A. Some of the energy is lost entirely B. All of the energy can be accounted for C. A physical change occurs D. All of the energy is changed to a useful form 57. The quantity of heat required to change the temperature of 1.00 g of a substance by 1.00 C id defined as which of the following? A. Joule B. Specific heat capacity C. Calorie D. Density 58. What is the amount of heat needed to melt one mole or one gram of a solid called? A. Molar heat of fusion B. Molar heat of vaporization C. Heat of reaction D. Enthalpy E. Specific heat capacity 59. Heat changes can occur when which of the following occurs? A. A substance dissolves B. A substance melts C. A substance solidifies D. A substance vaporizes E. All of the above 60. For a given substance, the molar heat of fusion has what relationship to the molar heat of vaporization? A. They are always equal B. The heat of fusion is less C. The heat of fusion is greater

11 61. When snow melts, what happens to the surrounding air A. It gets warmer B. It gets colder C. Nothing happens to the surrounding air 62. What is used to measure the heat involved in a chemical process A. Calorie B. Joule C. Densitometer D. Barometer E. Calorimeter 63. What is the quantity of heat needed to change the temperature of 1.00g of a substance by 1.00 C? A. Calorie B. Joule C. Heat of fusion D. Specific heat E. Heat of vaporization 64. How much heat is required to melt 1.6 mol of NaCl? (molar heat of fusion for NaCl = 30.2 kj/mol) A joules B joules C joules 65. At a constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures. This describes which of the gas laws? 66. The volume of a gas is doubled while the temperature is held constant. How does the gas pressure change? A. Varies depending on the nature of the gas B. Is reduced by one-half C. Remains unchanged D. Is doubled A. Boyle s law B. Charles law C. Dalton s law D. Gay-Lussac s law E. Ideal gas law

12 67. For gases, the pressure times the volume, divided by the product of the temperature and the amount in moles is equal to a constant value. This describes which of the gas laws? 68. As the temperature of the gas in a balloon decreases, which of the following will result? A. The pressure will increase B. The average kinetic energy of the gas will decrease C. The volume will increase D. All of the above A. Boyle s law B. Charles law C. Dalton s law D. Gay-Lussac s law E. Ideal gas law 69. The combined gas law relates which of these? A. Temperature and pressure only B. Temperature, pressure and volume C. Volume and temperature only D. Pressure and volume only 70. The pressure of a gas is directly proportional to its Kelvin temperature if the volume is kept constant. This describes which of the gas laws? A. Boyle s law B. Charles law C. Dalton s law D. Gay-Lussac s law E. Ideal gas law 71. Which of these is the normal form of the ideal gas law? A. PV/nT = R B. PV/T = nr C. P = nrt/v D. PV = nrt 72. When a container is filled with 3.00 moles of H 2, 2.00 moles of O 2, and 1.00 mole of N 2, the pressure in the container is 8787 kpa. What is the partial pressure of O 2? A. 202 kpa B kpa C. 404 kpa D. Impossible to calculate

13 73. What is the pressure exerted by 32.0g of oxygen in a 22.0 L container at 30.0 C? A atm B. 229 kpa C. 547 mmhg D. 309 kpa 74. What is the first step in most stoichiometry problems? A. Add the coefficients of the reagents B. Convert given quantities to moles C. Convert given quantities to volumes D. Convert given quantities to masses 75. What happens to the average kinetic energy of the particles in a sample of matter as the temperature of the sample is increased? A. It increases B. It decreases C. It does not change 76. What volume does 3.00 moles of gas particles occupy at STP? A L B L C L D L E x 10 2 L 77. What is the volume occupied by 71.0 g of chlorine gas at STP? A L B L C L D L E L 78. Which of the following is true according to the kinetic theory of gases? A. The particles of a gas move independently of each other B. The particles in a gas move rapidly C. The particles in a gas are far apart D. All of the above E. None of the above

14 79. The pressure of a gas in a container is 152 mmhg. What is this pressure in atm? A atm B atm C atm D atm 80. Why does a liquid s evaporation rate increase when the liquid is heated? A. Because more surface molecules have enough energy to overcome the attractive forces holding them in the liquid B. Because the average kinetic energy of the liquid decreases C. Because the surface area of the liquid is reduced D. Because the potential energy of the liquid increases 81. What is the pressure when a liquid is boiling at its normal boiling point? A kpa B kpa C kpa D kpa E. Not enough information is known 82. In general, what do we know about the boiling points of ionic solids? A. They tend to be high B. They tend to be low C. They tend to be average 83. What is the specific heat of a substance if 1560 cal is required to raise the temperature of a 312 g sample by 15.0 C 84. The amount of heat transferred from an object depends on all of the following except which? A. The specific heat of the object B. The change in temperature the object undergoes C. The initial temperature of the object D. The mass of the object A cal/g C B cal/g C C cal/g C D cal/g C

15 85. A piece of metal is heated, then submerged in cool water. Which statement below describes what happens? A. The temperature of the metal will increase B. The temperature of the water will increase C. The temperature of the water will decrease D. The temperature of the water will increase and the temperature of the metal will decrease E. The temperature of the water will decrease and the temperature of the metal will increase 86. Compared to g of iron, which of the following is true about a 10.0 g sample of iron? A. The 10.0 g sample has a higher specific heat B. The 10.0 g sample has a lower specific heat C. The 10.0 g sample has the same specific heat 87. Which of the following is not a form of energy? A. Light B. Pressure C. Heat D. Electricity 88. When your body breaks sown sugar completely, it releases if you burned the same amount of sugar in a flame. A. More heat than B. Less heat than C. The same amount of heat as 89. Which of the following are valid units for specific heat (or specific heat capacity) A. cal/g C B. cal C. cal/g D. C E. g C/cal 90. The amount of heat absorbed by a melting solid the amount of heat lost by a solidifying liquid. A. Is the same as B. Is less than C. Is greater than

16 91. To calculate the amount of heat absorbed as a substance melts, which of the following information is not needed? A. The mass of the substance B. The change in temperature C. The specific heat of the substance D. The density of the sample 92. For a given substance, the molar heat of vaporization the molar heat of condensation. A. Always equals B. Is less than C. Is greater than 93. When heat is added to boiling water, its temperature. A. Increases B. Decreases C. Stays the same D. Depends on the amount of water 94. Which of the following is the SI unit of energy? A. Calorie B. Specific heat C. Joule D. Heat of reaction E. Heat of fusion 95. What term can be described as the energy change involved in a chemical reaction? A. Heat of fusion B. Joule C. Specific heat D. Calorie E. Heat of reaction 96. What is the energy required to melt a solid at its melting point? A. Heat of reaction B. Heat capacity C. Specific heat D. Heat of fusion E. Heat of vaporization