1Final Exam Review-Comprehensive

1. A barometer measures which of the following: A. temperature of the atmosphere B. pressure of the atmosphere C. molecular motion D. volume of a gas

2. The attractive forces between molecules becomes less when A. temperature is raised at constant pressure B. temperature is lowered at constant pressure C. pressure is raised at constant temperature D. volume is decreased at constant temperature

3. When the molecules of a confined gas are made to move faster, A. the volume of the gas decreases. B. the temperature of the gas decreases. C. the temperature of the gas remains constant. D. the temperature of the gas increases.

4. The kinetic energy of the following gas molecules is the same. Which one is moving the fastest? A. CO B. O C. NH D. H

5. The boiling point of any liquid is: A. 100 degrees C B. the temperature at which as many molecules leave the liquid as return to it C. the temperature at which the vapor pressure is equal to the external pressure D. the temperature at which NO molecules can return to the bulk of the liquid

6. The critical temperature of a substance is A. the temperature required to liquefy the gas at one atmosphere pressure. B. the temperature at which the substance begins to decompose. C. the highest temperature at which the substance can be a liquid. D. the temperature at which the liquid evaporates.

7. Standard temperature and pressure (STP) are defined as A 0 ºC and 1.0 atm pressure .B 0 ºC and 273 mm Hg pressure. C 0 K and 1.0 atm pressure. D 0 K and 760 mm Hg pressure.

8. Which state of matter is characterized by the highest intermolecular forces of attraction? A. solid B. liquid C. gas

9. Which state of matter is most easily compressed into a smaller volume? A. gas B. liquid C. solid

10. Which state of matter is characterized by the lowest intermolecular forces of attraction? A. gas B. liquid C. solid

11. The boiling point of water is always 100 degrees C. A. True B. False

12. The properties of a solution are uniform throughout any single sample of the solution. A. True B. False

13. If a sample of gas is heated in a rigid container A. it may change its weight B. it may increase in volume C. it must increase its pressure D. it must increase its density

214. In which of the following phase change is energy released?

A. condensation, B. sublimation, C. vaporization D. ice melting

15. Observations suggest that the liquid moves by the sliding of one 2 layer over the other. The term below which best describes this is

A. Diffusion B. Immiscibility C. Viscosity D. Compressibility E. Surface tension

16. If a heavy gas, like carbon dioxide, is placed in the bottom of a container, and a light gas, such as hydrogen, is placed on top of 3 the heavy gas, within a few hours the two will be completely mixed. The term below which best describes this is

A. Diffusion B. Immiscibility C. Viscosity D. Compressibility

17. When a given mass of gas is heated while its volume is held constant A. the gas condenses to a liquid B. the pressure of the gas decreases C. the pressure of the gas remains the same D. the molecules will move faster

18. Atmospheric pressure is equal to A. 760 atm B. the weight of a column of mercury at sea level C. the height of mercury in an inverted tube supported by weight of air above the surface of the mercury D. 760 mm

19. The pressure of a gas is a measure of A. the speed of a gas molecule B. the number of gas molecules in a sample C. the force exerted by a gas on a specified area D. the total energy of a gas sample which is dependent on the temperature of that sample

20. When equal numbers of moles of two gases at the same temperature are mixed in a container, the pressure of the gaseous mixture is A. given by Gay_Lussac's law of combining volumes B. the product of the pressures each gas would have if alone C. the difference of the pressures each gas would have if alone in the container D. the sum of the pressures each would have if alone

21. If the volume of a given quantity of gas is held constant and its temperature is raised, the pressure will A. double B. be reduced C. be increased D. be reduced to one half the original pressure

22. According to kinetic theory, a difference between liquids and gases is A. distance between molecules B. average kinetic energy at a given temperature C. the molecules of one are in constant motion D. both A and B

23. Intermolecular forces in liquids are A. the greatest of any phase because of the fluidity of liquids B. the least of any phase because the molecules in a liquid are always in constant random motion C. intermediate between those of gases and solids D. equal to zero

24. Two groups of molecules are in a fluid state. One moves through the other. The process is called A. diffusion B. mitosis C. respiration D. excretion

25. When a solid is changed to a gas, without melting, the process is called A. diffusion B. boiling C. sublimation D. osmosis

326. For a sample of gas molecules, the average kinetic energy depends on the value of theA. temperature and pressureB. volume only.C. temperature only.D. temperature and number of moles.

27. In which state of matter (at a constant temperature) do the particles present have the greatest amount of energy?A. Solids B. Liquids C. Gases D. Solids and Liquids

28.The phase change represented by the equation I2 (s) ----> I2 (g) is calledA. deposition B. condensation C. melting D. sublimation

29. The energy an object possesses due to its relative position is: A. potential energy B. electrical energy C. chemical energy D. kinetic energy

30. The phase change from gas to solid is called _____. A. sublimation B. freezing C. deposition D. condensation E. melting

31. Which statement below is not true?A. deposition forms a solid and releases energy Diagram 1B. vaporization forms a gas and kinetic energy increasesC. sublimation forms a gas and requires energy inputD. freezing forms a solid and requires energy input

32. What is the melting point of the substance sat right?A. -5°C B. 5°C C. 15°C D. 25°

33. Which letter represents boiling of the liquid?A. d B. a C. b D.c

34.At which letter is liquid absorbing heat?A.a B.b C. c D. d

35.In the diagram below, a liquid substance is present at

A.x B.y C.z d. not show 36. What does k represent?A. critical point B.triple pointC.saturationD.y intercept

37. At which temperature and pressure does this substance change to a gas?A. 0C,25B. 100C, 1.5C.850C, 1.5D. none of these

438. If the pressure and temperature of a gas are held constant and some gas is added to the container & some is allowed

to escape, a change in which of the following can be observedA rate of diffusion B.chemical properties C.volume D.kinetic energy

39. What does the constant bombardment of gas molecules against the inside walls of a container produceA diffusion B pressure C temperature D density

40. Which of the following gases is the best choice for inflating a balloon that must remain inflated for a long period of timeA argon B oxygen C hydrogen D neon

41. If a sealed syringe is suddenly placed in hot water, in which direction would the piston (plunger) slide A out B in C cannot be predicted D no movement will occur

42. Convert the pressure 0.75 atm to mm HgA 760 mm Hg B 570 mm Hg C 101.325 mm Hg D 430 mm Hg

43. A breathing mixture used by deep sea divers contains helium, oxygen and carbon dioxide. What is the partial pressure of oxygen at 101.4 KPa if PHe = 82.5 KPa and PCo2 = 0.4 KPa.A 19.3 KPa B 82.9 KPa C 101.0 KPa D 18.5 KPa

44. If a balloon is heated, what happens to the pressure of the air inside the balloon if the volume remains constant -A decreasesB change can’t be predictedC increasesD stays the same

45. Why does the pressure inside a container of gas increase if more gas is added to the container.A there is an increase in the number of collisions between the particles and the walls of the containerB there is a decrease in the volume of the gasC there is an increase in the force of the collisions between the particles of the walls of the containerD there is an increase in the temperature of the gas

46. Standard temperature is exactlyA 2730C B.00C C.1000C D. 0 K

47. The volume of a gas is doubled, while the temperature is held constant. How does the gas pressure change?A it doublesB it does not changeC it is reduced by halfD it varies depending on the type of gas

48. A mixture of four gases exerts a total pressure of 860 mm Hg. Gases A & B exert 220 mm Hg. Gas C exerts 110 mm Hg. What pressure is exerted by Gas D?A 860 mm Hg B 220 mm Hg C 165 mm Hg D 310 mm Hg

49. The ___________ within a molecule are caused by the motion of its electrons and is temporaryA hydrogen bondingB fluidityC dispersion forcesD dipole-dipole interaction

50. Which of the following statements is NOT trueA at a given temperature, all gas particles have the same average kinetic energyB The viscosity of a liquid does not depend on the strength of intermolecular forcesC a liquid is less fluid than a gas because the particles of a liquid have greater intermolecular forcesD a gas expands until it fills its container because its particles are in constant & random motion

551. What quantity does the ideal gas allow a scientist to calculate that the other laws do not?

A temperature B volume C pressure D number of moles

52. Consider a gold cube and a silver cube. If the two cubes were at the same temperature, how would the average kinetic energy of the particles in the gold compare with the average kinetic energy of the particles in the silver?A There would be no difference in the average kinetic energyB The average kinetic energy of the gold particles would be greaterC The average kinetic energy of the silver particles would be greaterD No determination can be made based on the information given

53. The temperature at which the motion of particles theoretically ceases isA. -273 K B. 0oC C. 0 K D. 2730 C

54. The pressure of a gas in a container is 152 mm Hg. This is equivalent toA.0.4 atm B.0.3 atm C.2 atm D.0.2 atm

55. Glycerol boils at a slightly higher temperature than water. This reveals that glycerol’s attractive forces areA weaker than those of waterB the same as those of waterC nonexistentD stronger than those of water

56. Which of the following properties do solids share with liquidsA fluidityB definite shapeC definite volumeD slow rate of diffusion

57. Which term best describes the process by which particles escape from the surface of a non-boiling liquid and enter the gas state.A evaporation B. sublimation C. surface tension D.aeration

58. The particles in a liquid are usuallyA closer together and lower in energy than those in a gasB farther apart and higher in energy than those in a gasC closer together and lower in energy than those in a solidD farther apart and lower in energy than those in a solid

59. Two gases with unequal molar mass are injected into opposite ends of a long tube at the same time and allowed to diffuse toward the center. They should begin to mix A closer to the end that holds the heavier gasB in approximately 5 minutesC exactly in the middleD closer to the end that holds the lighter gas

60. What determines the average kinetic energy of the molecules of any gas?A container volumeB temperatureC molar massD pressure

61. According to the kinetic molecular theory, particles of matter A have different colorsB are in constant motionC have different shapesD are always fluid

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62.Which of the following is most likely a gas?

A B C

63. At a certain temperature and pressure, 0.2 mol of carbon dioxide has a volume of 3.1 L. A 3.1 L sample of hydrogen at the same temperature and pressure ______________A has a higher densityB contains the same number of atomsC contains the same number of moleculesD has the same mass

64. The equation for the production of methane is C + 2H2(g) CH4(g). How many liters of hydrogen are needed to produce 20.0 L of methane?A 20.0LB 2.0 LC 40 LD 22.4 L

65. The volume of gas is 400.0 mL when the pressure is 1.00 atm. At the same temperature, what is the pressure at which the volume of the gas is 2.0A 800 atmB 0.5 atmC 0.20 atmD 5.0 atm

66. A gas mixture is made up of oxygen, nitrogen and helium. According to the pie chart – if the total pressure of the mixture is 225 KPa, what is the partial pressure of oxygen. (He = 18%, Nit. = 34%, O2 = 48%)A 76.5 KPaB 225 KPaC 40.5 KPaD 108 KPa

67. How many times greater is the rate of effusion of oxygen than that of carbon dioxide gas at the same temperature and pressure. The molar mass of oxygen is 32.0 g/mol and the molar mass of carbon dioxide is 44.0 g/mol.A 1.173B 0.853C 2.173D 1.375

68. Spontaneous reactions are driven byA increasing enthalpy and increasing entropyB decreasing enthalpy and increasing entropyC increasing enthalpy and decreasing entropyD decreasing enthalpy and decreasing entropy

69. Which of the following best describes heat?A the energy transferred between samples of matter because of a difference in their temperatures

7B a measure of the average kinetic energy of the particles in a sample of matterC the energy stored in a sample of matterD bond energy

70. Which of the following has the highest entropy when produced in a reaction?A solid C gasB liquid D aqueous solution

71. Which of the following systems has the lowest entropy?A.salt dissolved in a container of water B.sand mixed in a container of waterC.oil floating in a container of waterD.a container of frozen water

72. What drives spontaneous reactions?A decreasing enthalpy and decreasing entropyB decreasing enthalpy and increasing entropyC increasing enthalpy and decreasing entropyD increasing enthalpy and increasing entropy

73. The quantity of energy released or absorbed as heat during a chemical reaction is called theA. enthalpy. C. entropy.B. heat of reaction. D. free energy.

74. Which of the following best describes enthalpy (H)? A. the total kinetic energy of a system B. the heat content of a chemical system C. the system's entropy D. the cell's energy equilibrium E. the condition of a cell that is not able to react 

75. When two solutions react the container “feels hot.” Thus,A. the reaction is endothermic.B. the reaction is exothermic.C. the energy of the universe is increased.D. the energy of both the system and the surroundings is decreased.

76. What is the energy released or absorbed as heat when one mole of a compound is produced by combination of its elements?

a.heat of formation c. free energyb.heat of combustion d. entropy

77. What does S stand for?a.enthalpy change c. entropy changeb.free energy change d. temperature change

78. Which of the following systems has the lowest entropy?a.salt dissolved in a container of water c. oil floating in a container of waterb.sand mixed in a container of water d. a container of frozen water

79. When a sugar cube is dissolved in a cup of tea, entropy isa. decreasingb. increasing and decreasingc. at equilibriumd. increasing

80. Two samples of iron, one with a mass of 50g and the other with a mass of 500g were placed in a boiling water bath at 1000C and were allowed to reach thermal equilibrium. What statement is true?

8a. The 50g piece has a higher temp.b. The 500g piece can transfer more heatc. The 500g piece has a higher temp.d. The 50g piece can transfer more heat

81. A reaction is spontaneous if Δ G isa. greater than Δ Hb. positivec. negatived. zero

82. Calculate the energy required to produce 7.0 mol Cl2O7 on the basis of the following balanced equation2Cl2(g) + 7O2(g) + 130 Cal

a. 460 Calb. 65 Calc. 19 Cald. 910 Cal

83. In an endothermic reaction, the total energy at the beginning of the reaction isa. equal to the total energy at the end of the reactionb. greater than the total energy at the end of the reactionc. less than the total energy at the end of the reactiond. None of the above

84. Two factors that determine whether a reaction will occur spontaneously are the change in the energy of a reaction system anda. the randomness of the particles in the systemb. the pressure of the systemc. the quickness of the reactiond. the concentration of the reactants in the system

85. Which of the following best describes energy in the form of heata. the energy transferred between samples of matter because of a difference in their temperatureb. a measure of the average kinetic energy of the particles in a sample of matterc. the energy stored in a sample of matter than can be emitted during combustion reactiond. bond energy

86. Given the equation I2(s) + 62.4 kJ I2(g), which of the following is truea. Δ H = + 62.4 kJb. The reaction releases heatc. Δ H = - 62.4 kJd. The reaction is exothermal

87. If the enthalpy involved in a chemical reaction has a negative signa. heat is gained from the surroundingsb. no heat is involved in the reactionc. heat is neither gained nor lostd. heat is lost to its surroundings

88. What is the enthalpy change, H for the following reaction2Mg(s) + SiCl4(l) Si(s) + 2MgCl2(s)

USE THE FOLLOWINGSi(s) + 2CL2(g) SiCl4(l) Δ H = -687 kJMg(s) + CL2(g) MgCL2 Δ H = -641 kJ

a. -595 kJb. -1328 kJc. 46 kJd. -1969 kJ

989. Standard conditions of temperature and pressure for a thermochemical equation are

a. 0oC & 101 KPab. 0oC & O KPac. 25oC & 101 KPad. 25oC & 22.4 KPa

90. Free energy change depends ona. change of enthalpy onlyb. temperature onlyc. temperate and changes of entropy and enthalpyd. change of entropy only

91. As a general rule, the entropy of a solid isa. more than that of a liquidb. zeroc. more than that of a gasd. less than that of a liquid

92. In a calorimeter, the energy content of a substance is calculated from measurement of the temperature change in a known mass ofa. iron b.air c.water d.steel

93. Suppose reaction A has a Δ H of -200 kJ and reaction B has a Δ H of -100 kJ. If reaction can be written as the sum of reaction A forward and reaction B reversed, what is Δ H for reaction C?a. +100 kJ b. +300 kJ c. -300 kJ d. -100 kJ

94. The majority of spontaneous chemical reaction in nature area. exothermicb. free energy reactionc. positive enthalpic reactiond. endothermic

95. The standard enthalpy of formation for an element in its natural form is equal toa. its molar massb. the standard entropy minus the temperaturec. its enthalpy of fusiond. zero kilojoules per mole

96.The amount of heat transferred from an object depends on which of the followinga. mass of the objectb. initial temperature of the objectc. specific heat of the objectd. all of the above

97. In the reaction below, entropy is 2H2(g) + O2(g) 2H2O(g)a. at equilibrium b. increasing c. equal to the enthalpy d. decreasing

98. In an exothermic reaction, the energy stored in the chemical bonds of the reactants isa. less than the heat releasedb. equal to the energy stored in the bonds of the productsc. less than the energy stored in the bond of the productsd. greater than the energy stored in the bonds of the products

99. Two objects are sitting next to each other in direct sunlight. Object A gets hotter than Object B. Choose the correct statement from the choices belowa. Can’t tell from the given informationb. Object A has a lower specific heat capacity than Object Bc. Both objects have the same specific heat capacityd. Object A has a higher specific heat capacity than Object B

10100. What would likely happen if you were to touch a flask in which an endothermic reaction were occurring

a. the flask would feel the same as before reaction startedb. the flask would feel warmer than before reaction startedc. the flask would feel cooler than before reaction startedd. None of the above

101. How does a calorie compare to a joulea.calorie is larger than a jouleb.calorie is smaller than a joulec.relationship can’t be determinedd.calorie is equal to a joule

102.If there are 4.187 J per calorie, what would be the equal of 15 caloriesa. 6300 J b. 63 J c. 63 kJ d. 3600 J

103. The heart required to change one mole of a substance from a solid to a liquid is called thea. Δ Hvap b. Δ Hcont c. Δ Hfus d. Δ Hsolid

104. Based on the chart of specific heat capacities, which element would require the most heat to raise one gram of a substance 10C?a. silver b. iron c. lead d. mercury

105. The vaporization of a substance is a(n) _________________ processa. polythermic b. exothermic c. ectothermic d. endothermic

106. Spontaneous reactions are driven bya. increasing enthalpy and increasing entropyb. decreasing enthalpy and increasing entropyc. increasing enthalpy and decreasing entropyd. decreasing enthalpy and decreasing entropy

107. 107.What is the volume occupied by 1 mol of oxygen at STP?a. 11.2 L c.22.4 Lb. 16.0 L d. 32.0 L