2 part gas law practice!!

Chemistry 1B Chapter 10 Worksheet - Daley

Name___________________________________

1) The National Weather Service routinelysupplies atmospheric pressure data to helppilots set their altimeters. The units the NWSuses for atmospheric pressure are inches ofmercury. A barometric pressure of 30.51inches of mercury corresponds to __________kPa.A) 103.3B) 77.50C) 775D) 1.020E) 16.01

2) A closed-end manometer was attached to avessel containing argon. The difference in themercury levels in the two arms of themanometer was 12.2 cm. Atmosphericpressure was 783 mmHg. The pressure of theargon in the container was __________mmHg.A) 882B) 661C) 122D) 795E) 771

3) A sample of gas (24.2 g) initially at 4.00 atmwas compressed from 8.00 L to 2.00 L atconstant temperature. After the compression,the gas pressure was __________ atm.A) 2.00B) 16.0C) 1.00D) 8.00E) 4.00

4) A balloon originally had a volume of 4.39 Lat 44 °C and a pressure of 729 torr. Theballoon must be cooled to __________°C toreduce its volume to 3.78 L (at constantpressure).A) 38B) 0C) 546D) 72.9E) 273

5) If 3.21 mol of a gas occupies 56.2 L at 44 °Cand 793 torr, 5.29 mol of this gas occupies__________ L under these conditions.A) 30.9B) 14.7C) 478D) 92.6E) 61.7

6) A gas originally at 27 °C and 1.00 atmpressure in a 3.9 L flask is cooled at constantpressure until the temperature is 11 °C. Thenew volume of the gas is __________ L.A) 0.27B) 0.24C) 3.9D) 4.1E) 3.7

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7) A sample of H2 gas (12.28 g) occupies 100.0 Lat 400.0 K and 2.00 atm. A sample weighing9.49 g occupies __________ L at 353 K and2.00 atm.A) 54.7B) 77.3C) 147D) 68.2E) 109

8) If 50.75 g of a gas occupies 10.0 L at STP, 129.3g of the gas will occupy __________ L at STP.A) 3.92B) 5.08C) 50.8D) 12.9E) 25.5

9) A sample of a gas originally at 25 °C and 1.00atm pressure in a 2.5 L container is allowed toexpand until the pressure is 0.85 atm and thetemperature is 15 °C. The final volume of thegas is __________ L.A) 2.1B) 2.8C) 3.0D) 0.38E) 2.6

10) The reaction of 50 mL of N2 gas with 150 mLof H2 gas to form ammonia via the equation:

N2 (g) + 3H2 (g) → 2NH3 (g)will produce __________ mL of ammonia ifpressure and temperature are kept constant.A) 50B) 150C) 200D) 250E) 100

11) The density of ammonia gas in a 4.32 Lcontainer at 837 torr and 45.0 °C is__________ g/L.A) 0.194B) 0.432C) 0.717D) 3.86

E) 4.22 × 10-2

12) A sample of gas (1.9 mol) is in a flask at 21 °Cand 697 mmHg. The flask is opened andmore gas is added to the flask. The newpressure is 795 mmHg and the temperature isnow 26 °C. There are now __________ mol ofgas in the flask.A) 3.5B) 1.6C) 2.9D) 0.28E) 2.1

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13) The density of N2O at 1.53 atm and 45.2 °C is__________ g/L.A) 1.76B) 2.58C) 9.99D) 18.2E) 0.388

14) The molecular weight of a gas is __________g/mol if 3.5 g of the gas occupies 2.1 L at STP.A) 2.7 × 10-2B) 41C) 5.5 × 103

D) 4.6 × 102E) 37

15) The volume of hydrogen gas at 38.0 °C and763 torr that can be produced by the reactionof 4.33 g of zinc with excess sulfuric acid is__________ L.A) 2.71 × 10-4B) 0.592C) 3.69 × 104D) 2.84E) 1.69

16) What volume (mL) of sulfur dioxide can beproduced by the complete reaction of 3.82 gof calcium sulfite with excess HCl (aq), whenthe final SO2 pressure is 827 torr at 44.0 °C?

A) 1.39 × 10-4

B) 1.00 × 10-3C) 761D) 578E) 0.106

17) Ammonium nitrite undergoes thermaldecomposition to produce only gases:

NH4NO2 (s) → N2 (g) + 2H2O (g)

What volume (L) of gas is produced by thedecomposition of 35.0 g of NH4NO2 (s) at525 ° C and 1.5 atm?A) 160B) 24C) 15D) 47E) 72

18) A sample of He gas (3.0 L) at 5.6 atm and 25°C was combined with 4.5 L of Ne gas at 3.6atm and 25 °C at constant temperature in a9.0 L flask. The total pressure in the flask was__________ atm. Assume the initial pressurein the flask was 0.00 atm.A) 1.0B) 3.7C) 9.2D) 24E) 2.6

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19) Since air is a mixture, it does not have a“molar mass.” However, for calculationpurposes, it is possible to speak of its“effective molar mass.” (An effective molarmass is a weighted average of the molarmasses of a mixture’s components.) If air atSTP has a density of 1.285 g/L, its effectivemolar mass is __________ g/mol.A) 26.9B) 31.4C) 28.8D) 34.4E) 30.0

20) In a gas mixture of He, Ne, and Ar with atotal pressure of 8.40 atm, the mole fractionof Ar is __________ if the partial pressures ofHe and Ne are 1.50 and 2.00 atm,respectively.A) 0.417B) 0.238C) 0.179D) 0.357E) 0.583

21) A gas mixture of Ne and Ar has a totalpressure of 4.00 atm and contains 16.0 mol ofgas. If the partial pressure of Ne is 2.75 atm,how many moles of Ar are in the mixture?A) 5.00B) 11.0C) 6.75D) 12.0E) 9.25

22) Sodium hydride reacts with excess water toproduce aqueous sodium hydroxide andhydrogen gas:

NaH (s) + H2O (l) → NaOH (aq) +H2 (g)

A sample of NaH weighing __________ g willproduce 982 mL of gas at 28.0 °C and 765torr, when the hydrogen is collected overwater. The vapor pressure of water at thistemperature is 28 torr.A) 0.960B) 2.93C) 0.925D) 925E) 0.0388

23) CO (5.00 g) and CO2 (5.00 g) were placed in a750.0 mL container at 50.0 °C. The partialpressure of CO2 in the container was__________ atm.A) 1.60B) 4.01C) 6.31D) 10.3E) 0.292

24) The root-mean-square speed of CO at 113 °Cis __________ m/s.A) 58.3B) 586C) 31.5D) 317E) 993

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25) Which of the following statements aboutgases is false?A) Distances between molecules of gas arevery large compared to bond distanceswithin molecules.

B) Non-reacting gas mixtures arehomogeneous.

C) Gases expand spontaneously to fill thecontainer they are placed in.

D) Gases are highly compressible.E) All gases are colorless and odorless atroom temperature.

26) Molecular compounds of low molecularweight tend to be gases at room temperature.Which of the following is most likely not agas at room temperature?A) LiClB) CH4C) H2D) HClE) Cl2

27) Gaseous mixtures __________.A) are all heterogeneousB) can only contain isolated atomsC) are all homogeneousD) can only contain moleculesE) must contain both isolated atoms andmolecules

28) Standard temperature and pressure (STP), inthe context of gases, refers to __________.A) 273 K and 1 pascalB) 298 K and 1 torrC) 273 K and 1 atmD) 273 K and 1 torrE) 298 K and 1 atm

29) The molar volume of a gas at STP is__________ L.A) 14.7B) 0.08206C) 62.36D) 1.00E) 22.4

30) “Isothermal” means __________.A) at constant pressureB) at ideal temperature and pressureconditions

C) at constant temperatureD) that ΔHrxn = 0E) at variable temperature and pressureconditions

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31) The pressure exerted by a column of liquid isequal to the product of the height of thecolumn times the gravitational constant timesthe density of the liquid, P = ghd. How higha column of water (d = 1.0 g/mL) would besupported by a pressure that supports a 713mm column of mercury (d = 13.6 g/mL)?A) 9.7 × 103 mmB) 14 mmC) 713 mmD) 1.2 × 104 mmE) 52 mm

32) Which statement about atmospheric pressureis false?A) Atmospheric pressure prevents waterin lakes, rivers, and oceans fromboiling away.

B) With an increase in altitude,atmospheric pressure increases as well.

C) The warmer the air, the lower theatmospheric pressure.

D) Air actually has weight.E) As air becomes thinner, its densitydecreases.

33) The kinetic-molecular theory predicts thatpressure rises as the temperature of a gasincreases because __________.A) the gas molecules collide morefrequently with the wall

B) the gas molecules collide lessfrequently with the wall

C) the gas molecules collide moreenergetically with the wall

D) the average kinetic energy of the gasmolecules decreases

E) both the gas molecules collide morefrequently with the wall and the gasmolecules collide more energeticallywith the wall

34) A 255 mL round-bottom flask is weighed andfound to have a mass of 114.85 g. A fewmilliliters of an easily vaporized liquid areadded to the flask and the flask is immersedin a boiling water bath. All of the liquidvaporizes at the boiling temperature ofwater, filling the flask with vapor. When allof the liquid has vaporized, the flask isremoved from the bath, cooled, dried, andreweighed. The new mass of the flask andthe condensed vapor is 115.23 g. Which ofthe following compounds could the liquidbe? (Assume the ambient pressure is 1 atm.)A) C2H6B) C3H7OHC) C4H9OHD) C2H5OHE) C4H10

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35) The average kinetic energy of the particles ofa gas is directly proportional to __________.A) the particle massB) the square of the rms speedC) the square of the particle massD) the rms speedE) the square root of the rms speed

36) According to kinetic-molecular theory, inwhich of the following gases will theroot-mean-square speed of the molecules bethe highest at 200 °C?A) H2OB) SF6C) HClD) Cl2E) None. The molecules of all gases havethe same root-mean-square speed atany given temperature.

37) According to kinetic-molecular theory, if thetemperature of a gas is raised from 100 °C to200 °C, the average kinetic energy of the gaswill __________.A) decrease by a factor of 100B) increase by a factor of 100C) increase by a factor of 1.27D) decrease by halfE) double

38) Which one of the following gases would havethe highest average molecular speed at 25°C?A) O2B) SF6C) CO2D) CH4E) N2

39) A 1.44-g sample of an unknown pure gasoccupies a volume of 0.335 L at a pressure of1.00 atm and a temperature of 100.0 °C. Theunknown gas is __________.A) argonB) heliumC) kryptonD) xenonE) neon

40) Given the equationC2H6 (g) + O2 (g) → CO2 (g) + H2O (g)

Determine the number of liters of O2consumed at STP when 270.0 grams of C2H6is burned.

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Answer KeyTestname: CHAPTER 10 WORKSHEET

1) APage Ref: Sec. 10.2

2) CPage Ref: Sec. 10.2

3) BPage Ref: Sec. 10.3


5) DPage Ref: Sec. 10.3

6) EPage Ref: Sec. 10.3


























32) BPage Ref: Sec. 10.2, 10.3








40) 706Page Ref: Sec. 10.5

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(PRACTICE TEST CONTINUED)

a) H2

b) He c) O2 d) N2 e) CO2

40. At a given temperature, this has the highest rate of diffusion.

41. This gas is the most plentiful in the earth’s atmosphere.

42. 1 mole of this occupying 1 liter would have the largest density.

43. Nitrogen gas was collected over water at a temperature of 40° C, and the pressure of the sample was measured at 796 mm Hg. If the vapor pressure of water at 40° C is 55 mm Hg, what is the partial pressure of the nitrogen gas?

a) 756 mm Hgb) 796 mm Hgc) 851 mm Hg d) 741 mm Hge) 55 mm Hg

44. An experiment to determine the molecular mass of a gas begins by heating a solid to produce a gaseous product. The gas passes through a tube and displaces water in an inverted, water-filled bottle. Which of the following necessary items may be determined after the experiment is completed?

a) mass of the solid usedb) vapor pressure of waterc) temperature of the displaced waterd) volume of the displaced watere) barometric pressure in the room

45. Determine the formula for a gaseous silane (SinH2n+2) if it has a density of 5.47 g per L at 0 C and 1.00 atm.

a) Si5H12

b) SiH4

c) Si4H10

d) Si3H8

e) Si2H6

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46. A sample of methane gas was collected over water at 35 C. The sample was found to have a total pressure of 756 mm Hg. Determine the partial pressure of the methane gas in the sample (vapor pressure of water at 35 C is 41 mm Hg).

a) 797 mm Hgb) 760 mm Hgc) 41 mm Hgd) 756 mm Hge) 715 mm Hg

47. A sample of argon gas is sealed in a container. The volume of the container is doubled. If the pressure remains constant, what happens to the absolute temperature?

a) It is doubled.b) It is squared. c) No change. d) It is halved. e) It cannot be predicted.

48. A gas sample is confined in a 5-liter container. Which of the following will occur if the temperature of the container is increased?

I. The kinetic energy of the gas will increase.II. The pressure of the gas will increase.III. The density of the gas will increase.

a) I onlyb) I and II onlyc) II onlyd) I and III onlye) I, II and III

49. Increasing the temperature of an ideal gas from 50 C to 75 C at constant volume will cause which of the following to increase for the gas?

I. the average distance between the moleculesII. the average speed of the moleculesIII. the average molecular mass of the gas.

a) I and IIb) II only c) II and IIId) I only e) III only

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50. A 22.0 gram sample of an unknown gas occupies 11.2 liters at standard temperature and pressure. Which of the following could be the identity of the gas?

a) carbon dioxide gasb) helium gas c) sulfur trioxide gasd) oxygen gase) nitrogen gas

51. The true volume of a particular real gas is larger than that calculated from the ideal gas equation. This occurs because the ideal gas equation is NOT correct for:

a) the shape of the moleculesb) the speed the molecules are movingc) the mass of the moleculesd) the attraction between the moleculese) the volume of the molecules

52. Two balloons are at the same temperature and pressure. One contains 14 g of nitrogen and the other contains 20.0 g of argon. All of the following statements are true EXCEPT

a) The density of the nitrogen sample is less than the density of the argon sample.b) The average kinetic energy of the nitrogen molecules is the same as the average kinetic

energy of the argon molecules.c) The volume of the nitrogen container is the same as the volume of the argon container.d) The average speed of the nitrogen molecules is the same as the average speed of the

argon molecules.e) The number of molecules in the nitrogen container is the same as the number of atoms in

the argon container.

53. Nitrogen gas was collected over water at 25°C. If the vapor pressure of water at 25°C is 23 mm Hg, and the total pressure in the container is measured at 781 mm Hg, what is the partial pressure of the nitrogen gas?


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54. Which of the following expressions is equal to the density of helium gas at standard temperature and pressure?

a)

b)

c)

d)

e)

55. Which of the following conditions would be most likely to cause the ideal gas laws to fail?

I. High pressureII. High temperature III. Large volume

a) I onlyb) II only c) I and III only d) I and II only e) II and III only

56. Aluminum metal reacts with HCl to produce aluminum chloride and hydrogen gas. How many grams of aluminum metal must be added to an excess of HCl to produce 33.6 L of hydrogen gas, if the gas is at STP?

a) 18.0 gb) 4.50 gc) 27.0 gd) 9.00 ge) 35.0 g

57. A glass container is filled, at room temperature, with equal numbers of moles of H2(g), O2(g), and NO2(g). The gases slowly leak out through a pinhole. After some of the gas has effused, which of the following is true of the relative values for the partial pressures of the gases remaining in the container?

a) O2 < NO2 < H2

b) H2 = NO2 = O2

c) H2 < O2 < NO2

d) NO2 < H2 < O2

e) H2 < NO2 < O2

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58. Ideal gases vary from real gases at conditions of

a) high temperature and low pressure. b) low temperature and low pressure.c) low temperature and high pressure.d) high temperature and high pressure. e) both high density and low pressure.

59. The average kinetic energy of nitrogen molecules changes by what factor when the temperature is increased from 30C to 60C?

a) square root of (333 - 303)b) 2c) 0.5d) (333 – 303)e) 28

60. Which of the following gases probably deviates most considerably from ideal gas behavior?

a) O2

b) SF4

c) SiH4

d) Hee) Ar

61. A 14.0-L cylinder contains 5.60 g N2, 79.9 g Ar and 6.40 g 02. What is the total pressure in atm at 27°C? (R =the ideal gas constant.)

a) 120 R b) 26 Rc) 30 Rd) 20 R e) 60 R

62. Which of the following assumptions is/are valid based on kinetic molecular theory?

a) Gas molecules have negligible volume. b) Gas molecules exert no attractive forces on one another c) The temperature of a gas in celcius is directly proportional to its kinetic energy. d) All of the above e) Only a and b

63. Which of the following best explains why a hotair balloon rises?

a) The heating of the air causes the pressure inside the balloon to increase.b) The temperature difference between the inside and outside air causes convection currents.c) Hot air has a lower density than cold air.d) Cooler air diffuses more slowly than the warmer air.e) The cool outside air pushes the balloon higher.

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64. In an experiment H2(g) and O2(g) were completely reacted, above the boiling point of water. If the initial pressure in the container before the reaction is denoted as x , which of the following expressions gives the final pressure, assuming ideal gas behavior?

a) 1.5xb) 2xc) xd) (0.6666666666.....)xe) 0.5x

65. An ideal gas of volume 189. mL is collected over water at 30°C and 777 torr. The vapor pressure of water is 32 torr@ 30°C. What pressure is exerted by the dry gas under these conditions?

a) 777 torrb) 32 x 777 torrc) 745 torrd) 32/77 torre) 320 torr

66. An ideal gas sample weighing 1.28 grams at 127C and 1.00 atm has a volume of 0.250 L. Determine the molar mass of the gas.

a) 80.5 g/molb) 0.00621 g/molc) 322 g/mold) 168 g/mole) 49.4 g/mol

67. When 4.0 moles of oxygen are confined in a 24-liter vessel at 176°C, the pressure is 6.0 atm. If the oxygen is allowed to expand isothermally until it occupies 36 liters, what will be the new pressure?

a) 2 atmb) 4 atmc) 3 atmd) 9 atme) 8 atm

68. A sealed container containing 8.0 grams of oxygen gas and 7.0 of nitrogen gas is kept at a constant temperature and pressure. Which of the following is true?

a) The density of nitrogen is greater than the density of oxygen.b) The volume occupied by nitrogen is greater than the volume occupied by oxygen.c) The volume occupied by oxygen is greater than the volume occupied by nitrogen.d) The average molecular speeds of the two gases are the same.e) The volume occupied by oxygen is equal to the volume occupied by nitrogen

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69. An ideal gas is contained in a 5.0 liter chamber at a temperature of 37°C. If the gas exerts a pressure of 2.0 atm on the walls of the chamber, which of the following expressions is equal to the number of moles of the gas? The gas constant, R, is 0.08 (L-atm)/(mol-K).

a)

b)

c)

d)

e)

70. A 2 L evacuated flask has a 0.2 mol sample of NO5(s) sealed inside it. The flask is heated to decompose the solid and cooled to 300 K. What is the nearest value to the final total pressure of the gases in the flask? (The value of the gas constant, R, is 0.082 L atm mol-1K-1.)

a) 0.6 atmb) 3 atmc) 0.05 atmd) 1.2 atme) 6 atm

71. A gas sample contains 0.1 mole of oxygen and 0.4 moles of nitrogen. If the sample is at standard temperature and pressure, what is the partial pressure due to nitrogen?

a) 0.2 atmb) 0.1 atmc) 0.8 atmd) 0.5 atme) 1.0 atm

72. If a sample of CH4 effuses at a rate of 9.0 mol per hour at 35C, which of the gases below will effuse at approximately twice the rate under the same conditions?

a) COb) F2

c) SiH4

d) O2

e) He

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73. A mixture of gases contains 1.5 moles of oxygen, 3.0 moles of nitrogen, and 0.5 moles of water vapor. If the total pressure is 700 mm Hg, what is the partial pressure of the nitrogen gas?


74. A balloon occupies a volume of 1.0 liter when it contains 0.16 grams of helium at 37° C and 1 atm pressure. If helium is added to the balloon until it contains 0.80 grams while pressure and temperature are kept constant, what will be the new volume of the balloon?

a) 0.50 litersb) 1.0 litersc) 4.0 litersd) 2.0 literse) 5.0 liters

75. A reaction produces a gaseous mixture of carbon dioxide, carbon monoxide, and water vapor. After one reaction, the mixture was analyzed and found to contain 0.60 mol of carbon dioxide, 0.30 mol of carbon monoxide, and 0.10 mol of water vapor. If the total pressure of the mixture was 0.80 atm, what was the partial pressure of the carbon monoxide?


76. Which of the following gases would be expected to have a rate of effusion that is one-third as large as that of H2?

a) O2

b) CO2

c) Hed) N2

e) H2O

77. A gaseous mixture at a constant temperature contains O2, CO2, and He. Which of the following lists the three gases in order of increasing average molecular speeds?

a) He, CO2, O2

b) He, O2, CO2

c) O2, CO2, Hed) O2, He, CO2

e) CO2, O2, He

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78. A sealed, rigid container is filled with three ideal gases: A, B, and C. The partial pressure of each gas is known. The temperature and volume of the system are known. What additional information is needed to determine the masses of the gases in the container?

a) the molar masses of the gasesb) the total pressurec) the volume of the gas moleculesd) the intermolecular forcese) the average distance traveled between molecular collisions

79. What is the volume of n moles of gas@ STP?

a) 22.4 Lb) n X 22.4 Lc) n X 22.4 L X 760 d) n X 22.4 LL X 273 X 760e) Cannot be determined.

80. A mixture of helium and neon gases has a total pressure of 1.2 atm. If the mixture contains twice as many moles of helium as neon, what is the partial pressure due to neon?


81. A steel tank containing argon gas has additional argon gas pumped into it at constant temperature. Which of the following is true for the gas in the tank?

a) There is an increase in the volume of the gas.b) The gas atoms travel with the same average speed.c) The gas atoms are separated by a greater average distance.d) There is no change in the number of gas atoms.e) There is a decrease in the pressure exerted by the gas.

82. An ideal gas fills a balloon at a temperature of 27°C and 1 atm pressure. By what factor will the volume of the balloon change if the gas in the balloon is heated to 127°C at constant pressure?

a) 4/3b) 4.703703703703..... c) 2d) 0.75e) 27/127

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83. A gas sample with a mass of 10 grams occupies 6.0 liters and exerts a pressure of 2.0 atm at a temperature of 26°C. Which of the following expressions is equal to the molecular mass of the gas? The gas constant, R, is 0.08 (L-atm)/(mol-K).

a)

b)

c)

d)

e)

84. The temperature of a sample of an ideal gas confined in a 2.0 L container was raised from 27°C to 77°C. If the initial pressure of the gas was 1,200 mm Hg, what was the final pressure of the gas?

a) 1,400 mm Hgb) 600 mm Hgc) 3,600 mm Hgd) 2,400 mm Hge) 300 mm Hg

85. In a closed inflexible system, 7.0 mol CO2, 7.0 mol Ar, 7.0 mol N2, and 4.0 mol Ne are trapped, with a total pressure of 10.0 atm. What is the partial pressure exerted by the neon gas?

a) 1.6 atmb) 29.0 atm c) 4.0 atmd) 10.0 atm e) 21.0 atm

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Short Answer

86. A hydrogen gas sample is collected over water. The volume of the sample was 190.0 mL at 26 C, and the pressure in the room was 754 mm Hg. The vapor pressure of water at 26 C is 25.2 mm Hg.

(a) Calculate the number of moles of hydrogen in the sample.

(b) Calculate how many molecules of water vapor are present in the sample.

(c) Determine the density (in g/L) of the gas mixture.

(d) determine the mole fraction of water.

87. A sample containing 2/3 mole of potassium chlorate, KClO3, is heated until it decomposes to potassium chloride and oxygen gas. The oxygen is collected in an inverted bottle through the displacement of water. Answer the following questions using this information.

(a) Write a balanced chemical equation for the reaction.

(b) How many moles of oxygen gas are produced?

(c) The temperature and pressure of the sample are adjusted to STP. The volume of the sample is found to be slightly greater than 22.4 liters. Explain.

(d) An excess of sulfur is burned in the oxygen. Write a balanced chemical equationand calculate the number of moles of gas formed.

(e) After the sulfur had completely reacted, a sample of the residual water was removed from the bottle and found to be acidic. Explain.

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88.

The graph above shows the changes in pressure with changing temperature of gas samples of helium and argon confined in a closed 2-liter vessel.

(a) What is the total pressure of the two gases in the container at a temperature of 200 K?

(b) How many moles of helium are contained in the vessel?

(c) How many molecules of helium are contained in the vessel?

(d) What is the ratio of the average speeds of the helium atoms to the average speeds of the argon atoms?

(e) If the volume of the container were reduced to 1 liter at a constant temperature of 300 K, what would be the new pressure of the helium gas?

89. Equal molar quantities of two gases, O2 and H2O, are confined in a closed vessel at constant temperature.

(a)Which gas, if any, has the greater partial pressure?

(b)Which gas, if any, has the greater density

(c) Which gas, if any, has the greater concentration?

(d) Which gas, if any, has the greater average kinetic energy?

(e) Which gas, if any, will show the greater deviation from ideal behavior?

(f) Which gas, if any, has the greater average molecular speed?

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90. SF6, H2O, and CO2 are all greenhouse gases because they absorb infrared radiation in the atmosphere. As such they are of interest to many researchers.

(a) Of the three gases, which deviates the most from ideal gas behavior?

(b) If all three ideal gases are held at constant temperature, which gas would have the highest average molecular speed?

(c) A container was with equal amounts H2O and CO2 and the pressure was measured. Assuming ideal behavior, if SF6 was then added such that the final pressure was four times that before its addition, the final number of moles of SF6 is how many times that of H2O?

(d) If a container held equal molar amounts of all three greenhouse gases, but was then compressed decreasing the volume within, which of the gases has the highest, final partial pressure assuming ideal behavior.

(e) Gas molecules exert pressure through collisions with the walls of the containers they are in. If a container is filled with equal amounts of each of the greenhouse gases, which gas undergoes the fewest collisions with the wall of the container per unit time?

ID: A

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(PRACTICE TEST CONTINUED)

Answer Section

MATCHING

40. A 41. D 42. E

MULTIPLE CHOICE

43. D 44. B 45. C 46. E 47. A 48. B 49. B 50. A 51. E 52. D 53. A 54. D 55. A 56. C 57. C 58. C 59. D 60. B 61. C 62. E 63. C 64. D 65. C 66. D 67. B 68. E 69. E 70. E 71. C 72. E 73. E 74. E 75. D

ID: A

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76. E 77. E 78. A 79. B 80. E 81. B 82. A 83. C 84. A 85. A

ID: A

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SHORT ANSWER

86.

ID: A

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87.

ID: A

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88.

ID: A

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89.

ID: A

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90.

2 part gas law practice!!

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