5) Gaseous mixtures ________.

A) can only contain molecules

B) are all heterogeneous

C) can only contain isolated atoms

D) are all homogeneous

E) must contain both isolated atoms and molecules

D) are all homogeneous

6) Which of the following equations shows an incorrect relationship between pressures given in terms of different units?

A) 1.20 atm = 122 kPa

B) 152 mm Hg = 2.03 × 104 Pa

C) 0.760 atm = 578 mm Hg

D) 1.0 torr = 2.00 mm Hg

E) 1.00 atm = 760 torr

D) 1.0 torr = 2.00 mm Hg

7) The pressure exerted by a column of liquid is equal to the product of the height of the column times the gravitational constant times the density of the liquid, P = ghd. How high a column of water (d = 1.0 g/mL) would be supported by a pressure that supports a 713 mm column of mercury (d = 13.6 g/mL)?

A) 14 mm

B) 52 mm

C) 713 mm

D) 1.2 × 10⁴ mm

E) 9.7 × 10³ mm

E) 9.7 × 10³ mm

8) The pressure exerted by a column of liquid is equal to the product of the height of the column times the gravitational constant times the density of the liquid, P = ghd. How high a column of methanol
(d = 0.79 g/mL) would be supported by a pressure that supports a 713 mm column of mercury
(d = 13.6 g/mL)?

A) 713 mm

B) 41 mm

C) 1.2 × 10⁴ mm

D) 9.7 × 10³ mm

E) 17 mm

C) 1.2 × 10⁴ mm

9) Which statement about atmospheric pressure is false?

A) As air becomes thinner, its density decreases.

B) Air actually has weight.

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

D) The warmer the air, the lower the atmospheric pressure.

E) Atmospheric pressure prevents water in lakes, rivers, and oceans from boiling away.

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

10) In ideal gas equation calculations, expressing pressure in Pascals (Pa), necessitates the use of the gas constant, R, equal to ________.

A) 0.08206 atm L mol-1K-1

B) 8.314 -Pa/mol-K

C) 62.36 L torr mol-1K-1

D) 1.987 cal mol-1K-1

E) none of the above

B) 8.314 -Pa/mol-K

11) The first person to investigate the relationship between the pressure of a gas and its volume was ________.

A) Amadeo Avogadro

B) Lord Kelvin

C) Jacques Charles

D) Robert Boyle

E) Joseph Louis Gay-Lussac

D) Robert Boyle

12) Of the following, ________ is a correct statement of Boyle's law.

A) PV = constant

B)_v ^P = constant

C) V/P= constant

D) V/T= constant

E) n/P= constant

A) PV = constant

13) "Isothermal" means ________.

A) at constant pressure

B) at constant temperature

C) at variable temperature and pressure conditions

D) at ideal temperature and pressure conditions

E) that ΔHrxn = 0

B) at constant temperature

14) Of the following, ________ is a valid statement of Charles' law.

A)P/T = constant

B)V/T = constant

C) PV = constant

D) V = constant × n

E) V = constant × P

B)V/T = constant

15) Which one of the following is a valid statement of Avogadro's law?

A) P/T = constant

B) V/T= constant

C) PV = constant

D) V = constant × n

E) V = constant × P

D) V = constant × n

16) Of the following, only ________ is impossible for an ideal gas.

A) V₁/T₁=V₂/T₂

B)V₁T₁ = V₂T₂

C) V₁/V₂=T₁/T₂

D)V₂ =T₂/T₁^V¹

E) V₁/V₂=T₁/T₂ = 0

B)V₁T₁ = V₂T₂

17) The molar volume of a gas at STP is ________ L.

A) 0.08206

B) 62.36

C) 1.00

D) 22.4

E) 14.7

D) 22.4

18) Standard temperature and pressure (STP), in the context of gases, refers to ________.

A) 298.15 K and 1 atm

B) 273.15 K and 1 atm

C) 298.15 K and 1 torr

D) 273.15 K and 1 pascal

E) 273.15 K and 1 torr

B) 273.15 K and 1 atm

19) Sodium bicarbonate is reacted with concentrated hydrochloric acid at 37.0 °C and 1.00 atm. The reaction of 6.00 kg of bicarbonate with excess hydrochloric acid under these conditions will produce ________ L of CO2.

A) 1.09 × 10²

B) 2.85 × 10⁴

C) 1.82 × 10⁴

D) 8.70 × 10²

E) 1.82 × 10³

E) 1.82 × 10³

20) Sodium bicarbonate is reacted with concentrated hydrochloric acid at 25.0 °C and 1.50 atm. The reaction of 7.75 kg of bicarbonate with excess hydrochloric acid under these conditions will produce ________ L of CO2.

A) 1.82 × 10³

B) 2.85 × 10⁴

C) 1.82 × 10⁴

D) 1.50 × 10³

E) 8.70 × 10²

D) 1.50 × 10³

21) The volume of a sample of gas (2.49 g) was 752 mL at 1.98 atm and 62 °C. The gas is ________.

A) SO₂

B) SO₃

C) NH₃

D) NO₂

E) Ne

D) NO₂

22) The density of NO2 in a 4.50 L tank at 760.0 torr and 25.0 °C is ________ g/L.

A) 1.64

B) 9.30

C) 1.68

D) 1.88

E) 3.27

D) 1.88

23) The density of air at STP is 1.285 g/L. Which of the following cannot be used to fill a balloon that will float in air at STP?

A) CH₄

B) NO

C) Ne

D) NH₃

E) HF

B) NO

24) The average kinetic energy of the particles of a gas is directly proportional to ________.

A) the rms speed

B) the square of the rms speed

C) the square root of the rms speed

D) the square of the particle mass

E) the particle mass

B) the square of the rms speed

25) The kinetic-molecular theory predicts that pressure rises as the temperature of a gas increases because ________.

A) the average kinetic energy of the gas molecules decreases

B) the gas molecules collide more frequently with the wall

C) the gas molecules collide less frequently with the wall

D) the gas molecules collide more energetically with the wall

E) both the gas molecules collide more frequently with the wall and the gas molecules collide more energetically with the wall

E) both the gas molecules collide more frequently with the wall and the gas molecules collide more energetically with the wall

26) According to kinetic-molecular theory, in which of the following gases will the root-mean-square speed of the molecules be the highest at 200 °C?

A) HCl

B) Cl₂

C)H₂O

D) SF₆

E) None. The molecules of all gases have the same root-mean-square speed at any given temperature.

C)H₂O

27) According to kinetic-molecular theory, if the temperature of a gas is raised from 100 °C to 200 °C, the average kinetic energy of the gas will ________.

A) double

B) increase by a factor of 1.27

C) increase by a factor of 100

D) decrease by half

E) decrease by a factor of 100

A) double

28) Which of the following is not part of the kinetic-molecular theory?

A) Atoms are neither created nor destroyed by ordinary chemical reactions.

B) Attractive and repulsive forces between gas molecules are negligible.

C) Gases consist of molecules in continuous, random motion.

D) Collisions between gas molecules do not result in the loss of energy.

E) The volume occupied by all of the gas molecules in a container is negligible compared to the volume of the container.

A) Atoms are neither created nor destroyed by ordinary chemical reactions.

29) Of the following gases, ________ will have the greatest rate of effusion at a given temperature.

A) NH₃

B) CH₄

C) Ar

D) HBr

E) HCl

B) CH₄

30) A tank containing both HF and HBr gases developed a leak. The ratio of the rate of effusion of HF to the rate of effusion of HBr is ________.

A) 4.04

B) 0.247

C) 2.01

D) 0.497

E) 16.3

C) 2.01

31) At STP, the ratio of the root-mean-square speed of CO2 to that of SO2 is ________.

A) 2.001

B) 2.119

C) 1.000

D) 1.207

E) 1.456

D) 1.207

32) Arrange the following gases in order of increasing average molecular speed at 25 °C.

Cl2, O2, F2, N2

A) Cl2 < F2 < O2 < N2

B) Cl2 < O2 < F2 < N2

C) N2 < F2 < Cl2 < O2

D) Cl2 < F2 < N2 < O2

E) F2 < O2 < N2 < Cl2

A) Cl2 < F2 < O2 < N2

33) A sample of oxygen gas (O2) was found to effuse at a rate equal to three times that of an unknown gas. The molecular weight of the unknown gas is ________ g/mol.

A) 288

B) 96

C) 55

D) 4

E) 10.7

A) 288

34) A mixture of carbon dioxide and an unknown gas was allowed to effuse from a container. The carbon dioxide took 1.25 times as long to escape as the unknown gas. Which one could be the unknown gas?

A) Cl₂

B) CO

C) HCl

D) H₂

E) SO₂

B) CO

35) An ideal gas differs from a real gas in that the molecules of an ideal gas ________.

A) have no attraction for one another

B) have appreciable molecular volumes

C) have a molecular weight of zero

D) have no kinetic energy

E) have an average molecular mass

A) have no attraction for one another

36) A real gas will behave most like an ideal gas under conditions of ________.

A) high temperature and high pressure

B) high temperature and low pressure

C) low temperature and high pressure

D) low temperature and low pressure

E) STP

B) high temperature and low pressure

37) Which noble gas is expected to show the largest deviations from the ideal gas behavior?

A) helium

B) neon

C) argon

D) krypton

E) xenon

E) xenon

38) The van der Waals equation for real gases recognizes that ________.

A) gas particles have non-zero volumes and interact with each other

B) molar volumes of gases of different types are different

C) the non-zero volumes of gas particles effectively decrease the amount of "empty space" between them

D) the molecular attractions between particles of gas decreases the pressure exerted by the gas

E) all of the above statements are true

A) gas particles have non-zero volumes and interact with each other

39) When gases are treated as real, via use of the van der Waals equation, the actual volume occupied by gas molecules ________ the pressure exerted and the attractive forces between gas molecules ________ the pressure exerted, as compared to an ideal gas.

A) decreases, increases

B) increases, increases

C) increases, decreases

D) does not affect, decreases

E) does not affect, increases

C) increases, decreases

40) A gas at a pressure of 10.0 Pa exerts a force of ________ N on an area of 5.5 m2.

A) 55

B) 0.55

C) 5.5

D) 1.8

E) 18

A) 55

41) A gas at a pressure of 325 torr exerts a force of ________ N on an area of 5.5 m2.

A) 1.8 × 10³

B) 59

C) 2.4 × 10⁵

D) 0.018

E) 2.4

C) 2.4 × 10⁵

42) A gas vessel is attached to an open-end manometer containing a nonvolatile liquid of density 0.791 g/mL as shown below.

The difference in heights of the liquid in the two sides of the manometer is 43.4 cm when the atmospheric pressure is 755 mm Hg. Given that the density of mercury is 13.6 g/mL, the pressure of the enclosed gas is ________ atm.

A) 1.03

B) 0.967

C) 0.993

D) 0.990

E) 0.987

B) 0.967

43) A gas vessel is attached to an open-end manometer filled with a nonvolatile liquid of density 0.993 g/mL as shown below.

The difference in heights of the liquid in the two sides of the manometer is 32.3 mm when the atmospheric pressure is 765 mm Hg. Given that the density of mercury is 13.6 g/mL, the pressure of the enclosed gas is ________ atm.

A) 1.05

B) 1.01

C) 0.976

D) 0.993

E) 1.08

A) 1.05

44) A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10 L to 15 L. The final pressure is ________ atm.

A) 1.5

B) 7.5

C) 0.67

D) 3.3

E) 15

C) 0.67

45) If 50.75 g of a gas occupies 10.0 L at STP, 129.3 g of the gas will occupy ________ L at STP.

A) 3.92

B) 50.8

C) 12.9

D) 25.5

E) 5.08

D) 25.5

46) A sample of H2 gas (12.28 g) occupies 100.0 L at 400.0 K and 2.00 atm. A sample weighing 9.49 g occupies ________ L at 353 K and 2.00 atm.

A) 109

B) 68.2

C) 54.7

D) 147

E) 77.3

B) 68.2

47) A sample of a gas (1.50 mol) is contained in a 15.0 L cylinder. The temperature is increased from 100 °C to 150 °C. The ratio of final pressure to initial pressure [P₂/P₁ ] is ________.

A) 1.50

B) 0.667

C) 0.882

D) 1.13

E) 1.00

D) 1.13

48) A sample of a gas originally at 25 °C and 1.00 atm pressure in a 2.5 L container is subject to a pressure of 0.85 atm and a temperature of 15 °C. The final volume of the gas is ________ L.

A) 3.0

B) 2.8

C) 2.6

D) 2.1

E) 0.38

B) 2.8

49) A sample of a gas originally at 29 °C and 1.25 atm pressure in a 3.0 L container is allowed to contract until the volume is 2.2 L and the temperature is 11 °C. The final pressure of the gas is ________ atm.

A) 2.9

B) 2.8

C) 1.6

D) 2.1

E) 0.38

C) 1.6

50) The amount of gas that occupies 60.82 L at 31.0 °C and 367 mm Hg is ________ mol.

A) 1.18

B) 0.850

C) 894

D) 11.6

E) 0.120

A) 1.18