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Ch 10: Chem Study Packet

front 1

1) Which of the following statements about gases is false?

A) Gases are highly compressible.

B) Distances between molecules of gas are very large compared to bond distances within molecules.

C) Non-reacting gas mixtures are homogeneous.

D) Gases expand spontaneously to fill the container they are placed in.

E) All gases are colorless and odorless at room temperature.

back 1

E) All gases are colorless and odorless at room temperature.

front 2

2) Of the following, ________ has a slight odor of bitter almonds and is toxic.

A) NH3

B) N2O

C) CO

D) CH4

E) HCN

back 2

E) HCN

front 3

3) Of the following, ________ has the odor of rotten eggs.

A) NH3

B) H2S

C) CO

D) NO2

E) HCN

back 3

B) H2S

front 4

4) One significant difference between gases and liquids is that ________.

A) a gas is made up of molecules

B) a gas expands to fill its container

C) a gas may consist of both elements and compounds

D) gases are always mixtures

E) All of the above answers are correct.

back 4

B) a gas expands to fill its container

front 5

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

back 5

D) are all homogeneous

front 6

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

back 6

D) 1.0 torr = 2.00 mm Hg

front 7

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

back 7

E) 9.7 × 103 mm

front 8

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

back 8

C) 1.2 × 104 mm

front 9

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.

back 9

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

front 10

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

back 10

B) 8.314 -Pa/mol-K

front 11

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

back 11

D) Robert Boyle

front 12

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

back 12

A) PV = constant

front 13

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

back 13

B) at constant temperature

front 14

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

back 14

B)V/T = constant

front 15

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

back 15

D) V = constant × n

front 16

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

back 16

B)V1T1 = V2T2

front 17

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

back 17

D) 22.4

front 18

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

back 18

B) 273.15 K and 1 atm

front 19

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

back 19

E) 1.82 × 103

front 20

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

back 20

D) 1.50 × 103

front 21

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

back 21

D) NO2

front 22

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

back 22

D) 1.88

front 23

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

back 23

B) NO

front 24

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

back 24

B) the square of the rms speed

front 25

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

back 25

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

front 26

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.

back 26

C)H2O

front 27

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

back 27

A) double

front 28

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.

back 28

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

front 29

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

back 29

B) CH4

front 30

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

back 30

C) 2.01

front 31

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

back 31

D) 1.207

front 32

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

back 32

A) Cl2 < F2 < O2 < N2

front 33

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

back 33

A) 288

front 34

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

back 34

B) CO

front 35

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

back 35

A) have no attraction for one another

front 36

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

back 36

B) high temperature and low pressure

front 37

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

back 37

E) xenon

front 38

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

back 38

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

front 39

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

back 39

C) increases, decreases

front 40

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

back 40

A) 55

front 41

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

back 41

C) 2.4 × 105

front 42

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

back 42

B) 0.967

front 43

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

back 43

A) 1.05

front 44

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

back 44

C) 0.67

front 45

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

back 45

D) 25.5

front 46

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

back 46

B) 68.2

front 47

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

back 47

D) 1.13

front 48

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

back 48

B) 2.8

front 49

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

back 49

C) 1.6

front 50

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

back 50

A) 1.18