CHEM Review Test 5

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

The molecular weight of a gas is ________ g/mol if 6.7 g of the gas occupies 6.3 L at STP. A) 24 B) 3.6 × 103 C) 27 D) 3.0 × 102 E) 1.8 × 10-2

A) 24

Automobile air bags use the decomposition of sodium azide as their source of gas for rapid inflation: 2NaN3 (s) → 2Na (s) + 3N2 (g). What mass (g) of NaN3 is required to provide 26.5 L of N2 at 22.0 °C and 1.10 atm? A) 52.2 B) 700. C) 0.807 D) 1.21 E) 1.10

A) 52.2

The temperature of a sample of CH4 gas (10.34 g) in a 50.0 L vessel at 1.33 atm is ________ °C. A) 984 B) -195 C) 195 D) 1260 E) -1260

A) 984

Which one of the following should have the lowest boiling point? A) CF4 B) SnF3 C) C4H9OH D) HCl E) F2O

A) CF4

Which of the following has dispersion forces as its only intermolecular force? A) CH4 B) HCl C) C6H13NH2 D) NaCl E) CH3Cl

A) CH4

Which one of the following gases would deviate the least from ideal gas behavior? A) Ne B) CH3Cl C) Kr D) CO2 E) F2

A) Ne

Of the following, ________ is a correct statement of Boyle's law. A) PV = constant B) P/V= constant C) V/P= constant D) V/T= constant E) n/P= constant

A) PV = constant

What type(s) of intermolecular forces exist between Br2 and CCl4? A) dispersion forces B) dispersion forces and ion-dipole C) dispersion forces and dipole-dipole D) dispersion forces, ion-dipole, and dipole-dipole E) None. Since both are gases at room temperature, they do not interact with each other.

A) dispersion forces

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

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

"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

The strongest interparticle attractions exist between particles of a ________, and the weakest interparticle attractions exist between particles of a ________. A) solid, liquid B) solid, gas C) liquid, gas D) liquid, solid E) gas, solid

B) solid, gas

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

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

________ are particularly polarizable. A) Small nonpolar molecules B) Small polar molecules C) Large nonpolar molecules D) Large polar molecules E) Large molecules, regardless of their polarity,

C) Large nonpolar molecules

Hydration is a specific example of the phenomenon known generally as ________. A) salutation B) disordering C) solvation D) condensation E) dilution

C) solvation

The shape of a liquid's meniscus is determined by ________. A) the viscosity of the liquid B) the type of material the container is made of C) the relative magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and its container D) the amount of hydrogen bonding in the liquid E) the volume of the liquid

C) the relative magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and its container

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

D) 0.583

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

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

The enthalpy change for converting 10.0 g of ice at -50.0 °C to water at 50.0 °C is ________ kJ. The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. For H2O, ΔHfus = 6.01 kJ/mol, and ΔHvap = 40.67 kJ/mol. A) 12.28 B) 4.38 C) 3138 D) 6.47 E) 9.15

D) 6.47

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

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

Which statements about viscosity are true? (i) Viscosity increases as temperature decreases. (ii) Viscosity increases as molecular weight increases. (iii) Viscosity increases as intermolecular forces increase. A) (i) only B) (ii) and (iii) C) (i) and (iii) D) none E) all

E) all

Large intermolecular forces in a substance are manifested by ________. A) low vapor pressure B) high boiling point C) high heats of fusion and vaporization D) high critical temperatures and pressures E) all of the above

E) all of the above

In general, the vapor pressure of a substance increases as ________ increases. A) surface tension B) molecular weight C) hydrogen bonding D) viscosity E) temperature

E) temperature