Choose the molecule or compound that exhibits dipole-dipole forces as its strongest intermolecular force.

SO₂

H₂

CF₄

BCl₃

NH₃

SO₂

Choose the pair of substances that are most likely to form a homogeneous solution.

LiF and C₆H₁₄

C₃H₈ and C₂H₅OH

Br₂ and PF₃

NH₃ and CH₃OH

NaCl and Hg

NH₃ and CH₃OH

Choose the substance with the highest boiling point.

CS₂

HF

I₂

KI

CH₄

KI

Choose the substance with the lowest surface tension.

CH₃CH₂CH₂CH₃

H₂O

C₆H₆

(CH₃)₂CO

CH₃SH

CH₃CH₂CH₂CH₃

Choose the substance with the lowest vapor pressure at a given temperature.

He

BF₃

BeCl₂

CO₂

PF₅

BeCl₂

Choose the substance with the lowest viscosity.

Cl₂CHCH₂Cl

Cl₃CCCl₃

Cl₃CCHCl₂

ClCH₂CH₂Cl

Cl₂CHCHCl₂

ClCH₂CH₂Cl

Give the change in condition to go from a liquid to a gas.

Cool or reduce pressure

Increase heat or reduce pressure

Cool or increase pressure

Increase heat or increase pressure

None of the above

Increase heat or reduce pressure

Give the characteristic of a first order reaction having only one reactant.

The rate of the reaction is directly proportional to the concentration of the reactant.

The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant.

The rate of the reaction is proportional to the square root of the concentration of the reactant.

The rate of the reaction is not proportional to the concentration of the reactant.

The rate of the reaction is proportional to the square of the concentration of the reactant.

The rate of the reaction is directly proportional to the concentration of the reactant.

Give the term for the temperature at which the gas and liquid phases form a supercritical fluid.

Definite temperature.

Absolute temperature.

Critical temperature.

Fluid temperature.

Solid temperature

Critical temperature.

Given the following balanced equation, determine the rate of reaction with respect to [NOCl]. If the rate of Cl₂ loss is 4.84 × 10^-2 M/s, what is the rate of formation of NOCl?
2 NO(g) + Cl₂(g) → 2 NOCl(g)

Answers:

4.84 × 10^-2 M/s

1.61 × 10^-2 M/s

1.45 × 10^-1 M/s

9.68 × 10^-2 M/s

2.42 × 10^-2 M/s

9.68 × 10^-2 M/s

Given the following rate law, how does the rate of reaction change if the concentration of X is halved and the concentration of Y is doubled?
Rate = k [X][Y]²
Answers:

The rate of reaction will increase by a factor of 5.

The rate of reaction will increase by a factor of 2.

The rate of reaction will decrease by a factor of 2.

The rate of reaction will increase by a factor of 4.

The rate of reaction will remain unchanged.

The rate of reaction will increase by a factor of 2.

How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value?

2

1.75

3

2.75

1

3

How much energy is required to vaporize 48.7 g of dichloromethane (CH₂Cl₂) at its boiling point, if its ΔH_vap is 31.6 kJ/mol?

18.1 kJ

55.1 kJ

31.2 kJ

15.4 kJ

6.49 kJ

18.1 kJ

Place the following compounds in order of decreasing strength of intermolecular forces.
HF O₂ CO₂
Answers:

HF > O₂ > CO₂

O₂ > CO₂ > HF

CO₂ > HF > O2

HF > CO₂ > O₂

CO₂ > O₂ > HF

HF > CO₂ > O₂

Place the following compounds in order of increasing strength of intermolecular forces.
CO₂ F₂ NH₂CH₃
Answers:

NH₂CH₃ < F₂ < CO₂

NH₂CH₃ < CO₂ < F₂

F₂ < CO₂ < NH₂CH₃

CO₂ < NH₂CH₃ < F₂

F₂ < NH₂CH₃ < CO₂

F₂ < CO₂ < NH₂CH₃

What are the units of k in a first order reaction?

1/s

What are the units of k in the following rate law?
Rate = k[X][Y]

M^-1s^-1

What data should be plotted to show that experimental concentration data fits a second-order reaction?

1/[reactant] vs. time

ln[reactant] vs. time

ln(k) vs. E_a

ln(k) vs. 1/T

[reactant] vs. time

1/[reactant] vs. time

What is the overall order of the following reaction, given the rate law?
2 X + 3 Y → 2 Z Rate = k[X]¹[Y]²
Answers:

1st order

0th order

2nd order

5th order

3rd order

3rd order

What is the overall order of the following reaction, given the rate law?
2NO(g) + H₂(g) → N₂(g) + 2H₂O(g) Rate = k[NO]²[H₂]
Answers:

0th order

3rd order

4th order

2nd order

1st order

3rd order

What is the strongest type of intermolecular force present in CHF₃?

hydrogen bonding

ion-dipole

dipole-dipole

dispersion

None of the above

dipole-dipole

What is the strongest type of intermolecular force present in H₂?

dispersion

hydrogen bonding

ion-dipole

dipole-dipole

None of the above

dispersion

What is the strongest type of intermolecular force present in NH₂CH₃?

dipole-dipole

ion-dipole

dispersion

hydrogen bonding

None of the above

hydrogen bonding

represents the equation for a first-order half-life?

t 1/2 =

represents the integrated rate law for a first-order reaction?

= -kt

Which of the following statements is TRUE?

Until a certain point, the potential energy of molecules decrease as they get closer to one another.

Intermolecular forces are generally stronger than bonding forces.

Increasing the pressure on a solid usually causes it to become a liquid.

Energy is given off when the attraction between two molecules is broken.

None of the above are true.

Until a certain point, the potential energy of molecules decrease as they get closer to one another.

Which substance below has the strongest intermolecular forces?

C₃X₂, ΔH_vap= 36.4 kJ/mol

DX₂, ΔH_vap= 23.3 kJ/mol

BY₂, ΔH_vap= 26.7 kJ/mol

A₂X, ΔH_vap= 39.6 kJ/mol

EY₃, ΔH_vap= 21.5 kJ/mol

A₂X, ΔH_vap= 39.6 kJ/mol