Question 1

Which of the following best explains why water has a higher boiling point than methane, even though both are small molecules?

Accepted Answer

Water molecules form hydrogen bonds, which are stronger than the London dispersion forces present in methane.

Question 2

A solution is prepared by dissolving 10.0 g of NaCl in enough water to make 500 mL of solution. What is the molarity of the solution? (Molar mass of NaCl = 58.44 g/mol)

Accepted Answer

$$0.342\ \mathrm{M}$$

Question 3

Which of the following statements about colligative properties is correct?

Accepted Answer

Colligative properties depend only on the number of solute particles, not their identity.

Question 4

A reaction has a rate law: $$	ext{rate} = k[\mathrm{A}]^2[\mathrm{B}]. If $$the concentration of A is doubled and B is halved, how does the rate change?

Accepted Answer

The rate increases by a factor of 2.

Question 5

Which of the following best describes the difference between the rate constant ($$k) $$and the equilibrium constant ($$K$$)?

Accepted Answer

The rate constant describes how fast a reaction proceeds, while the equilibrium constant describes the ratio of products to reactants at equilibrium.

Question 6

For the reaction $$\mathrm{N}_2(g) + 3\mathrm{H}_2(g) \rightleftharpoons 2\mathrm{NH}_3(g)$$, which of the following changes will shift the equilibrium to the right?

Accepted Answer

Increasing the pressure by decreasing the volume.

Question 7

A solution has $$[\mathrm{H}^+] = 1.0 	imes 10$$^{-5}$$\ \mathrm{M}. $$What is its pH?

Accepted Answer

$$5.0$$

Question 8

Which of the following is a characteristic of a buffer solution?

Accepted Answer

It resists changes in pH when small amounts of acid or base are added.

Question 9

During a titration, 25.0 mL of 0.100 M HCl is neutralized by 0.100 M NaOH. What volume of NaOH is required?

Accepted Answer

$$25.0\ \mathrm{mL}$$

Question 10

Which of the following best explains the common ion effect?

Accepted Answer

The solubility of a salt decreases when a common ion is added to the solution.

Question 11

Which of the following statements about entropy ($$\Delta S) is $$correct?

Accepted Answer

Entropy is a measure of the disorder or randomness of a system.

Question 12

Given the reaction $$2\mathrm{Ag}^+(aq) + \mathrm{Cu}(s) \rightarrow 2\mathrm{Ag}(s) + \mathrm{Cu}^{2+}(aq)$$, which species is oxidized?

Accepted Answer

$$\mathrm{Cu}(s)$$

Question 13

Which of the following is true about a spontaneous reaction at constant temperature and pressure?

Accepted Answer

$$\Delta G \u003c 0$$

Question 14

Which of the following correctly describes the function of the salt bridge in a galvanic (voltaic) cell?

Accepted Answer

It allows the flow of ions to maintain electrical neutrality.

Question 15

A saturated solution of $$\mathrm{AgCl} is in $$equilibrium. If NaCl is added to the solution, what will happen?

Accepted Answer

More $$\mathrm{AgCl}$$ will precipitate out.

Question 16

Which of the following is the correct balanced half-reaction for the reduction of $$\mathrm{MnO}_4^- to$$ $$\mathrm{Mn}^{2+} in $$acidic solution?

Accepted Answer

$$\mathrm{MnO}_4^- + 8\mathrm{H}^+ + 5e^- \rightarrow \mathrm{Mn}^{2+} + 4\mathrm{H}_2O$$

Question 17

Which of the following is true for a reaction at equilibrium?

Accepted Answer

The rates of the forward and reverse reactions are equal.

Question 18

A weak acid, HA, has a $$K_a = 1.0 	imes 10$$^{-5}$$. What is the pH of a 0.10 M solution of HA? (Assume x$$ \ll 0.10$$)

Accepted Answer

$$3.0$$

Question 19

Which of the following best describes the effect of increasing temperature on the solubility of most solid salts in water?

Accepted Answer

Solubility increases with increasing temperature.

Question 20

Which of the following equations correctly relates Gibbs free energy to enthalpy and entropy?

Accepted Answer

$$\Delta G = \Delta H - T\Delta S$$

General Chemistry II: Course Syllabus and Study Guide

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