Question 1

Which of the following best describes the role of intermolecular forces in determining the boiling point of a liquid?

Accepted Answer

Stronger intermolecular forces result in a higher boiling point because more energy is required to separate the molecules.

Question 2

A sample of gas is compressed at constant temperature from 2.0 L to 1.0 L. According to Boyle's Law, what happens to the pressure?

Accepted Answer

The pressure is doubled.

Question 3

Which equation correctly represents the relationship between Gibbs free energy ($$\Delta G$$), enthalpy ($$\Delta H$$), and entropy ($$\Delta S) at $$constant temperature?

Accepted Answer

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

Question 4

Which of the following statements about chemical equilibrium is correct?

Accepted Answer

At equilibrium, the rates of the forward and reverse reactions are equal.

Question 5

A reaction has an activation energy of 50 kJ/mol. If a catalyst is added, which of the following is most likely to occur?

Accepted Answer

The activation energy decreases, increasing the reaction rate.

Question 6

Which of the following best explains why ionic compounds tend to have high melting points?

Accepted Answer

Ionic compounds are held together by strong electrostatic attractions between oppositely charged ions.

Question 7

Which of the following is the correct expression for the equilibrium constant $$K_c$$ for the reaction $$aA + bB \rightleftharpoons cC + dD$$?

Accepted Answer

$$K_c = \dfrac{[C]^c [D]^d}{[A]^a [B]^b}$$

Question 8

A solution is prepared by dissolving 0.5 mol of NaCl in enough water to make 1.0 L of solution. What is the molarity of the solution?

Accepted Answer

0.5 M

Question 9

Which of the following best describes the effect of increasing temperature on the rate of a chemical reaction?

Accepted Answer

The rate increases because more molecules have sufficient energy to overcome the activation energy barrier.

Question 10

Which of the following is a correct statement about acids and bases according to the Brønsted-Lowry definition?

Accepted Answer

An acid is a substance that donates a proton.

Question 11

A chemical reaction is exothermic and spontaneous at room temperature. Which of the following is most likely true about $$\Delta H$$ and $$\Delta G$$ for this reaction?

Accepted Answer

$$\Delta H \u003c 0$$ and $$\Delta G \u003c 0$$

Question 12

Which of the following is the correct formula for calculating the entropy change ($$\Delta S) $$for a reversible process at constant temperature?

Accepted Answer

$$\Delta S = \dfrac{q_{rev}}{T}$$

Question 13

Which of the following best describes a colligative property?

Accepted Answer

A property that depends on the number of solute particles present, not their identity.

Question 14

Which of the following is the correct balanced equation for the dissociation of sulfuric acid ($$H_2SO_4) in $$water?

Accepted Answer

$$H_2SO_4 + 2H_2O \rightarrow 2H_3O^+ + SO_4$^{2-}$$

Question 15

A voltaic cell is constructed using a zinc electrode in $$ZnSO_4$$ solution and a copper electrode in $$CuSO_4$$ solution. Which of the following correctly identifies the anode and cathode?

Accepted Answer

Copper is the cathode, zinc is the anode.

Question 16

Which of the following best explains why water is a good solvent for ionic compounds?

Accepted Answer

Water molecules are polar and can stabilize ions through ion-dipole interactions.

Question 17

Which of the following is the correct rate law for a reaction that is first order in $$A$$ and second order in $$B$$?

Accepted Answer

$$rate = k[A][B]^2$$

Question 18

A radioactive isotope has a half-life of 10 years. If you start with 80 grams, how much will remain after 30 years?

Accepted Answer

20 grams

Question 19

Which of the following best describes the process of osmosis?

Accepted Answer

The movement of solvent molecules from low to high solute concentration through a semipermeable membrane.

CHM 2046 - Chemistry Fundamentals II: Course Overview and Study Guide

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