Question 1

A solution is prepared by dissolving 10.0 g of NaCl in 100.0 g of water. Which of the following best describes the effect of this solute on the vapor pressure of water at 25°C?
Correct answer: The vapor pressure of water decreases because NaCl lowers the number of water molecules at the surface.

Accepted Answer

The vapor pressure of water decreases because NaCl lowers the number of water molecules at the surface.

Question 2

Which of the following statements about the Gibbs Free Energy equation (ΔG = ΔH - TΔS) is correct when predicting the spontaneity of a reaction at constant temperature and pressure?
Correct answer: A negative ΔG indicates the reaction is spontaneous.

Accepted Answer

A negative ΔG indicates the reaction is spontaneous.

Question 3

A reaction has a rate law: rate = k[A]^2[B]. If the concentration of A is doubled and B is halved, by what factor does the reaction rate change?
Correct answer: The rate increases by a factor of 2.

Accepted Answer

The rate increases by a factor of 2.

Question 4

Which of the following best explains why adding a catalyst increases the rate of a chemical reaction?
Correct answer: It lowers the activation energy required for the reaction.

Accepted Answer

It lowers the activation energy required for the reaction.

Question 5

A saturated solution of AgCl is in equilibrium with its solid at 25°C. What will happen to the concentration of Ag+ ions if NaCl is added to the solution?
Correct answer: The concentration of Ag+ ions will decrease due to the common ion effect.

Accepted Answer

The concentration of Ag+ ions will decrease due to the common ion effect.

Question 6

Which of the following is true regarding the Nernst equation and its application to electrochemical cells?
Correct answer: The Nernst equation accounts for non-standard concentrations of reactants and products.

Accepted Answer

The Nernst equation accounts for non-standard concentrations of reactants and products.

Question 7

A weak acid, HA, is dissolved in water. Which of the following statements is correct regarding its acid dissociation equilibrium?
Correct answer: The solution contains mostly undissociated HA molecules.

Accepted Answer

The solution contains mostly undissociated HA molecules.

Question 8

During a titration of a polyprotic acid with a strong base, which of the following is observed at each equivalence point?
Correct answer: A sharp increase in pH occurs at each equivalence point.

Accepted Answer

A sharp increase in pH occurs at each equivalence point.

Question 9

Which of the following best describes the function of the salt bridge in a galvanic cell?
Correct answer: It maintains electrical neutrality by allowing ion flow between half-cells.

Accepted Answer

It maintains electrical neutrality by allowing ion flow between half-cells.

Question 10

A nuclear reaction is described as follows: 14C → 14N + e−. What type of nuclear decay is this?
Correct answer: Beta decay

Accepted Answer

Beta decay

Question 11

A reaction is exothermic (ΔH  0). What can be concluded about the spontaneity of the reaction at all temperatures?
Correct answer: The reaction is spontaneous at all temperatures.

Accepted Answer

The reaction is spontaneous at all temperatures.

Question 12

Which of the following best explains why increasing the temperature generally increases the rate of a chemical reaction?
Correct answer: It increases the number of effective collisions between reactant molecules.

Accepted Answer

It increases the number of effective collisions between reactant molecules.

Question 13

A buffer solution is prepared by mixing acetic acid and sodium acetate. Which of the following best describes the buffer's ability to resist changes in pH?
Correct answer: It can neutralize both added acids and bases.

Accepted Answer

It can neutralize both added acids and bases.

Question 14

Which of the following changes will shift the equilibrium of the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) to the right?
Correct answer: Removing NH3 as it forms.

Accepted Answer

Removing NH3 as it forms.

Question 15

A patient is treated for acidosis (low blood pH) in a hospital. Which of the following chemical principles is most directly involved in the medical intervention?
Correct answer: Le Chatelier's Principle and buffer systems in blood.

Accepted Answer

Le Chatelier's Principle and buffer systems in blood.

Question 16

Which of the following is a correct application of the concept of colligative properties in real life?
Correct answer: Adding salt to ice on roads lowers the freezing point, preventing ice formation.

Accepted Answer

Adding salt to ice on roads lowers the freezing point, preventing ice formation.

Question 17

Which of the following best describes the role of entropy (ΔS) in determining the spontaneity of a chemical process?
Correct answer: An increase in entropy can favor spontaneity, depending on enthalpy and temperature.

Accepted Answer

An increase in entropy can favor spontaneity, depending on enthalpy and temperature.

Question 18

A solution is prepared by mixing 0.10 M HCl and 0.10 M NaOH. What is the resulting pH of the solution?
Correct answer: pH = 7

Accepted Answer

pH = 7

Question 19

Which of the following statements about electrolytic and galvanic cells is correct?
Correct answer: In an electrolytic cell, a non-spontaneous reaction is driven by an external voltage.

Accepted Answer

In an electrolytic cell, a non-spontaneous reaction is driven by an external voltage.

General Chemistry II: Course Overview and Key Concepts

Study Guide - Practice Questions

Study Guide - Flashcards