UNE GENERAL CHEMISTRY II MIDTERM 2026
| Complete Study Guide | Verified Practice
Questions, Correct Answers & Detailed
Explanations | Latest Exam Prep PDF
UNE GENERAL CHEMISTRY II MIDTERM 2026
Complete Study Guide | Verified Practice Questions, Correct Answers &
Detailed Explanations
DOCUMENT OVERVIEW
• This comprehensive study guide contains 200 carefully curated multiple-choice
practice questions organized by topic to systematically reinforce all concepts
covered in General Chemistry II, including thermodynamics, kinetics, equilibrium,
acid-base chemistry, electrochemistry, and more.
• Use this material by working through questions section by section, reviewing
detailed rationales for every answer to identify knowledge gaps, and retaking
challenging questions until concepts are mastered—ideal preparation for exam
success.
QUESTIONS
1. What is the primary focus of thermodynamics in chemistry?
A) The study of reaction mechanisms and catalysts
B) The study of energy changes and heat flow in chemical reactions
C) The study of molecular structure and bonding
D) The study of reaction rates and kinetics
E) The study of atomic masses and isotopes
CORRECT ANSWER: B) The study of energy changes and heat flow in
chemical reactions
,Rationale: Thermodynamics is the branch of chemistry that deals with the heat
and energy associated with chemical reactions and physical changes. It examines
how energy is absorbed or released (enthalpy), the spontaneity of processes (Gibbs
free energy), and the disorder or randomness in systems (entropy). Options A, D,
and E refer to kinetics, atomic structure, and nuclear chemistry respectively, while
option C relates to bonding theory.
2. Which of the following statements about enthalpy is correct?
A) Enthalpy is always negative for spontaneous reactions
B) Enthalpy represents the total heat content of a system at constant pressure
C) Enthalpy increases when a reaction absorbs energy
D) Enthalpy is a measure of molecular disorder
E) Enthalpy cannot be measured directly
CORRECT ANSWER: B) Enthalpy represents the total heat content of a
system at constant pressure
Rationale: Enthalpy (H) is defined as the total heat content of a substance at
constant pressure and is calculated as H = U + PV. While enthalpy can be negative
or positive for spontaneous reactions (Option A is incorrect), and increases in
endothermic reactions (Option C is partially correct but incomplete), the most
comprehensive and accurate definition is that it represents total heat content at
constant pressure. Entropy, not enthalpy, measures molecular disorder (Option D).
Enthalpy can be determined from calorimetry and Hess's Law calculations (Option E
is false).
3. What does Hess's Law state?
A) The enthalpy change of a reaction depends on the pathway taken
B) The enthalpy change of a reaction is independent of the pathway and depends
only on initial and final states
,C) The sum of all enthalpy changes in a cycle equals zero only for exothermic
reactions
D) Enthalpy changes are always directly proportional to temperature
E) The enthalpy of a reaction cannot be calculated from thermochemical equations
CORRECT ANSWER: B) The enthalpy change of a reaction is independent of
the pathway and depends only on initial and final states
Rationale: Hess's Law is a fundamental principle stating that the enthalpy change
(ΔH) of a chemical reaction depends only on the initial and final states, not on the
intermediate steps or pathway. This makes enthalpy a state function. This principle
allows chemists to calculate enthalpy changes for reactions that cannot be directly
measured by combining thermochemical equations. Option A contradicts Hess's
Law, Option C incorrectly limits it to exothermic reactions, Option D confuses
temperature dependency, and Option E is false.
4. Which process is endothermic?
A) Combustion of gasoline
B) Freezing of water
C) Rusting of iron
D) Melting of ice
E) Neutralization of a strong acid with a strong base
CORRECT ANSWER: D) Melting of ice
Rationale: An endothermic process requires energy input from the surroundings.
Melting is a phase change that requires heat absorption to break intermolecular
forces. Combustion (A), rusting (C), and strong acid-base neutralizations (E) are
exothermic, releasing energy. Freezing (B) is exothermic as heat is released when
water changes from liquid to solid state.
5. What is entropy?
, A) The energy available to do work in a system
B) A measure of the disorder or randomness in a system
C) The rate at which a reaction proceeds
D) The heat capacity of a substance
E) The ability of a system to maintain thermal equilibrium
CORRECT ANSWER: B) A measure of the disorder or randomness in a
system
Rationale: Entropy (S) is a thermodynamic quantity that measures the degree of
disorder or randomness in a system. Higher entropy means greater disorder.
According to the Second Law of Thermodynamics, the entropy of an isolated
system always increases. Option A describes Gibbs free energy, Option C refers to
kinetics, Option D is heat capacity, and Option E describes thermal equilibrium, all
incorrect definitions of entropy.
6. What is the relationship between Gibbs free energy, enthalpy, and entropy?
A) ΔG = ΔH + TΔS
B) ΔG = ΔH - TΔS
C) ΔG = TΔS - ΔH
D) ΔG = ΔH × TΔS
E) ΔG = ΔH ÷ TΔS
CORRECT ANSWER: B) ΔG = ΔH - TΔS
Rationale: The Gibbs free energy equation is ΔG = ΔH - TΔS, where ΔG is the change
in Gibbs free energy, ΔH is the change in enthalpy, T is absolute temperature in
Kelvin, and ΔS is the change in entropy. This equation predicts spontaneity: when
ΔG is negative, the reaction is spontaneous; when positive, it is non-spontaneous.
Option A has the wrong sign for entropy, while Options C, D, and E have incorrect
mathematical relationships.
| Complete Study Guide | Verified Practice
Questions, Correct Answers & Detailed
Explanations | Latest Exam Prep PDF
UNE GENERAL CHEMISTRY II MIDTERM 2026
Complete Study Guide | Verified Practice Questions, Correct Answers &
Detailed Explanations
DOCUMENT OVERVIEW
• This comprehensive study guide contains 200 carefully curated multiple-choice
practice questions organized by topic to systematically reinforce all concepts
covered in General Chemistry II, including thermodynamics, kinetics, equilibrium,
acid-base chemistry, electrochemistry, and more.
• Use this material by working through questions section by section, reviewing
detailed rationales for every answer to identify knowledge gaps, and retaking
challenging questions until concepts are mastered—ideal preparation for exam
success.
QUESTIONS
1. What is the primary focus of thermodynamics in chemistry?
A) The study of reaction mechanisms and catalysts
B) The study of energy changes and heat flow in chemical reactions
C) The study of molecular structure and bonding
D) The study of reaction rates and kinetics
E) The study of atomic masses and isotopes
CORRECT ANSWER: B) The study of energy changes and heat flow in
chemical reactions
,Rationale: Thermodynamics is the branch of chemistry that deals with the heat
and energy associated with chemical reactions and physical changes. It examines
how energy is absorbed or released (enthalpy), the spontaneity of processes (Gibbs
free energy), and the disorder or randomness in systems (entropy). Options A, D,
and E refer to kinetics, atomic structure, and nuclear chemistry respectively, while
option C relates to bonding theory.
2. Which of the following statements about enthalpy is correct?
A) Enthalpy is always negative for spontaneous reactions
B) Enthalpy represents the total heat content of a system at constant pressure
C) Enthalpy increases when a reaction absorbs energy
D) Enthalpy is a measure of molecular disorder
E) Enthalpy cannot be measured directly
CORRECT ANSWER: B) Enthalpy represents the total heat content of a
system at constant pressure
Rationale: Enthalpy (H) is defined as the total heat content of a substance at
constant pressure and is calculated as H = U + PV. While enthalpy can be negative
or positive for spontaneous reactions (Option A is incorrect), and increases in
endothermic reactions (Option C is partially correct but incomplete), the most
comprehensive and accurate definition is that it represents total heat content at
constant pressure. Entropy, not enthalpy, measures molecular disorder (Option D).
Enthalpy can be determined from calorimetry and Hess's Law calculations (Option E
is false).
3. What does Hess's Law state?
A) The enthalpy change of a reaction depends on the pathway taken
B) The enthalpy change of a reaction is independent of the pathway and depends
only on initial and final states
,C) The sum of all enthalpy changes in a cycle equals zero only for exothermic
reactions
D) Enthalpy changes are always directly proportional to temperature
E) The enthalpy of a reaction cannot be calculated from thermochemical equations
CORRECT ANSWER: B) The enthalpy change of a reaction is independent of
the pathway and depends only on initial and final states
Rationale: Hess's Law is a fundamental principle stating that the enthalpy change
(ΔH) of a chemical reaction depends only on the initial and final states, not on the
intermediate steps or pathway. This makes enthalpy a state function. This principle
allows chemists to calculate enthalpy changes for reactions that cannot be directly
measured by combining thermochemical equations. Option A contradicts Hess's
Law, Option C incorrectly limits it to exothermic reactions, Option D confuses
temperature dependency, and Option E is false.
4. Which process is endothermic?
A) Combustion of gasoline
B) Freezing of water
C) Rusting of iron
D) Melting of ice
E) Neutralization of a strong acid with a strong base
CORRECT ANSWER: D) Melting of ice
Rationale: An endothermic process requires energy input from the surroundings.
Melting is a phase change that requires heat absorption to break intermolecular
forces. Combustion (A), rusting (C), and strong acid-base neutralizations (E) are
exothermic, releasing energy. Freezing (B) is exothermic as heat is released when
water changes from liquid to solid state.
5. What is entropy?
, A) The energy available to do work in a system
B) A measure of the disorder or randomness in a system
C) The rate at which a reaction proceeds
D) The heat capacity of a substance
E) The ability of a system to maintain thermal equilibrium
CORRECT ANSWER: B) A measure of the disorder or randomness in a
system
Rationale: Entropy (S) is a thermodynamic quantity that measures the degree of
disorder or randomness in a system. Higher entropy means greater disorder.
According to the Second Law of Thermodynamics, the entropy of an isolated
system always increases. Option A describes Gibbs free energy, Option C refers to
kinetics, Option D is heat capacity, and Option E describes thermal equilibrium, all
incorrect definitions of entropy.
6. What is the relationship between Gibbs free energy, enthalpy, and entropy?
A) ΔG = ΔH + TΔS
B) ΔG = ΔH - TΔS
C) ΔG = TΔS - ΔH
D) ΔG = ΔH × TΔS
E) ΔG = ΔH ÷ TΔS
CORRECT ANSWER: B) ΔG = ΔH - TΔS
Rationale: The Gibbs free energy equation is ΔG = ΔH - TΔS, where ΔG is the change
in Gibbs free energy, ΔH is the change in enthalpy, T is absolute temperature in
Kelvin, and ΔS is the change in entropy. This equation predicts spontaneity: when
ΔG is negative, the reaction is spontaneous; when positive, it is non-spontaneous.
Option A has the wrong sign for entropy, while Options C, D, and E have incorrect
mathematical relationships.
