UNE GENERAL CHEMISTRY II MIDTERM EXAM– QUESTIONS AND ANSWERS | VERIFIED AND WELL DETAILED
ANSWERS | PLUS RATIONALES | DOWNLOAD AND PASS | LATEST EXAM UPDATE 2026/2027
Core Domains
Chemical Thermodynamics and Thermochemistry
Chemical Kinetics and Reaction Mechanisms
Chemical Equilibrium and Le Chatelier's Principle
Acid-Base Equilibria and Buffer Systems
Solubility Equilibria and Precipitation Reactions
Electrochemistry and Redox Reactions
Nuclear Chemistry and Radioactivity
Transition Metals and Coordination Chemistry
Laboratory Safety, Ethics, and Regulatory Compliance
Introduction
This comprehensive midterm examination assesses mastery of foundational and applied concepts in General Chemistry
II. It evaluates students' understanding of thermodynamic principles, reaction kinetics, equilibrium systems,
electrochemistry, and coordination chemistry. Questions integrate theoretical knowledge with practical laboratory
,scenarios, regulatory compliance, and ethical decision-making. The exam employs multiple-choice and scenario-based
formats to test critical thinking, quantitative reasoning, and real-world application. Students must demonstrate
competency in problem-solving, data interpretation, and professional judgment expected in scientific and regulatory
environments. This assessment prepares candidates for advanced coursework and professional practice in chemistry-
related fields.
SECTION ONE: QUESTIONS 1–50
Question 1
Which statement best describes the first law of thermodynamics?
A. Energy can be created but not destroyed
B. The entropy of the universe always increases
C. Energy can be converted from one form to another but cannot be created or destroyed
D. Heat always flows spontaneously from cold to hot
🟢 Correct Answer: C. Energy can be converted from one form to another but cannot be created or destroyed
🔴 Explanation: The first law of thermodynamics is the law of conservation of energy, stating that energy cannot be
created or destroyed, only transformed. Option A violates conservation. Option B describes the second law. Option
,D violates the second law.
Question 2
A system absorbs 250 J of heat and does 75 J of work on the surroundings. What is the change in internal energy?
A. +325 J
B. +175 J
C. −175 J
D. −325 J
🟢 Correct Answer: B. +175 J
🔴 Explanation: ΔE = q + w. Heat absorbed is positive (q = +250 J). Work done by the system is negative (w = −75
J). ΔE = 250 − 75 = +175 J.
Question 3
Which process is always spontaneous regardless of temperature?
, A. Endothermic with decreasing entropy
B. Exothermic with increasing entropy
C. Endothermic with increasing entropy
D. Exothermic with decreasing entropy
🟢 Correct Answer: B. Exothermic with increasing entropy
🔴 Explanation: ΔG = ΔH − TΔS. When ΔH is negative (exothermic) and ΔS is positive (increasing entropy), ΔG is
always negative, making the process spontaneous at all temperatures.
Question 4
Calculate the standard enthalpy change for the reaction: 2H₂(g) + O₂(g) → 2H₂O(l), given ΔH°f[H₂O(l)] = −285.8
kJ/mol.
A. −285.8 kJ
B. −571.6 kJ
C. +571.6 kJ
D. +285.8 kJ
🟢 Correct Answer: B. −571.6 kJ
ANSWERS | PLUS RATIONALES | DOWNLOAD AND PASS | LATEST EXAM UPDATE 2026/2027
Core Domains
Chemical Thermodynamics and Thermochemistry
Chemical Kinetics and Reaction Mechanisms
Chemical Equilibrium and Le Chatelier's Principle
Acid-Base Equilibria and Buffer Systems
Solubility Equilibria and Precipitation Reactions
Electrochemistry and Redox Reactions
Nuclear Chemistry and Radioactivity
Transition Metals and Coordination Chemistry
Laboratory Safety, Ethics, and Regulatory Compliance
Introduction
This comprehensive midterm examination assesses mastery of foundational and applied concepts in General Chemistry
II. It evaluates students' understanding of thermodynamic principles, reaction kinetics, equilibrium systems,
electrochemistry, and coordination chemistry. Questions integrate theoretical knowledge with practical laboratory
,scenarios, regulatory compliance, and ethical decision-making. The exam employs multiple-choice and scenario-based
formats to test critical thinking, quantitative reasoning, and real-world application. Students must demonstrate
competency in problem-solving, data interpretation, and professional judgment expected in scientific and regulatory
environments. This assessment prepares candidates for advanced coursework and professional practice in chemistry-
related fields.
SECTION ONE: QUESTIONS 1–50
Question 1
Which statement best describes the first law of thermodynamics?
A. Energy can be created but not destroyed
B. The entropy of the universe always increases
C. Energy can be converted from one form to another but cannot be created or destroyed
D. Heat always flows spontaneously from cold to hot
🟢 Correct Answer: C. Energy can be converted from one form to another but cannot be created or destroyed
🔴 Explanation: The first law of thermodynamics is the law of conservation of energy, stating that energy cannot be
created or destroyed, only transformed. Option A violates conservation. Option B describes the second law. Option
,D violates the second law.
Question 2
A system absorbs 250 J of heat and does 75 J of work on the surroundings. What is the change in internal energy?
A. +325 J
B. +175 J
C. −175 J
D. −325 J
🟢 Correct Answer: B. +175 J
🔴 Explanation: ΔE = q + w. Heat absorbed is positive (q = +250 J). Work done by the system is negative (w = −75
J). ΔE = 250 − 75 = +175 J.
Question 3
Which process is always spontaneous regardless of temperature?
, A. Endothermic with decreasing entropy
B. Exothermic with increasing entropy
C. Endothermic with increasing entropy
D. Exothermic with decreasing entropy
🟢 Correct Answer: B. Exothermic with increasing entropy
🔴 Explanation: ΔG = ΔH − TΔS. When ΔH is negative (exothermic) and ΔS is positive (increasing entropy), ΔG is
always negative, making the process spontaneous at all temperatures.
Question 4
Calculate the standard enthalpy change for the reaction: 2H₂(g) + O₂(g) → 2H₂O(l), given ΔH°f[H₂O(l)] = −285.8
kJ/mol.
A. −285.8 kJ
B. −571.6 kJ
C. +571.6 kJ
D. +285.8 kJ
🟢 Correct Answer: B. −571.6 kJ
