CHEM 104 MODULE 3 PRACTICE EXAM
QUESTIONS AND CORRECT ANSWERS
(VERIFIED ANSWERS) PLUS RATIONALES
2025
1. Which of the following is an example of an endothermic process?
A. Melting ice
B. Condensation of steam
C. Freezing water
D. Combustion of gasoline
Melting absorbs heat, so it is an endothermic process.
2. Which of the following quantities is a measure of heat?
A. Temperature
B. Joule
C. Kelvin
D. Celsius
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,Joules (or calories) measure heat; temperature measures thermal energy level,
not total heat.
3. The First Law of Thermodynamics states:
A. Energy is created in reactions
B. Energy is destroyed in chemical changes
C. Energy is conserved
D. Energy flows from cold to hot spontaneously
The First Law means energy cannot be created or destroyed—only transferred or
transformed.
4. In a calorimetry experiment, the specific heat of water is:
A. 2.02 J/g°C
B. 4.18 J/g°C
C. 1.00 J/g°C
D. 8.31 J/g°C
Water's specific heat is high at 4.18 J/g°C, making it excellent for thermal
buffering.
5. What is the sign of ΔH for an exothermic reaction?
A. Positive
B. Negative
C. Zero
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, D. Undefined
Exothermic reactions release heat, resulting in a negative enthalpy change.
6. Which process is not associated with an energy change?
A. Melting ice
B. Freezing water
C. Breaking a glass
D. Boiling water
Breaking a glass is a physical action without significant thermal energy
exchange.
7. The enthalpy change (ΔH) is a measure of:
A. Heat at constant volume
B. Heat at constant pressure
C. Work done on the system
D. Energy lost as light
Enthalpy is defined as heat at constant pressure.
8. If q = m × c × ΔT, what does ΔT represent?
A. Total temperature
B. Heat gained
C. Temperature change
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QUESTIONS AND CORRECT ANSWERS
(VERIFIED ANSWERS) PLUS RATIONALES
2025
1. Which of the following is an example of an endothermic process?
A. Melting ice
B. Condensation of steam
C. Freezing water
D. Combustion of gasoline
Melting absorbs heat, so it is an endothermic process.
2. Which of the following quantities is a measure of heat?
A. Temperature
B. Joule
C. Kelvin
D. Celsius
1|Page
,Joules (or calories) measure heat; temperature measures thermal energy level,
not total heat.
3. The First Law of Thermodynamics states:
A. Energy is created in reactions
B. Energy is destroyed in chemical changes
C. Energy is conserved
D. Energy flows from cold to hot spontaneously
The First Law means energy cannot be created or destroyed—only transferred or
transformed.
4. In a calorimetry experiment, the specific heat of water is:
A. 2.02 J/g°C
B. 4.18 J/g°C
C. 1.00 J/g°C
D. 8.31 J/g°C
Water's specific heat is high at 4.18 J/g°C, making it excellent for thermal
buffering.
5. What is the sign of ΔH for an exothermic reaction?
A. Positive
B. Negative
C. Zero
2|Page
, D. Undefined
Exothermic reactions release heat, resulting in a negative enthalpy change.
6. Which process is not associated with an energy change?
A. Melting ice
B. Freezing water
C. Breaking a glass
D. Boiling water
Breaking a glass is a physical action without significant thermal energy
exchange.
7. The enthalpy change (ΔH) is a measure of:
A. Heat at constant volume
B. Heat at constant pressure
C. Work done on the system
D. Energy lost as light
Enthalpy is defined as heat at constant pressure.
8. If q = m × c × ΔT, what does ΔT represent?
A. Total temperature
B. Heat gained
C. Temperature change
3|Page
