,CHEM 103 Module 5 Exam | General
Chemistry I w/Lab | Portage Learning | Q & A
| 2026 Edition
1. A chemical reaction that releases heat to its surroundings is classified as:
A) Endothermic
B) Exothermic
C) Isothermal
D) Adiabatic
Correct Answer: Exothermic
Rationale: An exothermic reaction releases heat to the surroundings, resulting in a negative change in
enthalpy (ΔH < 0). This is the opposite of an endothermic reaction, which absorbs heat from the
surroundings.
2. What is the term for the amount of heat required to raise the temperature of one gram of a
substance by one degree Celsius?
A) Heat capacity
B) Specific heat capacity
C) Enthalpy
D) Calorimetry
Correct Answer: Specific heat capacity
Rationale: Specific heat capacity (c) is the amount of heat needed to raise the temperature of exactly
one gram of a substance by exactly one degree Celsius. It is a material-specific property.
3. The enthalpy change (ΔH) for a chemical reaction is defined as:
A) The heat absorbed or released at constant pressure
,B) The heat absorbed or released at constant volume
C) The total energy of the system
D) The heat required to vaporize a substance
Correct Answer: The heat absorbed or released at constant pressure
Rationale: Enthalpy change (ΔH) is the heat absorbed or released during a chemical reaction when the
process occurs at constant pressure, which is the most common condition for reactions in the
laboratory.
4. A student is calculating the heat (q) required to warm a 50.0 g sample of water from 25.0 °C to 75.0
°C. Which equation should they use, and what is the value of the specific heat capacity of water?
A) q = m × ΔT × c; c = 4.184 J/(g·°C)
B) q = m × ΔT × c; c = 0.385 J/(g·°C)
C) q = m × c / ΔT; c = 2.03 J/(g·°C)
D) q = c × ΔT / m; c = 4.184 J/(g·°C)
Correct Answer: q = m × ΔT × c; c = 4.184 J/(g·°C)
Rationale: The equation q = m × c × ΔT is used to calculate the heat absorbed or released during a
temperature change. The specific heat capacity of water is 4.184 J/(g·°C).
5. Using the equation q = m × c × ΔT, calculate the heat (in joules) required to raise the temperature of
50.0 g of water from 25.0 °C to 75.0 °C.
A) 10,460 J
B) 5,230 J
C) 2,615 J
D) 15,690 J
Correct Answer: 10,460 J
, Rationale: ΔT = 75.0 °C - 25.0 °C = 50.0 °C. q = (50.0 g) × (4.184 J/(g·°C)) × (50.0 °C) = 10,460 J.
6. Which of the following is an intensive property?
A) Mass
B) Volume
C) Temperature
D) Heat capacity
Correct Answer: Temperature
Rationale: Intensive properties are independent of the amount of substance present. Temperature is
intensive, while mass, volume, and heat capacity are extensive properties.
7. The three major components of thermochemistry are:
A) Heat, work, and internal energy
B) Heat, pressure, and temperature
C) Work, pressure, and enthalpy
D) Temperature, volume, and mass
Correct Answer: Heat, work, and internal energy
Rationale: Thermochemistry involves the study of heat, work, and internal energy as they relate to
chemical reactions and physical changes.
8. Which of the following is defined as the capacity to do work?
A) Heat
B) Energy
C) Temperature
Chemistry I w/Lab | Portage Learning | Q & A
| 2026 Edition
1. A chemical reaction that releases heat to its surroundings is classified as:
A) Endothermic
B) Exothermic
C) Isothermal
D) Adiabatic
Correct Answer: Exothermic
Rationale: An exothermic reaction releases heat to the surroundings, resulting in a negative change in
enthalpy (ΔH < 0). This is the opposite of an endothermic reaction, which absorbs heat from the
surroundings.
2. What is the term for the amount of heat required to raise the temperature of one gram of a
substance by one degree Celsius?
A) Heat capacity
B) Specific heat capacity
C) Enthalpy
D) Calorimetry
Correct Answer: Specific heat capacity
Rationale: Specific heat capacity (c) is the amount of heat needed to raise the temperature of exactly
one gram of a substance by exactly one degree Celsius. It is a material-specific property.
3. The enthalpy change (ΔH) for a chemical reaction is defined as:
A) The heat absorbed or released at constant pressure
,B) The heat absorbed or released at constant volume
C) The total energy of the system
D) The heat required to vaporize a substance
Correct Answer: The heat absorbed or released at constant pressure
Rationale: Enthalpy change (ΔH) is the heat absorbed or released during a chemical reaction when the
process occurs at constant pressure, which is the most common condition for reactions in the
laboratory.
4. A student is calculating the heat (q) required to warm a 50.0 g sample of water from 25.0 °C to 75.0
°C. Which equation should they use, and what is the value of the specific heat capacity of water?
A) q = m × ΔT × c; c = 4.184 J/(g·°C)
B) q = m × ΔT × c; c = 0.385 J/(g·°C)
C) q = m × c / ΔT; c = 2.03 J/(g·°C)
D) q = c × ΔT / m; c = 4.184 J/(g·°C)
Correct Answer: q = m × ΔT × c; c = 4.184 J/(g·°C)
Rationale: The equation q = m × c × ΔT is used to calculate the heat absorbed or released during a
temperature change. The specific heat capacity of water is 4.184 J/(g·°C).
5. Using the equation q = m × c × ΔT, calculate the heat (in joules) required to raise the temperature of
50.0 g of water from 25.0 °C to 75.0 °C.
A) 10,460 J
B) 5,230 J
C) 2,615 J
D) 15,690 J
Correct Answer: 10,460 J
, Rationale: ΔT = 75.0 °C - 25.0 °C = 50.0 °C. q = (50.0 g) × (4.184 J/(g·°C)) × (50.0 °C) = 10,460 J.
6. Which of the following is an intensive property?
A) Mass
B) Volume
C) Temperature
D) Heat capacity
Correct Answer: Temperature
Rationale: Intensive properties are independent of the amount of substance present. Temperature is
intensive, while mass, volume, and heat capacity are extensive properties.
7. The three major components of thermochemistry are:
A) Heat, work, and internal energy
B) Heat, pressure, and temperature
C) Work, pressure, and enthalpy
D) Temperature, volume, and mass
Correct Answer: Heat, work, and internal energy
Rationale: Thermochemistry involves the study of heat, work, and internal energy as they relate to
chemical reactions and physical changes.
8. Which of the following is defined as the capacity to do work?
A) Heat
B) Energy
C) Temperature
