Title: CHEM 1211L Specific Heat & Heat Transfer MCQs – Lab Quiz Buster!

Multiple Choice Questions on Specific Heat and Heat Transfer
1. What is the specific heat of a substance?

 A) The amount of heat needed to raise the temperature of 1 gram of the substance
by 1 °C
 B) The total heat energy contained in a substance
 C) The heat required to melt 1 gram of a substance
 D) The heat released during a chemical reaction



2. If a substance absorbs heat and its temperature increases, which statement is true?

 A) q is negative
 B) q is zero
 C) q is positive
 D) q cannot be determined



3. Which of the following has the highest specific heat?

 A) Aluminum
 B) Water
 C) Iron
 D) Copper



4. A 250 g piece of copper absorbs 5,000 J of heat, and its temperature increases from 20 °C
to 80 °C. What is the specific heat of copper?

 A) 0.333 J/g °C
 B) 0.453 J/g °C
 C) 0.900 J/g °C
 D) 1.000 J/g °C

6. What happens to the temperature of a substance when it absorbs heat?

 A) It decreases
 B) It remains constant
 C) It increases
 D) It fluctuates unpredictably

,7. When 150 g of a substance absorbs 600 J of heat, what is the temperature change if the
specific heat of the substance is 0.5 J/g °C?

 A) 2 °C
 B) 4 °C
 C) 8 °C
 D) 10 °C



8. A cold pack absorbs heat from the environment. What type of process does this
represent?

 A) Exothermic
 B) Endothermic
 C) Isothermal
 D) Adiabatic



9. If a metal with a specific heat of 0.385 J/g °C undergoes a temperature change of 40 °C
after absorbing 1,540 J of heat, what is the mass of the metal?

 A) 100 g
 B) 15 0g
 C) 200 g
 D) 25 g



10. Which statement is true regarding the relationship between heat capacity and mass?

 A) Heat capacity is an intensive property
 B) Heat capacity is an extensive property
 C) Heat capacity remains constant regardless of mass
 D) Heat capacity decreases with increasing mass

11. What is the heat capacity of a substance that requires 500 J of heat to increase its
temperature by 25 °C?

 A) 10 J/°C
 B) 20 J/°C
 C) 25 J/°C
 D) 50 J/°C

, 12. If water is used to absorb heat in a reaction, what effect will this have on the water's
temperature?

 A) The temperature will decrease
 B) The temperature will remain the same
 C) The temperature will increase
 D) The temperature will oscillate

14. In an exothermic reaction, the surroundings:

 A) Absorb heat from the reaction
 B) Release heat to the reaction
 C) Experience an increase in temperature
 D) Both A and C are correct

15. When calculating heat transfer, what does a negative q value indicate?

 A) Heat is absorbed by the substance
 B) Heat is released by the substance
 C) The temperature remains constant
 D) The process is reversible

11. Consider the following reactions:

1. C(s) + O₂(g) → CO₂(g), ΔH = -393.5 kJ

2. H₂(g) + ½ O₂(g) → H₂O(l), ΔH = -285.8 kJ

3. C(s) + 2 H₂(g) → CH₄(g), ΔH = -74.8 kJ

Using Hess's Law, calculate the enthalpy change for the following reaction:

CH₄(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(l)

 A) -890.36 kJ

 B) -75.2 kJ

 C) -393.5 kJ

 D) -285.8 kJ

12. In the context of the reaction between NaCl and AgNO₃, what does a positive heat value
indicate?

 A) The reaction absorbs heat from the surroundings.

 B) The reaction releases heat to the surroundings.

 C) The reaction occurs at a constant temperature.