Questions on Calorimetry
Multiple-Choice Questions – Calorimetry
1. What is the primary purpose of calorimetry?
A) To calculate entropy
B) To measure heat transfer
C) To find molecular mass
D) To analyze chemical structure
E) To determine gas pressure
2. A calorimeter is a device used to:
A) Separate compounds
B) Analyze gases
C) Measure temperature directly
D) Measure heat change in a process
E) Determine pH levels
3. What does the specific heat capacity of a substance represent?
A) Heat needed to boil 1 g of it
B) Heat required to melt 1 mol
C) Heat needed to raise 1 g by 1°C
D) Energy in one mole
E) Heat lost per second
4. Which of the following is the correct unit for specific heat?
A) J
B) J/mol
C) J/g·°C
D) °C/J
E) cal/mol
5. The formula used in calorimetry to calculate heat is:
A) q = mcΔT
B) q = PV
C) q = ΔH/T
D) q = mRT
E) q = E – PΔV
6. What does "q" represent in calorimetry?
A) Heat absorbed or released
B) Pressure of a system
C) Energy of a bond
D) Entropy
E) Volume of gas
7. In a calorimetry experiment, the mass used in the equation refers to:
A) Total mass of system
B) Mass of the heat source
C) Mass of the thermometer
D) Mass of the substance gaining or losing heat
E) Mass of the calorimeter
8. Which of the following statements is true?
A) Calorimeters produce heat
B) Calorimetry only applies to solids
C) Heat lost = heat gained
D) Calorimetry requires vacuum
E) Energy is created in calorimetry
9. In an endothermic process observed in a calorimeter, the temperature of the surroundings:
A) Increases
B) Decreases
C) Remains constant
D) Becomes negative
E) Doubles
10. A substance with a low specific heat will:
A) Require more heat to change temperature
B) Heat up quickly
C) Not change temperature
D) Never cool down
E) Be a good insulator
11. Which of these materials has the highest specific heat capacity?
A) Lead
B) Water
C) Gold
D) Iron
E) Mercury
12. In bomb calorimetry, the reaction occurs at:
A) Constant volume
B) Constant pressure
C) Constant temperature
D) Constant mass
E) Constant entropy
13. Which component of a calorimeter ensures minimal heat exchange with surroundings?
A) Metal container
B) Air gap
C) Insulating walls
D) Thermometer
E) Reaction chamber
14. In the equation q = mcΔT, what does ΔT represent?
A) Absolute temperature
B) Mass loss
C) Heat capacity
D) Change in temperature
E) Heat of fusion
15. A reaction releases 500 J of heat. What is the sign of q?
A) Positive
B) Negative
C) Zero
D) Undefined
E) Depends on specific heat
16. What is the heat gained by 100 g of water (c = 4.18 J/g°C) heated from 25°C to 75°C?
A) 209 J
B) 5000 J
C) 20900 J
D) 10450 J
E) 4180 J
17. Why is water often used in calorimetry?
A) High boiling point
B) Low density
C) Low reactivity
D) High specific heat
E) It evaporates easily
18. If a metal cools down in water inside a calorimeter, the metal is:
A) Gaining heat
B) Losing mass
C) Releasing heat
D) Not interacting
E) Undergoing fusion
19. Calorimetry is based on which law of thermodynamics?
A) Zeroth
B) First
C) Second
D) Third
E) Law of Entropy
20. Which of the following would increase accuracy in a calorimetry experiment?
A) Using an open container
B) Stirring constantly
C) Using a poor conductor
D) Adding dry ice
E) Heating with an open flame
- Questions about Exothermic and Endothermic Processes
- Questions on Heat Capacity and Specific Heat
- Questions on Enthalpy
Answers with Explanations
1. B – Calorimetry measures heat transfer during physical or chemical changes.
2. D – A calorimeter is used to measure heat flow.
3. C – Specific heat is the heat required to raise the temp of 1 g of a substance by 1°C.
4. C – The correct unit is J/g·°C.
5. A – The main calorimetry equation is q = mcΔT.
6. A – "q" represents the heat absorbed or released by the substance.
7. D – The mass in q = mcΔT refers to the substance undergoing the temperature change.
8. C – Energy is conserved: heat lost = heat gained.
9. B – In endothermic reactions, surroundings lose heat, so temperature decreases.
10. B – Low specific heat means the substance heats up (or cools down) quickly.
11. B – Water has the highest specific heat capacity of the listed options.
12. A – Bomb calorimeters operate at constant volume.
13. C – Insulating walls prevent heat loss to surroundings.
14. D – ΔT is the change in temperature: final – initial.
15. B – Heat released = q is negative (exothermic).
16. C – q = 100 × 4.18 × (75–25) = 20,900 J.
17. D – Water has a high specific heat, making it ideal for absorbing/releasing heat.
18. C – As the metal cools, it releases heat to the water.
19. B – Calorimetry relies on the First Law: energy is conserved.
20. B – Stirring ensures even temperature distribution, improving accuracy.
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