Lesson 3.1.4.2

3.1.4.2 Calorimetry Quiz: AQA Chemistry, Unit 1

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 3.1.4.2, Calorimetry: 20 multiple choice questions for the AQA Chemistry (7405), Unit 1: Physical chemistry, written with Revision Ninja.

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The 20 questions

  1. In the calorimetry equation q = mcΔT, what does m represent?

    • Mass of vessel
    • Mass of liquid
    • Molar mass
    • Mass of solute

  2. What are the units of specific heat capacity, c, in q = mc delta T when mass is in grams?

    • kJ mol-1
    • J g-1 K-1
    • mol dm-3
    • g cm-3

  3. What is the unit of q when m is in grams, c is in J g-1 K-1 and delta T is in kelvin?

    • g
    • kJ mol-1
    • K
    • J

  4. In the calorimetry equation q = mcΔT, which letter represents specific heat capacity?

    • m
    • q
    • c
    • ΔT

  5. To calculate molar enthalpy change from heat energy q, what is q divided by?

    • Mass in grams
    • Temperature change
    • Specific heat capacity
    • Number of moles

  6. Which simple calorimeter is commonly used in school calorimetry experiments?

    • Copper calorimeter
    • Conical flask
    • Glass beaker
    • Polystyrene cup

  7. Which unit is used for molar enthalpy change?

    • kJ mol-1
    • mol dm-3
    • J g-1
    • g mol-1

  8. How much heat is needed to warm 50.0 cm3 of water by 6.0 K? Use c = 4.18 J g-1 K-1 and density 1.00 g cm-3.

    • 1254 J
    • 209 J
    • 12.5 kJ
    • 2508 J

  9. 0.50 g of ethanol (Mr = 46) burns and warms 100 g of water by 15.0 K. What is the enthalpy of combustion per mole? Use c = 4.18 J g-1 K-1.

    • +577 kJ mol-1
    • -12.5 kJ mol-1
    • -577 kJ mol-1
    • -6.27 kJ mol-1

  10. A reaction of 0.0100 mol releases 50.0 kJ mol-1 of heat into 100 g of solution with c = 4.18 J g-1 K-1. What is the temperature rise?

    • 0.12 K
    • 1.20 K
    • 12.0 K
    • 0.50 K

  11. 200 g of water absorbs 8360 J of energy. With c = 4.18 J g-1 K-1, what is the temperature rise?

    • 10.0 K
    • 5.00 K
    • 0.100 K
    • 20.0 K

  12. Why is polystyrene used to make simple cup calorimeters?

    • Good thermal insulator
    • Chemically reactive
    • High heat capacity
    • Good thermal conductor

  13. A calorimeter transfers 2.09 kJ of energy to 100 g of water with c = 4.18 J g-1 K-1. What is the temperature rise?

    • 0.200 K
    • 5.00 K
    • 2.09 K
    • 50.0 K

  14. A reaction releases 1.50 kJ of heat from 0.0300 mol of reactant. What is the molar enthalpy change?

    • +50.0 kJ mol-1
    • -0.45 kJ mol-1
    • -50.0 kJ mol-1
    • -1.50 kJ mol-1

  15. A student heats 50 g of water from 20 C to 35 C. How much energy is absorbed? Use c = 4.18 J g-1 K-1.

    • 10450 J
    • 2.09 J
    • 3135 J
    • 209 J

  16. 1.00 g of a solid of Mr 60 releases 3.00 kJ of heat when it reacts with excess reagent. What is the molar enthalpy change?

    • -18.0 kJ mol-1
    • -3.00 kJ mol-1
    • -180 kJ mol-1
    • +180 kJ mol-1

  17. Why is an experimental enthalpy change often less exothermic than the literature value?

    • Impure water
    • Incomplete ionisation
    • Heat loss
    • High atmospheric pressure

  18. What effect does heat loss have on a calculated experimental enthalpy change?

    • No effect
    • Flips the sign
    • Overestimates magnitude
    • Underestimates magnitude

  19. What mass of ethanol (Mr = 46) must burn to release 5.00 kJ of heat, given delta cH = -1367 kJ mol-1?

    • 1.37 g
    • 0.0797 g
    • 0.0037 g
    • 0.168 g

  20. A reaction of 0.250 mol releases 7.5 kJ of heat into 100 g of water (c = 4.18 J g-1 K-1). What is the temperature rise?

    • 1.79 K
    • 75.0 K
    • 17.9 K
    • 7.5 K

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