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 q = mc delta T, what does m represent?

    • The number of moles of product formed in the reaction
    • The mass of the substance whose temperature changes
    • The molar mass of the reactant, in grams per mole
    • The mass of the calorimeter container and its lid

  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. Which quantity in q = mc delta T is the specific heat capacity?

    • delta T, the temperature change of the substance measured by a thermometer
    • m, the mass of the substance in grams, measured with a balance before heating
    • c, the energy needed to raise the temperature of 1 g of a substance by 1 K
    • q, the heat transferred to or from the surroundings during the reaction

  5. To convert q into a molar enthalpy change, what is q divided by?

    • The mass of the calorimeter, measured in grams before the experiment starts
    • The temperature change of the solution measured during the experiment
    • The volume of the calorimeter in cubic centimetres after the reaction
    • The number of moles of the limiting substance

  6. Which equipment is used in the calorimetry practical in the specification?

    • An electrolysis cell
    • A titration burette only
    • A Bunsen burner and crucible only
    • A polystyrene cup with a thermometer

  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 a polystyrene cup used as a calorimeter in school practicals?

    • To reduce heat loss to the surroundings
    • To change the enthalpy of the reaction
    • To react with the acid being measured
    • To increase the rate of the reaction

  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. A student's value for the enthalpy change is -48 kJ mol-1, but the literature value is -56 kJ mol-1. Which is a valid reason for the difference?

    • Students cannot measure the temperature accurately, so every calorimetry result is unreliable overall
    • The sign of the enthalpy change was reported incorrectly, so the answer should be positive
    • Heat was lost to the surroundings, and the solution was assumed to have the specific heat capacity of water
    • The Mr of the reactant was entered too large, which changes the moles used in the calculation

  18. A reaction is carried out in an open container with no lid. Why does this make the measured enthalpy change smaller in magnitude?

    • Evaporation has no effect on the temperature, so the measured rise is unaffected overall
    • The specific heat capacity of the solution increases, so less energy warms the solution
    • The reaction takes in extra heat from the air, which makes the temperature rise larger
    • Heat is lost to the surroundings, so the temperature rise is smaller

  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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