plumiCalorimetry: AQA A‑Level Chemistry questions
AQA A-Level Chemistry past-paper questions on 3.1.4.2 Calorimetry, 2008–2025, with mark schemes and examiner’s reports where available.
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Q01.2
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All 72 questions on Calorimetry, as a list
- June 2025, Paper 3, Q01.2 (5 marks): A student does an experiment to determine a value for the enthalpy of solution of potassium hydroxide. The student uses this method. • Add some distilled water
- June 2025, Paper 3, Q01.4 (1 mark): Suggest why the value calculated in Question 01.3 is different from the experimental value given in Question 01.2. [1 mark]
- June 2025, AS Paper 1, Q18 (1 mark): The reaction between hydrochloric acid and sodium hydroxide is exothermic. Which row shows the solutions that will give the greatest temperature increase when m
- June 2025, AS Paper 2, Q07.2 (5 marks): The enthalpy of combustion of ethanol is –1371 kJ mol–1 A sample of ethanol is burned completely in air to raise the temperature of 55.0 g of water by 46.2 °C C
- June 2024, Paper 2, Q11.1 (4 marks): Limonene is found in the skin of citrus fruits. Figure 6 shows a diagram of the apparatus used in an experiment to determine a value for the enthalpy of combust
- June 2024, Paper 2, Q11.2 (5 marks): Table 3 shows values, obtained by different methods, for the enthalpy of combustion of a different liquid hydrocarbon. Table 3 Method Enthalpy of combustion / k
- June 2024, AS Paper 1, Q08.4 (6 marks): Identify three aspects of this method which could cause inaccurate results. Describe how the student could improve these three aspects of the method to obtain m
- June 2023, Paper 2, Q08.2 (5 marks): Palmitic acid burns in air. In a calorimetry experiment, combustion of 387 mg of palmitic acid increases the temperature of 0.150 kg of water from 23.9 °C to 37
- June 2023, Paper 2, Q08.3 (2 marks): State how the value calculated in Question 08.2 is likely to differ from data book values. Give one reason, other than heat loss, for this difference. [2 marks]
- June 2023, Paper 3, Q05.1 (3 marks): Calculate ∆Hvap for water. [1 kW = 1 kJ s–1] [3 marks] ∆Hvap kJ mol–1
- June 2023, AS Paper 2, Q05.1 (3 marks): The student finds that when all the alcohol is burned, the temperature of the water increases from 18.9 °C to 78.1 °C Calculate the enthalpy of combustion, in k
- June 2023, AS Paper 2, Q05.2 (2 marks): Table 2 shows the enthalpies of combustion of some alcohols. Table 2 Alcohol Enthalpy of combustion / kJ mol –1 Ethanol –1367 Propan-1-ol –2021 Butan-1-ol –2676
- June 2022, Paper 3, Q01.3 (3 marks): A student does an experiment to determine a value for the enthalpy of solution for ammonium nitrate. The student uses this method. • Measure 25.0 cm3 of distill
- June 2022, Paper 3, Q01.4 (1 mark): The uncertainty in each of the temperature readings from the thermometer used in this experiment is ±0.1°C Calculate the percentage uncertainty in the temperatu
- June 2022, Paper 3, Q01.5 (2 marks): Suggest a change to the student’s method, using the same apparatus, that would reduce the percentage uncertainty in the temperature change. Give a reason for yo
- June 2022, Paper 3, Q01.6 (1 mark): Another student obtained a value of +15 kJ mol−1 using the same method. Suggest the main reason for the difference between this experimental value for the entha
- June 2022, AS Paper 2, Q07.4 (4 marks): A student investigated the combustion of propanone (C3H6O) using calorimetry. A copper calorimeter containing water was heated by the complete combustion of som
- November 2021, Paper 2, Q03.1 (2 marks): Design a table to record all the readings necessary to determine an experimental value for the enthalpy of combustion for heptane in this experiment. [2 marks]
- November 2021, Paper 2, Q03.2 (2 marks): The student considered using a glass beaker on a tripod and gauze instead of the clamped copper calorimeter. Suggest two disadvantages of using a glass beaker o
- November 2021, Paper 2, Q03.3 (2 marks): Suggest two reasons why the value of enthalpy of combustion from this experiment is less exothermic than a data book value. [2 marks] Reason 1 Reason 2
- November 2021, Paper 2, Q03.4 (1 mark): Suggest one addition to this apparatus that would improve the accuracy of the enthalpy value obtained. [1 mark]
- November 2021, AS Paper 1, Q07.2 (3 marks): A student does an experiment to determine the enthalpy of combustion of propan-1-ol (CH3CH2CH2OH, Mr = 60.0). Combustion of 0.497 g of propan-1-ol increases the
- November 2021, AS Paper 1, Q07.3 (1 mark): The enthalpy of combustion determined experimentally is less exothermic than that calculated using enthalpies of formation. Give one possible reason for this, o
- November 2020, Paper 3, Q05.1 (3 marks): The heat energy released in the calorimeter, q = Ccal∆T Calculate the heat capacity (Ccal) in kJ K−1 [3 marks] Ccal kJ K−1
- November 2020, Paper 3, Q05.2 (2 marks): When the experiment is repeated with 2.00 g of octane (Mr = 114.0) the temperature change recorded is 12.2 °C Calculate the heat change, in kJ mol−1, for octane
- November 2020, Paper 3, Q05.4 (2 marks): The thermometer used to measure the temperature change of 12.2 °C in Question 05.2 has an uncertainty of ± 0.1 °C in each reading. Calculate the percentage unce
- November 2020, AS Paper 1, Q04.2 (6 marks): A student determines the enthalpy change for the reaction between calcium carbonate and hydrochloric acid. CaCO3(s) + 2 HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l) Th
- November 2020, AS Paper 1, Q04.3 (5 marks): In a different experiment 50.0 cm3 of 0.500 mol dm–3 aqueous hydrochloric acid are reacted with 50.0 cm3 of 0.500 mol dm–3 aqueous sodium hydroxide. NaOH(aq) +
- November 2020, AS Paper 1, Q04.4 (1 mark): Suggest how, without changing the apparatus, the experiment in Question 04.3 could be improved to reduce the percentage uncertainty in the temperature change. [
- November 2020, AS Paper 2, Q22 (1 mark): The temperature changed from 21.8 °C to 19.2 °C during a calorimetry experiment. The uncertainty of each reading of the thermometer is ±0.1 °C What is the perce
- November 2020, AS Paper 2, Q23 (1 mark): An experiment is done to determine the enthalpy of combustion of a fuel using a calorimeter containing water. b = mass of fuel burned / g w = mass of water heat
- June 2019, AS Paper 1, Q20 (1 mark): Some fuel in a spirit burner is burned, and the heat produced is used to heat a container of water. In this experiment: The mass of water heated = m g The tempe
- June 2019, AS Paper 2, Q03.1 (4 marks): A student determined the enthalpy of combustion of cyclohexane (C6H12). The student • placed a pure sample of cyclohexane in a spirit burner • placed the spirit
- June 2019, AS Paper 2, Q03.2 (1 mark): A data book value for the enthalpy of combustion of cyclohexane is –3920 kJ mol−1 The student concluded that the temperature rise recorded in the experiment was
- June 2018, Paper 2, Q03.4 (3 marks): A student carried out an experiment to determine the enthalpy of combustion of ethanol. Combustion of 457 mg of ethanol increased the temperature of 150 g of wa
- June 2018, Paper 3, Q04.1 (5 marks): Plot a graph of temperature against time on the grid opposite. Use your graph to find the temperature rise, ∆T, at the fourth minute. Show your working on the g
- June 2018, Paper 3, Q04.2 (1 mark): The uncertainty in each of the temperature readings from the thermometer used in this experiment was ±0.1° C Calculate the percentage uncertainty in the value f
- June 2018, Paper 3, Q04.3 (1 mark): Suggest a change to the experiment that would minimise heat loss. [1 mark]
- June 2018, Paper 3, Q04.4 (2 marks): Suggest and explain another change to the experiment that would decrease the percentage uncertainty in the use of the same thermometer. [2 marks]
- June 2018, Paper 3, Q04.5 (5 marks): A second student completed an experiment to determine the enthalpy of neutralisation for the reaction between ethanedioic acid solution (HOOCCOOH) and potassium
- June 2018, Paper 3, Q04.6 (2 marks): In a similar experiment to that in Question 04.5, the enthalpy of neutralisation for the reaction between sulfuric acid and potassium hydroxide solution was fou
- June 2018, AS Paper 2, Q03.1 (4 marks): When ethanoic acid reacts with sodium hydroxide, the enthalpy change, ∆H, is –56.1 kJ mol–1 CH3COOH(aq) + NaOH(aq) ⟶ CH3COONa(aq) + H2O(l) Calculate the tempera
- June 2018, AS Paper 2, Q03.2 (2 marks): A student recorded the temperature of aqueous ethanoic acid in a polystyrene cup for three minutes. At the fourth minute, the student added sodium hydrogencarbo
- June 2017, Paper 3, Q01.1 (1 mark): Suggest one reason why the enthalpy change for this reaction cannot be determined directly by calorimetry. [1 mark]
- June 2017, Paper 3, Q01.3 (6 marks): Describe how you would carry out an experiment to determine the enthalpy of solution of anhydrous magnesium chloride. You should use about 0.8 g of anhydrous ma
- June 2017, AS Paper 1, Q03.1 (6 marks): Show by calculation which reactant was in excess. Use the data to calculate the experimental value for enthalpy of reaction in kJ mol−1(Assume that the specific
- June 2017, AS Paper 1, Q03.2 (1 mark): Another student used the same method and obtained a value for the enthalpy of reaction of −142 kJ mol−1 A data book value for the enthalpy of reaction is −310 k
- June 2017, AS Paper 1, Q03.3 (6 marks): Suggest how the students’ method, and the analysis of the results, could be improved in order to determine a more accurate value for the enthalpy of reaction. J
- June 2016, AS Paper 2, Q02.1 (4 marks): A student carried out an experiment to determine the enthalpy of combustion of methanol. Methanol was placed in a spirit burner and the mass of the spirit burne
- June 2016, AS Paper 2, Q02.2 (1 mark): Suggest one reason, other than incomplete combustion or heat transfer to the atmosphere, why the student’s value for the enthalpy of combustion of methanol is d
- June 2016, AS Paper 2, Q02.3 (1 mark): The uncertainty in each of the temperature readings from the thermometer in this experiment was ±0.25 °C. This gave an overall uncertainty in the temperature ri
- June 2016, AS Paper 2, Q02.4 (1 mark): The student said correctly that using a thermometer with an overall uncertainty for the rise in temperature of ±0.5 °C was adequate for this experiment. Explain
- Specimen, Paper 1, Q09.1 (4 marks): 9 A 5.00 g sample of potassium chloride was added to 50.0 g of water initially at 20.0 °C. The mixture was stirred and as the potassium chloride dissolved, the
- Specimen, Paper 1, Q09.2 (4 marks): Enthalpy of solution = kJ mo 5
- June 2015, CHEM2 (old spec), Q7(c) (3 marks): A student determined a value for the enthalpy change when a sample of propanone was burned. The heat produced was used to warm some water in a copper calorimete
- June 2015, CHEM2 (old spec), Q7(f) (2 marks): Suggest two reasons why the value obtained by the student in Question 7 (c) is different from the value calculated in Question 7 (e). [2 marks] Reason 1 Reason
- June 2014, CHEM2 (old spec), Q9(b) (5 marks): A student carried out a laboratory experiment to determine the enthalpy change when a sample of ethanol was burned. The heat produced was used to warm some wate
- June 2013, CHEM5 (old spec), Q2(c)(ii) (5 marks): A solution is formed when 5.00 g of potassium chloride are dissolved in 20.0 g of water. The initial temperature of the water is 298 K. Calculate the final temp
- January 2013, CHEM2 (old spec), Q4(d)(i) (3 marks): Use these data to calculate the enthalpy change, in kJ mol–1, for this reaction of copper(II) sulfate. This is the student value for ΔH1 In this experiment, you
- January 2013, CHEM2 (old spec), Q4(d)(ii) (1 mark): Suggest one reason why the student value for ΔH1 calculated in part (d) (i) is less accurate than the data book value given in part (c). (1 mark)
- June 2012, CHEM2 (old spec), Q2(e) (3 marks): A student carried out an experiment to determine the enthalpy change when a sample of methanol was burned. The student found that the temperature of 140 g of wa
- January 2011, CHEM2 (old spec), Q9(b) (3 marks): The student carried out a laboratory experiment to determine the enthalpy change when a sample of butan-1-ol was burned. The student found that the temperature
- January 2011, CHEM2 (old spec), Q9(d)(ii) (2 marks): Give two reasons why the experimental values obtained by the student are lower than the calculated values using the enthalpy of formation data.
- June 2010, CHEM2 (old spec), Q8(d) (4 marks): A student carried out a simple laboratory experiment to measure the enthalpy change for Process 3. The student showed that the temperature of 200 g of water inc
- June 2009, CHEM2 (old spec), Q3(a)(i) (1 mark): 3 (a) (i) Write an expression for the heat change (q) which relates mass (m), specific heat capacity (c) and change in temperature (∆T). (1 mark)
- June 2009, CHEM2 (old spec), Q3(a)(ii) (1 mark): 3 (a) (ii) Calculate the amount of heat required to increase the temperature of 8.80 g of ethyl ethanoate by 9.5 K during the mixing process. (You should assume
- June 2009, CHEM2 (old spec), Q3(a)(iii) (1 mark): 3 (a) (iii) Calculate the amount of heat required to increase the temperature of 11.95 g of trichloromethane by 9.5 K during the mixing process. (You should ass
- June 2009, CHEM2 (old spec), Q3(a)(iv) (2 marks): 3 (a) (iv) Using the values from parts (a) (ii) and (a) (iii), calculate the molar enthalpy change in kJ mol–1 for the mixing process. (2 marks)
- June 2009, CHEM2 (old spec), Q3(b) (1 mark): 3 (b) The students deduced that the heat change was due only to the formation of intermolecular forces between ethyl ethanoate molecules and trichloromethane mo
- June 2008, CHM5 (2008 spec), Q9(a) (5 marks): 9 (a) Calculate the mass of methanol that should be burned in order to raise the temperature of 1.00kg of water from 20.0°C to 100°C. The enthalpy of combustion
- January 2008, CHM2 (2008 spec), Q3(e) (4 marks): (e) In an experiment 0.92 g of propan-1-ol, C3H7OH, was burned and the heat given off used to raise the temperature of 250g of water. The temperature rise was 1
- January 2008, CHM2 (2008 spec), Q3(f) (1 mark): (f) Suggest why the experimental value of the enthalpy of combustion obtained in part (e) is less reliable than the value obtained in part (c). (1 mark)
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