plumiEnergetics: AQA A‑Level Chemistry questions
Every AQA A-Level Chemistry exam question on 3.1.4 Energetics, 2016–2025, with its mark scheme and examiner’s report.
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Calculations
Q04.1
The whole paper ↗![June 2025 Paper 1, question 04.1: Give the standard conditions indicated by the symbol o in ΔfH o and S o [1 mark]](https://pub-e8a9dbab8e2a4d089f52b2a45e0d0b50.r2.dev/bank/74051-jun25-04-1-qp.webp)
Q04.3
The whole paper ↗![June 2025 Paper 1, question 04.3: Assume that the bonds between N and O in NO2 are the same. Calculate the mean bond enthalpy, in kJ mol–1, for a bond between N and O in NO2 [3 marks] Bond entha](https://pub-e8a9dbab8e2a4d089f52b2a45e0d0b50.r2.dev/bank/74051-jun25-04-3-qp.webp)
Q01.1
The whole paper ↗![June 2025 Paper 3, question 01.1: Give the equation, including state symbols, for the process that occurs when the enthalpy of solution of potassium hydroxide is determined. [1 mark]](https://pub-e8a9dbab8e2a4d089f52b2a45e0d0b50.r2.dev/bank/74053-jun25-01-1-qp.webp)
Q01.2
The whole paper ↗
Q01.4
The whole paper ↗![June 2025 Paper 3, question 01.4: Suggest why the value calculated in Question 01.3 is different from the experimental value given in Question 01.2. [1 mark]](https://pub-e8a9dbab8e2a4d089f52b2a45e0d0b50.r2.dev/bank/74053-jun25-01-4-qp.webp)
Q07.1
The whole paper ↗![June 2025 AS Paper 2, question 07.1: Define enthalpy change. [1 mark]](https://pub-e8a9dbab8e2a4d089f52b2a45e0d0b50.r2.dev/bank/74042-jun25-07-1-qp.webp)
Q07.2
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Q07.3
The whole paper ↗![June 2025 AS Paper 2, question 07.3: Use Table 2 to show that an expression for the sum of the bond enthalpies for all the bonds in the products is 2536n + 926 [1 mark]](https://pub-e8a9dbab8e2a4d089f52b2a45e0d0b50.r2.dev/bank/74042-jun25-07-3-qp.webp)
Q07.4
The whole paper ↗
![June 2025 AS Paper 2, question 22: Which reaction at 298 K has a standard enthalpy change equal to the standard enthalpy of formation of liquid iodoethane? [1 mark] A 1 2 I2(I) + 2 C(s) + 5 2 H2(](https://pub-e8a9dbab8e2a4d089f52b2a45e0d0b50.r2.dev/bank/74042-jun25-22-qp.webp)
Q11.1
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Q11.2
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Q08.1
The whole paper ↗![June 2024 AS Paper 1, question 08.1: Define standard enthalpy of formation. [2 marks]](https://pub-e8a9dbab8e2a4d089f52b2a45e0d0b50.r2.dev/bank/74041-jun24-08-1-qp.webp)
Q08.2
The whole paper ↗
Q08.3
The whole paper ↗![June 2024 AS Paper 1, question 08.3: Suggest why the enthalpy change for the thermal decomposition of solid silver nitrate(III) is difficult to determine experimentally. [1 mark]](https://pub-e8a9dbab8e2a4d089f52b2a45e0d0b50.r2.dev/bank/74041-jun24-08-3-qp.webp)
Q08.4
The whole paper ↗
![June 2024 AS Paper 2, question 19: What is the enthalpy of combustion, in kJ mol–1, of propane? [1 mark] A −211.7 B −419.7 C −2220 D −2878](https://pub-e8a9dbab8e2a4d089f52b2a45e0d0b50.r2.dev/bank/74042-jun24-19-qp.webp)
![June 2024 AS Paper 2, question 20: What is the enthalpy change, in kJ mol–1, when butane reacts to form propane, hydrogen and carbon? [1 mark] A +21.2 B +17.5 C −17.5 D −21.2](https://pub-e8a9dbab8e2a4d089f52b2a45e0d0b50.r2.dev/bank/74042-jun24-20-qp.webp)
All 112 questions on Energetics, as a list
- June 2025, Paper 1, Q04.1 (1 mark): Give the standard conditions indicated by the symbol o in ΔfH o and S o [1 mark]
- June 2025, Paper 1, Q04.3 (3 marks): Assume that the bonds between N and O in NO2 are the same. Calculate the mean bond enthalpy, in kJ mol–1, for a bond between N and O in NO2 [3 marks] Bond entha
- June 2025, Paper 3, Q01.1 (1 mark): Give the equation, including state symbols, for the process that occurs when the enthalpy of solution of potassium hydroxide is determined. [1 mark]
- 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, Q07.1 (1 mark): Define enthalpy change. [1 mark]
- 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 2025, AS Paper 2, Q07.3 (1 mark): Use Table 2 to show that an expression for the sum of the bond enthalpies for all the bonds in the products is 2536n + 926 [1 mark]
- June 2025, AS Paper 2, Q07.4 (3 marks): An expression for the sum of the bond enthalpies for all the bonds in the reactants is 1916n + 724 A calculated value for the enthalpy of combustion of an alkan
- June 2025, AS Paper 2, Q18 (1 mark): The standard enthalpies of combustion for carbon, hydrogen and benzene (C6H6) are –394, –286 and –3273 kJ mol–1 respectively. What is the standard enthalpy of f
- June 2025, AS Paper 2, Q22 (1 mark): Which reaction at 298 K has a standard enthalpy change equal to the standard enthalpy of formation of liquid iodoethane? [1 mark] A 1 2 I2(I) + 2 C(s) + 5 2 H2(
- 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, Q08.1 (2 marks): Define standard enthalpy of formation. [2 marks]
- June 2024, AS Paper 1, Q08.2 (2 marks): Silver nitrate(V) is formed when silver nitrate(III) undergoes thermal decomposition. 2 AgNO2(s) ⟶ Ag(s) + AgNO3(s) + NO(g) ΔH = +56.2 kJ mol–1 The standard ent
- June 2024, AS Paper 1, Q08.3 (1 mark): Suggest why the enthalpy change for the thermal decomposition of solid silver nitrate(III) is difficult to determine experimentally. [1 mark]
- 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 2024, AS Paper 2, Q19 (1 mark): What is the enthalpy of combustion, in kJ mol–1, of propane? [1 mark] A −211.7 B −419.7 C −2220 D −2878
- June 2024, AS Paper 2, Q20 (1 mark): What is the enthalpy change, in kJ mol–1, when butane reacts to form propane, hydrogen and carbon? [1 mark] A +21.2 B +17.5 C −17.5 D −21.2
- 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 2, Q08.6 (3 marks): Ethanol is a biofuel that can be produced by the fermentation of glucose. C6H12O6 → 2 C2H5OH + 2 CO2 Glucose has the structural formula shown. Table 3 shows som
- June 2023, Paper 2, Q08.7 (2 marks): The carbon dioxide produced from fermentation can be reacted with steam to make more ethanol. The equation for this reaction is 2 CO2(g) + 3 H2O(g) → C2H5OH(g)
- 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, Paper 3, Q10 (1 mark): Which reaction has a standard enthalpy change equal to the standard enthalpy of formation for barium chloride? [1 mark] A Ba(g) + Cl2(g) → BaCl2(s) B Ba2+(g) +
- June 2023, AS Paper 1, Q15 (1 mark): Which reaction has an enthalpy change equal to the standard enthalpy of formation of potassium oxide? [1 mark] A 4 K(s) + O2(g) → 2 K2O(s) B 2 K(s) + O(g) → K2O
- 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 2023, AS Paper 2, Q05.3 (3 marks): The equation for the complete combustion of gaseous pentan-1-ol is shown. CH3(CH2)3CH2OH(g) + 7 1 2 O2(g) → 5 CO2(g) + 6 H2O(g) ΔH= –3388 kJ mol–1 Table 3 shows
- June 2023, AS Paper 2, Q05.4 (2 marks): The energy stored in fuels can be compared using energy density values measured in kJ dm–3 Calculate the energy density of butan-1-ol. enthalpy of combustion of
- June 2022, Paper 1, Q03.5 (5 marks): Hydrazine (N2H4) is used as a rocket fuel that is oxidised by hydrogen peroxide. The equation for this reaction in the gas phase is The enthalpy change for this
- 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, Q07.3 (2 marks): Table 2 shows the enthalpies of combustion of the three fuels from the fermentation of silverskin. Table 2 Fuel Standard enthalpy of combustion / kJ mol–1 Energ
- 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
- June 2022, AS Paper 2, Q07.5 (3 marks): Butan-1-ol can be added to petrol for cars. An equation for the complete combustion of gaseous butan-1-ol is shown. C4H9OH(g) + 6 O2(g) → 4 CO2(g) + 5 H2O(g) ΔH
- November 2021, Paper 1, Q01.1 (1 mark): State the meaning of the term enthalpy change. [1 mark]
- 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, Paper 2, Q04.1 (3 marks): Use Figure 3 and the data shown in Table 1 to calculate ΔH2 [3 marks] Table 1 ΔH / kJ mol–1 Enthalpy of atomisation for carbon +715 Enthalpy of atomisation for
- November 2021, AS Paper 1, Q07.1 (2 marks): State the meaning of the term standard enthalpy of combustion. [2 marks]
- 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 2021, AS Paper 2, Q08.1 (1 mark): Define the term enthalpy change. [1 mark]
- November 2021, AS Paper 2, Q08.2 (4 marks): Propane undergoes complete combustion. C3H8(g) + 5 O2(g) ⟶ 3 CO2(g) + 4 H2O(l) ∆H = –2046 kJ mol–1 Table 3 shows some bond enthalpy data. Table 3 Bond C–H C=O O
- November 2021, AS Paper 2, Q08.3 (1 mark): Explain why the value given for the O=O bond enthalpy in Question 08.2 is not a mean value. [1 mark] Section B Answer all questions in this section. Only one an
- 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, Q05.3 (1 mark): State why the heat change calculated from the bomb calorimeter experiment is not an enthalpy change. [1 mark]
- 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, Paper 3, Q09 (1 mark): Which reaction has an enthalpy change equal to the standard enthalpy of formation of silver iodide? [1 mark] A Ag(g) + 1 2 I2(g) → AgI(s) B Ag(s) + 1 2 I2(s) →
- November 2020, Paper 3, Q10 (1 mark): Some bond enthalpies are given. Bond C H O H O=O C=O Bond enthalpy/ kJ mol–1 412 463 496 743 Which is the enthalpy change of this reaction in kJ mol−1? CH4(g) +
- November 2020, AS Paper 1, Q04.1 (1 mark): State the meaning of the term enthalpy change as applied to a chemical reaction. [1 mark]
- 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 1, Q12 (1 mark): Which reaction has an enthalpy change equal to the standard enthalpy of formation of lithium fluoride? [1 mark] A Li(g) + 1 2 F2(g) → LiF(s) B Li+(g) + F–(g) →
- November 2020, AS Paper 1, Q20 (1 mark): Two reactions of iron with oxygen are shown. Fe(s) + 1 2 O2(g) → FeO(s) ΔH = – 272 kJ mol–1 2 Fe(s) + 3 2 O2(g) → Fe2O3(s) ΔH = – 822 kJ mol–1 What is the entha
- November 2020, AS Paper 2, Q01.1 (2 marks): Define the term standard enthalpy of formation. [2 marks]
- November 2020, AS Paper 2, Q01.2 (3 marks): The equation for a reaction used to manufacture 1-chloropropane is 3 CH3CH2CH2OH(l) + PCl3(l) → 3 CH3CH2CH2Cl(l) + H3PO3(s) The enthalpy change for this reactio
- November 2020, AS Paper 2, Q21 (1 mark): Some enthalpy change data are shown. C(s) + 2 H2(g) → CH4(g) ΔH = –75 kJ mol–1 H2(g) → 2 H(g) ΔH = +436 kJ mol–1 What is the enthalpy change, in kJ mol–1, for t
- 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, Paper 3, Q08 (1 mark): Nitrogen dioxide is produced from ammonia and air as shown in these equations 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) ΔH = –909 kJ mol–1 2 NO(g) + O2(g) → 2 NO2
- June 2019, AS Paper 1, Q01.5 (3 marks): Hydrogen fluoride reacts with ethyne (C2H2) as shown in the equation. All compounds are in the gaseous state. ∆H = –179 kJ mol–1 Table 1 shows some mean bond en
- June 2019, AS Paper 1, Q14 (1 mark): Which equation represents the reaction that has a standard enthalpy change equal to the standard enthalpy of formation for barium chloride? [1 mark] A Ba(g) + C
- 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 2019, AS Paper 2, Q03.3 (3 marks): Table 2 gives some values of standard enthalpies of combustion (∆cHo). Table 2 Substance C(s) H2(g) C6H12(l) Standard enthalpy of combustion, ∆cHo / kJ mol–1 –3
- 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 1, Q07.5 (2 marks): Potassium chlorate(VII), KClO4, is used in fireworks. When potassium chlorate(VII) decomposes, it produces potassium chloride and oxygen. Give an equation for t
- 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 2018, AS Paper 2, Q20 (1 mark): What is the enthalpy of formation of buta-1,3-diene, C4H6(g)? Substance Enthalpy of combustion / kJ mol–1 C4H6(g) –2546 C(s) –394 H2(g) –286 [1 mark] A +112 kJ
- 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, Q01.2 (2 marks): Some enthalpies of solution are shown in Table 1. Table 1 Salt Enthalpy of solution / kJ mol−1 MgCl2(s) −155 MgCl2.4H2O(s) −39 Calculate the enthalpy change for
- 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, Q02.1 (1 mark): Write an equation, including state symbols, for the reaction with an enthalpy change equal to the enthalpy of formation for iron(III) oxide. [1 mark
- June 2017, AS Paper 1, Q02.2 (3 marks): Table 2 contains some standard enthalpy of formation data. Table 2 CO(g) Fe2O3(s) ΔfH o / kJ mol−1 −111 −822 Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ΔH = −19 kJ mo
- June 2017, AS Paper 1, Q02.3 (3 marks): Some enthalpy data are given in Table 3. Table 3 Process ΔH / kJ mol−1 N2(g) + 3H2(g) → 2NH3(g) −92 N2(g) → 2N(g) +944 H2(g) → 2H(g) +436 Use the data from Tabl
- June 2017, AS Paper 1, Q02.4 (1 mark): Give one reason why the bond enthalpy that you calculated in Question 2.3 is different from the mean bond enthalpy quoted in a data book (388 kJ mol−1). [1 mark
- 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 2017, AS Paper 2, Q04.2 (2 marks): An expression can be derived using bond enthalpy data to estimate the enthalpy of combustion (∆cH) of an alkane. For an alkane with n carbon atoms: ∆cH = – (496
- June 2017, AS Paper 2, Q04.3 (1 mark): Suggest one reason, other than the use of mean bond enthalpies, why a value for the enthalpy of combustion of a liquid alkane is different from the value obtain
- June 2017, AS Paper 2, Q04.4 (3 marks): Values of the enthalpy change for combustion of 1 g of some alkanes are shown in Table 2. Table 2 methane ethane propane butane pentane Enthalpy change in kJ fo
- June 2017, AS Paper 2, Q04.5 (2 marks): Isooctane (2,2,4-trimethylpentane) is an important component of petrol used in cars. When isooctane is burned, the enthalpy change is −47.8 kJ g−1 Isooctane is
- 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
- June 2016, AS Paper 2, Q02.5 (3 marks): The enthalpy of combustion of ethanol is −1371 kJ mol−1. The density of ethanol is 0.789 g cm−3. Calculate the heat energy released in kJ when 0.500 dm3 of etha
- June 2016, AS Paper 2, Q22 (1 mark): Some enthalpy data is given in Table 3. Table 3 Bond C−H O−H H−H C≡O Bond enthalpy / kJ mol−1 413 463 436 To be calculated Use the information in Table 3 and th
- Specimen, Paper 1, Q04.1 (3 marks): H–H bond enthalpy = kJ mo
- Specimen, Paper 1, Q04.2: 9
- Specimen, Paper 1, Q04.3 (1 mark): Suggest one environmental advantage of manufacturing methanol fuel by this reaction. [1 mark] 0 4 . 3
- 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
- Specimen, Paper 3, Q09 (1 mark): 6
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