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Equilibrium constant Kp for homogeneous systems: AQA A‑Level Chemistry questions

Every AQA A-Level Chemistry exam question on 3.1.10 Equilibrium constant Kp for homogeneous systems, 2016–2025, with its mark scheme and examiner’s report.

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2,301 questions

  1. Q04.1

    June 2024 · Paper 1

    2 marks3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    June 2024 Paper 1, question 04.1: A mixture of 2.00 mol of H2O(g) and 2.00 mol of CO(g) is allowed to reach equilibrium at a constant temperature in a 20 dm3 container. At equilibrium, there are

  2. Q04.2

    June 2024 · Paper 1

    1 mark3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    June 2024 Paper 1, question 04.2: State why the equilibrium constant (Kp) for this reaction has no units. [1 mark]

  3. Q04.4

    June 2024 · Paper 1

    4 marks3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    June 2024 Paper 1, question 04.4: Give an expression for Kp for this reaction. Calculate the value of Kp at 6000 kPa State the units. [4 marks] Kp Units

  4. Q04.5

    June 2024 · Paper 1

    1 mark3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    June 2024 Paper 1, question 04.5: State the effect, if any, of an increase in volume of the container on the value of Kp for this reaction at a constant temperature. [1 mark]

  5. Q04.1

    June 2023 · Paper 1

    3 marks3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    June 2023 Paper 1, question 04.1: A 0.317 mol sample of nitrogen dioxide is placed in a sealed flask and heated at a constant temperature until equilibrium is reached. At equilibrium, the flask

  6. Q04.2

    June 2023 · Paper 1

    1 mark3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    June 2023 Paper 1, question 04.2: The total pressure in the flask in Question 04.1 is 120 kPa at equilibrium. Calculate the partial pressure, in kPa, of NO2 If you were unable to answer Question

  7. Q04.3

    June 2023 · Paper 1

    3 marks3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    June 2023 Paper 1, question 04.3: Table 1 shows the mole fractions of the three gases in a different equilibrium mixture. 2 NO2(g) ⇌ 2 NO(g) + O2(g) ΔH = +113 kJ mol–1 Table 1 Gas Mole fraction

  8. Q04.4

    June 2023 · Paper 1

    2 marks3.1.6 Chemical equilibria, Le Chatelier’s principle and Kc3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    June 2023 Paper 1, question 04.4: The equilibrium mixture in Question 04.3 is compressed into a smaller volume. Deduce the effect, if any, of this change on the equilibrium yield of oxygen and o

  9. Q28

    June 2023 · Paper 3

    1 mark3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    June 2023 Paper 3, question 28: The equation for the complete combustion of butane is C4H10 + 6 1 2 O2 → 4 CO2 + 5 H2O What is the mole fraction of butane in a mixture of butane and oxygen wit

  10. Q01.3

    June 2022 · Paper 1

    3 marks3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    June 2022 Paper 1, question 01.3: Carbon monoxide and hydrogen react to form methanol. CO(g) + 2 H2(g) ⇌ CH3OH(g) 0.430 mol of carbon monoxide is mixed with 0.860 mol of hydrogen. At equilibrium

  11. Q01.4

    June 2022 · Paper 1

    1 mark3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    June 2022 Paper 1, question 01.4: Give an expression for the equilibrium constant (Kp) for this reaction. CO(g) + 2 H2(g) ⇌ CH3OH(g) [1 mark] Kp

  12. Q01.5

    June 2022 · Paper 1

    3 marks3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    June 2022 Paper 1, question 01.5: A different mixture of carbon monoxide and hydrogen is left to reach equilibrium at a temperature T. Some data for this equilibrium are shown in Table 1. Table

  13. Q01.6

    June 2022 · Paper 1

    2 marks3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    June 2022 Paper 1, question 01.6: Use the Kp value from Table 1 to calculate a value for Kp for the following reaction at temperature T. CH3OH(g) ⇌ CO(g) + 2 H2(g) Give the units for Kp [2 marks

  14. Q05.2

    November 2021 · Paper 1

    4 marks3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    November 2021 Paper 1, question 05.2: A 0.460 mol sample of SO2 is mixed with a 0.250 mol sample of O2 in a sealed container at a constant temperature. When equilibrium is reached at a pressure of 2

  15. Q05.3

    November 2021 · Paper 1

    3 marks3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    November 2021 Paper 1, question 05.3: A different mixture of SO2 and O2 reaches equilibrium at a different temperature. Table 4 shows the partial pressures of the gases at equilibrium. Table 4 Gas P

  16. Q05.4

    November 2021 · Paper 1

    1 mark3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    November 2021 Paper 1, question 05.4: What is the effect on the value of Kp if the pressure of this equilibrium mixture is increased at a constant temperature? 2 SO2(g) + O2(g) ⇌ 2 SO3(g) [1 mark] T

  17. Q09

    November 2021 · Paper 3

    1 mark3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    November 2021 Paper 3, question 09: What is the mole fraction of 1.0 g of a compound of relative molecular mass 100.0 dissolved in 30.0 g of a solvent of relative molecular mass 50.0? [1 mark] A 6

  18. Q06.2

    November 2020 · Paper 1

    4 marks3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    November 2020 Paper 1, question 06.2: A 0.230 mol sample of carbon monoxide is mixed with hydrogen in a 1:2 mol ratio and allowed to reach equilibrium in a sealed flask at temperature T. At equilibr

  19. Q06.3

    November 2020 · Paper 1

    2 marks3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    November 2020 Paper 1, question 06.3: Give an expression for the equilibrium constant (Kp) for this reaction. State the units. [2 marks] Kp Units

  20. Q06.4

    November 2020 · Paper 1

    2 marks3.1.6 Chemical equilibria, Le Chatelier’s principle and Kc3.1.10 Equilibrium constant Kp for homogeneous systems
    The whole paper ↗
    November 2020 Paper 1, question 06.4: Some more carbon monoxide is added to the mixture in Question 06.2. The new mixture is allowed to reach equilibrium at temperature T. State the effect, if any,
All 36 questions on Equilibrium constant Kp for homogeneous systems, as a list
  1. June 2024, Paper 1, Q04.1 (2 marks): A mixture of 2.00 mol of H2O(g) and 2.00 mol of CO(g) is allowed to reach equilibrium at a constant temperature in a 20 dm3 container. At equilibrium, there are
  2. June 2024, Paper 1, Q04.2 (1 mark): State why the equilibrium constant (Kp) for this reaction has no units. [1 mark]
  3. June 2024, Paper 1, Q04.4 (4 marks): Give an expression for Kp for this reaction. Calculate the value of Kp at 6000 kPa State the units. [4 marks] Kp Units
  4. June 2024, Paper 1, Q04.5 (1 mark): State the effect, if any, of an increase in volume of the container on the value of Kp for this reaction at a constant temperature. [1 mark]
  5. June 2023, Paper 1, Q04.1 (3 marks): A 0.317 mol sample of nitrogen dioxide is placed in a sealed flask and heated at a constant temperature until equilibrium is reached. At equilibrium, the flask
  6. June 2023, Paper 1, Q04.2 (1 mark): The total pressure in the flask in Question 04.1 is 120 kPa at equilibrium. Calculate the partial pressure, in kPa, of NO2 If you were unable to answer Question
  7. June 2023, Paper 1, Q04.3 (3 marks): Table 1 shows the mole fractions of the three gases in a different equilibrium mixture. 2 NO2(g) ⇌ 2 NO(g) + O2(g) ΔH = +113 kJ mol–1 Table 1 Gas Mole fraction
  8. June 2023, Paper 1, Q04.4 (2 marks): The equilibrium mixture in Question 04.3 is compressed into a smaller volume. Deduce the effect, if any, of this change on the equilibrium yield of oxygen and o
  9. June 2023, Paper 3, Q28 (1 mark): The equation for the complete combustion of butane is C4H10 + 6 1 2 O2 → 4 CO2 + 5 H2O What is the mole fraction of butane in a mixture of butane and oxygen wit
  10. June 2022, Paper 1, Q01.3 (3 marks): Carbon monoxide and hydrogen react to form methanol. CO(g) + 2 H2(g) ⇌ CH3OH(g) 0.430 mol of carbon monoxide is mixed with 0.860 mol of hydrogen. At equilibrium
  11. June 2022, Paper 1, Q01.4 (1 mark): Give an expression for the equilibrium constant (Kp) for this reaction. CO(g) + 2 H2(g) ⇌ CH3OH(g) [1 mark] Kp
  12. June 2022, Paper 1, Q01.5 (3 marks): A different mixture of carbon monoxide and hydrogen is left to reach equilibrium at a temperature T. Some data for this equilibrium are shown in Table 1. Table
  13. June 2022, Paper 1, Q01.6 (2 marks): Use the Kp value from Table 1 to calculate a value for Kp for the following reaction at temperature T. CH3OH(g) ⇌ CO(g) + 2 H2(g) Give the units for Kp [2 marks
  14. November 2021, Paper 1, Q05.2 (4 marks): A 0.460 mol sample of SO2 is mixed with a 0.250 mol sample of O2 in a sealed container at a constant temperature. When equilibrium is reached at a pressure of 2
  15. November 2021, Paper 1, Q05.3 (3 marks): A different mixture of SO2 and O2 reaches equilibrium at a different temperature. Table 4 shows the partial pressures of the gases at equilibrium. Table 4 Gas P
  16. November 2021, Paper 1, Q05.4 (1 mark): What is the effect on the value of Kp if the pressure of this equilibrium mixture is increased at a constant temperature? 2 SO2(g) + O2(g) ⇌ 2 SO3(g) [1 mark] T
  17. November 2021, Paper 3, Q09 (1 mark): What is the mole fraction of 1.0 g of a compound of relative molecular mass 100.0 dissolved in 30.0 g of a solvent of relative molecular mass 50.0? [1 mark] A 6
  18. November 2020, Paper 1, Q06.2 (4 marks): A 0.230 mol sample of carbon monoxide is mixed with hydrogen in a 1:2 mol ratio and allowed to reach equilibrium in a sealed flask at temperature T. At equilibr
  19. November 2020, Paper 1, Q06.3 (2 marks): Give an expression for the equilibrium constant (Kp) for this reaction. State the units. [2 marks] Kp Units
  20. November 2020, Paper 1, Q06.4 (2 marks): Some more carbon monoxide is added to the mixture in Question 06.2. The new mixture is allowed to reach equilibrium at temperature T. State the effect, if any,
  21. November 2020, Paper 1, Q06.5 (2 marks): State the effect, if any, of the addition of a catalyst on the value of Kp for this equilibrium. Explain your answer. [2 marks] Effect on value of Kp Explanatio
  22. June 2019, Paper 1, Q07.1 (2 marks): A sample of sulfur trioxide was heated and allowed to reach equilibrium at a given temperature. The equilibrium mixture contained 6.08 g of sulfur dioxide. Calc
  23. June 2019, Paper 1, Q07.2 (4 marks): A different mass of sulfur trioxide was heated and allowed to reach equilibrium at 1050 K 2 SO3(g) ⇌ 2 SO2(g) + O2(g) The amounts of each substance in the equil
  24. June 2019, Paper 1, Q07.3 (2 marks): For this reaction at 1050 K the equilibrium constant, Kp = 7.62 x 105 Pa For this reaction at 500 K the equilibrium constant, Kp = 3.94 x 104 Pa Explain how thi
  25. June 2019, Paper 1, Q07.4 (2 marks): Use data from Question 07.3 to calculate the value of Kp, at 500 K, for the equilibrium represented by this equation. Deduce the units of Kp SO3(g) ⇌ SO2(g) + 1
  26. June 2019, Paper 3, Q11 (1 mark): The equation for the reaction between sulfur dioxide and oxygen is shown. 2 SO2(g) + O2(g) ⇌ 2 SO3(g) In an experiment, 2.00 mol of sulfur dioxide are mixed wit
  27. June 2019, Paper 3, Q12 (1 mark): Nitrogen reacts with hydrogen in this exothermic reaction N2(g) + 3 H2(g) ⇌ 2 NH3(g) Which change increases the equilibrium yield of ammonia but has no effect o
  28. June 2018, Paper 1, Q02.1 (3 marks): When equilibrium was reached, the total pressure in the flask was 150 kPa and the mole fraction of NH3(g) in the mixture was 0.80 Calculate the partial pressure
  29. June 2018, Paper 1, Q02.2 (1 mark): Give an expression for the equilibrium constant (Kp) for this reaction. [1 mark] Kp
  30. June 2018, Paper 1, Q02.3 (2 marks): In a different equilibrium mixture, under different conditions, the partial pressures of the gases are shown in Table 2. Table 2 Gas Partial pressure / kPa N2 1
  31. June 2018, Paper 1, Q02.4 (3 marks): The enthalpy change for the reaction is –92 kJ mol–1 State the effect, if any, of an increase in temperature on the value of Kp for this reaction. Justify your
  32. June 2017, Paper 1, Q09.2 (2 marks): The equation shows the final stage in the production of methanol. CO(g) + 2H2(g) ⇌ CH3OH(g) 20.1 mol of carbon monoxide and 24.2 mol of hydrogen were placed in
  33. June 2017, Paper 1, Q09.3 (6 marks): A different mixture of carbon monoxide and hydrogen was allowed to reach equilibrium at 600 K At equilibrium, the mixture contained 2.76 mol of carbon monoxide,
  34. June 2017, Paper 3, Q28 (1 mark): A 385 cm3 sample of carbon dioxide at 100 kPa and 25 °C was mixed with 2.89 × 10−2 mol of argon. The gas constant, R = 8.31 J K−1 mol−1 What is the mole fractio
  35. Specimen, Paper 1, Q04.6 (7 marks): Kp = Units =
  36. Specimen, Paper 3, Q12: Which change would alter the value of the equilibrium constant (Kp) for this reaction? 2SO2(g) + O2(g) 2SO3(g) [1 mar A Increasing the total pressure of the sys

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