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Simple rate equations, orders of reaction and rate constants: CAIE A‑Level Chemistry questions

Every CAIE A-Level Chemistry exam question on 26.1 Simple rate equations, orders of reaction and rate constants, June 2024 and the specimen papers, with its mark scheme and examiner’s report.

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312 questions

  1. Q5(a)(i)

    June 2024 · Paper 4

    1 mark26.1 Simple rate equations, orders of reaction and rate constants
    The whole paper ↗
    June 2024 Paper 4, question 5(a)(i): Use Fig. 5.1 to determine the initial rate of reaction 1. Show your working. rate = mol dm–3 min–1 [1]

  2. Q5(a)(ii)

    June 2024 · Paper 4

    1 mark26.1 Simple rate equations, orders of reaction and rate constants
    The whole paper ↗
    June 2024 Paper 4, question 5(a)(ii): The rate equation for reaction 1 is rate = k [S2O8 2–] [I–]. Suggest why a large excess of iodide ions allows the rate constant to be determined from the half-l

  3. Q5(c)

    June 2024 · Paper 4

    1 mark26.1 Simple rate equations, orders of reaction and rate constants
    The whole paper ↗
    June 2024 Paper 4, question 5(c): Describe the effect of an increase in temperature on the rate constant and the rate of reaction 1. [1]

  4. Q5(d)

    June 2024 · Paper 4

    1 mark26.1 Simple rate equations, orders of reaction and rate constants
    The whole paper ↗
    June 2024 Paper 4, question 5(d): In aqueous solution, thiosulfate ions, S2O3 2–, react with hydrogen ions, as shown in reaction 2. reaction 2 S2O3 2– + 2H+ SO2 + S + H2O The rate of reaction is

  5. Q5(e)

    June 2024 · Paper 4

    2 marks26.1 Simple rate equations, orders of reaction and rate constants
    The whole paper ↗
    June 2024 Paper 4, question 5(e): The compound nitrosyl bromide, NOBr, can be formed as shown in reaction 3. reaction 3 2NO(g) + Br2(g) 2NOBr(g) The rate is first order with respect to [NO] and

  6. Q3(a)(i)

    Specimen · Paper 4

    1 mark26.1 Simple rate equations, orders of reaction and rate constants
    The whole paper ↗
    Specimen Paper 4, question 3(a)(i): Explain what is meant by order of reaction with respect to a particular reagent. [1]

  7. Q3(a)(ii)

    Specimen · Paper 4

    2 marks26.1 Simple rate equations, orders of reaction and rate constants
    The whole paper ↗
    Specimen Paper 4, question 3(a)(ii): Use the results of experiment 1 to calculate the rate constant, k, for this reaction. Include the units of k. k = units [2]

  8. Q3(a)(iii)

    Specimen · Paper 4

    1 mark26.1 Simple rate equations, orders of reaction and rate constants
    The whole paper ↗
    Specimen Paper 4, question 3(a)(iii): Use the data in Table 3.1 to calculate the initial rate in experiment 2. initial rate = mol dm–3 s–1 [1]

  9. Q3(a)(iv)

    Specimen · Paper 4

    1 mark26.1 Simple rate equations, orders of reaction and rate constants
    The whole paper ↗
    Specimen Paper 4, question 3(a)(iv): Use the data in Table 3.1 to calculate [Cl O2] in experiment 3. [Cl O2] = mol dm–3 [1]

  10. Q3(b)(i)

    Specimen · Paper 4

    1 mark26.1 Simple rate equations, orders of reaction and rate constants
    The whole paper ↗
    Specimen Paper 4, question 3(b)(i): Explain what is meant by rate-determining step. [1]

  11. Q3(b)(ii)

    Specimen · Paper 4

    1 mark26.1 Simple rate equations, orders of reaction and rate constants
    The whole paper ↗
    Specimen Paper 4, question 3(b)(ii): The mechanism of the reaction between Cl O2 and F2 has two steps. Suggest equations for the two steps of this mechanism. step 1 step 2 [1]

  12. Q3(b)(iii)

    Specimen · Paper 4

    1 mark26.1 Simple rate equations, orders of reaction and rate constants
    The whole paper ↗
    Specimen Paper 4, question 3(b)(iii): State and explain which of the two steps is the rate-determining step. rate-determining step = [1]

  13. Q3(c)

    Specimen · Paper 4

    1 mark26.1 Simple rate equations, orders of reaction and rate constants
    The whole paper ↗
    Specimen Paper 4, question 3(c): Describe the effect of temperature change on the rate of a reaction and the rate constant. [1] [Total: 9]
All 13 questions on Simple rate equations, orders of reaction and rate constants, as a list
  1. June 2024, Paper 4, Q5(a)(i) (1 mark): Use Fig. 5.1 to determine the initial rate of reaction 1. Show your working. rate = mol dm–3 min–1 [1]
  2. June 2024, Paper 4, Q5(a)(ii) (1 mark): The rate equation for reaction 1 is rate = k [S2O8 2–] [I–]. Suggest why a large excess of iodide ions allows the rate constant to be determined from the half-l
  3. June 2024, Paper 4, Q5(c) (1 mark): Describe the effect of an increase in temperature on the rate constant and the rate of reaction 1. [1]
  4. June 2024, Paper 4, Q5(d) (1 mark): In aqueous solution, thiosulfate ions, S2O3 2–, react with hydrogen ions, as shown in reaction 2. reaction 2 S2O3 2– + 2H+ SO2 + S + H2O The rate of reaction is
  5. June 2024, Paper 4, Q5(e) (2 marks): The compound nitrosyl bromide, NOBr, can be formed as shown in reaction 3. reaction 3 2NO(g) + Br2(g) 2NOBr(g) The rate is first order with respect to [NO] and
  6. Specimen, Paper 4, Q3(a)(i) (1 mark): Explain what is meant by order of reaction with respect to a particular reagent. [1]
  7. Specimen, Paper 4, Q3(a)(ii) (2 marks): Use the results of experiment 1 to calculate the rate constant, k, for this reaction. Include the units of k. k = units [2]
  8. Specimen, Paper 4, Q3(a)(iii) (1 mark): Use the data in Table 3.1 to calculate the initial rate in experiment 2. initial rate = mol dm–3 s–1 [1]
  9. Specimen, Paper 4, Q3(a)(iv) (1 mark): Use the data in Table 3.1 to calculate [Cl O2] in experiment 3. [Cl O2] = mol dm–3 [1]
  10. Specimen, Paper 4, Q3(b)(i) (1 mark): Explain what is meant by rate-determining step. [1]
  11. Specimen, Paper 4, Q3(b)(ii) (1 mark): The mechanism of the reaction between Cl O2 and F2 has two steps. Suggest equations for the two steps of this mechanism. step 1 step 2 [1]
  12. Specimen, Paper 4, Q3(b)(iii) (1 mark): State and explain which of the two steps is the rate-determining step. rate-determining step = [1]
  13. Specimen, Paper 4, Q3(c) (1 mark): Describe the effect of temperature change on the rate of a reaction and the rate constant. [1] [Total: 9]

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