Lesson 3.1.9.1

3.1.9.1 Rate equations Quiz: AQA Chemistry, Unit 1

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 3.1.9.1, Rate equations: 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 the rate equation Rate = k[A]ᵐ[B]ⁿ, what does the exponent m represent?

    • Stoichiometric coefficient
    • Overall order
    • Rate constant
    • Order of A

  2. Which factor directly changes the value of the rate constant k for a given reaction?

    • Concentration
    • Pressure
    • Surface area
    • Temperature

  3. Which set of values are reactant orders restricted to at A-level Chemistry?

    • 1 and 2 only
    • 0, 1 and 2
    • 1, 2 and 3
    • -1, 0 and 1

  4. A reaction has the rate equation Rate = k[A][B]. What are the units of k when concentrations are in mol dm^-3 and rate in mol dm^-3 s^-1?

    • s^-1
    • dm^3 mol^-1 s^-1
    • mol dm^-3 s^-1
    • mol^-1 dm^3

  5. A first-order reaction has Rate = k[A]. What are the units of k?

    • s^-1
    • dm^3 mol^-1 s^-1
    • dm^6 mol^-2 s^-1
    • mol dm^-3 s^-1

  6. A zero-order reaction has Rate = k. What are the units of k when rate is in mol dm^-3 s^-1?

    • dm^3 mol^-1 s^-1
    • mol dm^-3 s^-1
    • mol^-1 dm^3 s
    • s^-1

  7. For a reaction with Rate = k[A]^2 and k = 0.50 dm^3 mol^-1 s^-1, what is the rate when [A] = 0.20 mol dm^-3?

    • 0.0080 mol dm^-3 s^-1
    • 0.40 mol dm^-3 s^-1
    • 0.020 mol dm^-3 s^-1
    • 0.10 mol dm^-3 s^-1

  8. For Rate = k[A][B]^2 with k = 2.0 dm^6 mol^-2 s^-1, [A] = 0.10 and [B] = 0.20 mol dm^-3, what is the rate?

    • 0.10 mol dm^-3 s^-1
    • 0.040 mol dm^-3 s^-1
    • 0.0080 mol dm^-3 s^-1
    • 0.0040 mol dm^-3 s^-1

  9. How does an increase in temperature affect the rate constant k of a reaction?

    • It becomes zero
    • It increases
    • It decreases
    • It stays constant

  10. Which rearrangement of k = Ae^(-Ea/RT) allows a straight-line graph of experimental data to be plotted?

    • ln k = -Ea/(RT) + ln A
    • k = -Ea/(RT) + A
    • ln k = Ea/(RT) - ln A
    • 1/k = Ea/(RT) + A

  11. The rate constant k is measured at several temperatures. What is the gradient of a graph of ln k against 1/T?

    • Ea/R
    • ln A
    • -Ea/R
    • -R/Ea

  12. For a reaction with k = A e^(-Ea/RT), A = 1.0 x 10^10 s^-1, Ea = 60 kJ/mol and T = 300 K, what is k? Use R = 8.314 J K^-1 mol^-1.

    • About 36 s^-1
    • About 0.036 s^-1
    • About 0.36 s^-1
    • About 3.6 s^-1

  13. What is the gradient of a concentration–time graph for a zero-order reaction?

    • -k
    • +k
    • 1/k
    • Zero

  14. Doubling the concentration of reactant B has no effect on rate. What is the order with respect to B?

    • Second order
    • Half order
    • Zero order
    • First order

  15. The rate equation is Rate = k[A][B]^2. By what factor does the rate increase when [A] is tripled and [B] is doubled?

    • 24
    • 9
    • 12
    • 6

  16. Initial rate data: [A] = 0.10, [B] = 0.10 mol dm^-3 gives rate 2.0 x 10^-3 mol dm^-3 s^-1; [A] = 0.20, [B] = 0.10 gives rate 8.0 x 10^-3. With Rate = k[A]^2, what is k?

    • 0.20 dm^3 mol^-1 s^-1
    • 2.0 dm^3 mol^-1 s^-1
    • 0.020 dm^3 mol^-1 s^-1
    • 0.50 dm^3 mol^-1 s^-1

  17. If Rate = k[A]², how many molecules of A are in the rate-determining step?

    • Two
    • Three
    • Zero
    • One

  18. How must the orders of reaction in a rate equation always be determined?

    • From balanced equations
    • Experimentally
    • From stoichiometry
    • From molar masses

  19. A reaction is first order in A, with Rate = k[A]. If [A] is doubled at constant temperature, what happens to the rate?

    • It is unchanged
    • It doubles
    • It halves
    • It quadruples

  20. For Rate = k[A]², by what factor does the rate change if [A] is halved?

    • One quarter
    • One half
    • Double
    • One eighth

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