Lesson 16.1.3

16.1.3 Determining orders from experimental data Quiz: Pearson Edexcel Chemistry, Unit 16

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 16.1.3, Determining orders from experimental data: 20 multiple choice questions for the Pearson Edexcel Chemistry (9CH0), Unit 16: Kinetics II, written with Revision Ninja.

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The 20 questions

  1. What is meant by the order of reaction with respect to a reactant?

    • The time taken for that reactant's concentration to halve
    • The number of moles of that reactant shown in the balanced equation
    • The energy the reactant must absorb before any reaction can occur
    • The power to which that reactant's concentration is raised in the rate equation

  2. What is the overall order of a reaction with rate = k[A]^2[B]?

    • 2
    • 1
    • 3
    • 5

  3. What are the units of the rate constant for an overall second-order reaction, if rate is in mol dm-3 s-1 and concentrations are in mol dm-3?

    • dm3 mol-1 s-1
    • mol dm-3 s-1
    • dm6 mol-2 s-1
    • s-1

  4. Which rate equation describes a reaction that is first order in A and zero order in B?

    • rate = k[B]
    • rate = k[A]
    • rate = k[A][B]
    • rate = k[A]^2

  5. A horizontal straight line on a rate-concentration graph shows what about the reactant?

    • The reaction is first order with respect to that reactant
    • The reaction is zero order with respect to that reactant
    • The reaction has no catalyst present in the mixture
    • The reaction is second order with respect to that reactant

  6. A rate equation is rate = k[X]^0[Y]^2. Which statement is correct?

    • The reaction is second order in X and zero order in Y
    • The reaction is zero order in X and second order in Y
    • The rate constant has no units in this equation
    • The reaction is first order in both X and Y

  7. Which statement about the rate constant k is correct?

    • k is the number of collisions per second between reactant molecules
    • k is always equal to the rate of reaction at 1 mol dm-3 concentrations for any reaction
    • k changes as the reactant concentrations change during the reaction
    • k is constant for a given reaction at a fixed temperature and changes only when the temperature changes

  8. Initial rates: 0.10 mol dm-3 of A gives 2.0 x 10^-4 mol dm-3 s-1, and 0.20 mol dm-3 of A gives 8.0 x 10^-4 mol dm-3 s-1. What is the order with respect to A?

    • 3
    • 0
    • 1
    • 2

  9. When [B] is tripled with [A] held constant, the rate triples. What is the order with respect to B?

    • 3
    • 1
    • 0
    • 2

  10. When [C] is doubled and the rate is unchanged, what is the order with respect to C?

    • 1/2
    • 0
    • 2
    • 1

  11. Data: [X] = 0.10, [Y] = 0.10 gives rate 1.5 x 10^-3; [X] = 0.20, [Y] = 0.10 gives 3.0 x 10^-3; [X] = 0.10, [Y] = 0.30 gives 4.5 x 10^-3. Which rate equation fits?

    • rate = k[X][Y]^2
    • rate = k[X][Y]
    • rate = k[X]^2[Y]
    • rate = k[Y]

  12. Using the data in the previous set, what is the rate constant k for rate = k[X][Y]?

    • 1.5 dm3 mol-1 s-1
    • 0.015 dm3 mol-1 s-1
    • 0.15 dm3 mol-1 s-1
    • 0.15 mol dm-3 s-1

  13. For rate = k[A]^2 with k = 0.040 dm3 mol-1 s-1 and [A] = 0.20 mol dm-3, what is the rate?

    • 2.0 x 10^-1 mol dm-3 s-1
    • 8.0 x 10^-3 mol dm-3 s-1
    • 1.6 x 10^-3 mol dm-3 s-1
    • 4.0 x 10^-4 mol dm-3 s-1

  14. For rate = k[A][B], a rate of 3.0 x 10^-4 mol dm-3 s-1 occurs at [A] = 0.10 and [B] = 0.30 mol dm-3. What is k?

    • 0.0010 dm3 mol-1 s-1
    • 1.0 dm3 mol-1 s-1
    • 0.10 dm3 mol-1 s-1
    • 0.010 dm3 mol-1 s-1

  15. A rate equation is rate = k[A]^2. What happens to the rate if [A] is multiplied by 5?

    • It increases 5 times
    • It increases 10 times
    • It increases 2 times
    • It increases 25 times

  16. Doubling [A] quadruples the rate and tripling [B] has no effect. If the original rate is R, what is the rate when [A] is halved and [B] doubled?

    • R/4
    • R/2
    • R/8
    • 2R

  17. Initial rate data show that doubling [A] gives four times the rate and doubling [B] gives twice the rate. A student proposes rate = k[A][B]. Which evaluation is best?

    • The proposal is correct because doubling both concentrations gives eight times the rate
    • The proposal is wrong because the order with respect to A is 2, so the equation should be rate = k[A]^2[B]
    • The proposal is correct because the overall order must equal the sum of the two orders
    • The proposal is wrong because a reaction with two reactants cannot have a first-order rate equation

  18. Doubling [A] doubles the rate, and tripling [B] gives nine times the rate. Which rate equation fits?

    • rate = k[A][B]^2
    • rate = k[A][B]
    • rate = k[A]^2[B]
    • rate = k[A]^2[B]^2

  19. A rate constant is 0.20 dm3 mol-1 s-1 for rate = k[A][B]. If [A] = 0.50 and [B] = 0.10 mol dm-3 initially, what is the rate when [A] = 1.00 and [B] = 0.20 mol dm-3?

    • 0.020 mol dm-3 s-1
    • 0.0040 mol dm-3 s-1
    • 0.040 mol dm-3 s-1
    • 0.10 mol dm-3 s-1

  20. A rate equation has k = 2.0 x 10^-3 and rate = k[A]^2[B]. Which expression gives the rate in mol dm-3 s-1 with concentrations in mol dm-3?

    • Rate = 2.0 x 10^-3 [A]^2[B] mol dm-3 s-1
    • Rate = 2.0 x 10^-3 [A]^2[B] s-1
    • Rate = 2.0 x 10^-3 [A]^2 mol dm-3 s-1
    • Rate = 2.0 x 10^-3 [A][B]^2 mol dm-3 s-1

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