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

The 20 questions

1. What does the order of reaction with respect to a reactant represent?

   • Activation energy
   • Power of concentration
   • Rate constant unit
   • Stoichiometric ratio

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. What reaction order produces a horizontal line on a rate-concentration graph?

   • Zero order
   • First order
   • Third order
   • Second order

6. In the rate equation rate = k[X]^0[Y]^2, what is the order with respect to X?

   • First order
   • Second order
   • Third order
   • Zero order

7. What factor changes the value of the rate constant, k, for a given reaction?

   • Temperature
   • Pressure
   • Concentration
   • Surface area

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. Doubling [A] quadruples the rate, while doubling [B] doubles it. What is the order with respect to A?

    • Zero order
    • First order
    • Second order
    • Third order

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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