Lesson 16.1.5

16.1.5 Activation energy from rate data Quiz: Pearson Edexcel Chemistry, Unit 16

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 16.1.5, Activation energy from rate 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 the minimum energy required by colliding particles for a successful chemical reaction?

    • Ionisation energy
    • Activation energy
    • Enthalpy change
    • Lattice energy

  2. How does adding a catalyst increase the rate of a chemical reaction?

    • Lowers enthalpy change
    • Increases activation energy
    • Increases enthalpy change
    • Lowers activation energy

  3. In the Arrhenius equation k = A e^(-Ea/RT), what does the symbol A represent?

    • Rate constant
    • Activation energy
    • Pre-exponential factor
    • Gas constant

  4. A graph of ln k against 1/T is a straight line. What is its gradient?

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

  5. The Arrhenius equation is used with R in J K-1 mol-1 and Ea in J mol-1. What is the unit of Ea/R?

    • kJ mol-1
    • K
    • J mol-1 K
    • mol K J-1

  6. Which rearrangement of the Arrhenius equation gives y = mx + c with y = ln k and x = 1/T?

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

  7. Why does increasing temperature increase the rate constant of a reaction?

    • More successful collisions
    • Lower activation energy
    • Higher activation energy
    • Fewer particle collisions

  8. Two reactions have identical A values and temperatures. Which reaction has the larger rate constant?

    • Higher enthalpy change
    • Lower activation energy
    • Lower temperature
    • Higher activation energy

  9. How does adding a catalyst affect a Maxwell-Boltzmann distribution curve?

    • Flattens the peak
    • Unchanged curve shape
    • Shifts peak right
    • Shifts peak left

  10. A plot of ln k against 1/T has a gradient of -4.8 x 10^3 K. What is the activation energy?

    • 580 kJ mol-1
    • 40 kJ mol-1
    • 4.8 kJ mol-1
    • -40 kJ mol-1

  11. The rate constant doubles when temperature rises from 298 K to 308 K, approximately. Which activation energy best fits?

    • About 53 kJ mol-1
    • About 530 kJ mol-1
    • About 5.3 kJ mol-1
    • About 106 kJ mol-1

  12. A reaction has Ea = 75 kJ mol-1. By what factor does k increase when temperature rises from 298 K to 308 K?

    • About 10
    • About 1.5
    • About 2.7
    • About 5.4

  13. Ea = 50 kJ mol-1. By what factor does k increase when temperature rises from 300 K to 320 K?

    • About 3.5
    • About 10
    • About 7.0
    • About 1.3

  14. A catalyst lowers Ea from 80 kJ mol-1 to 50 kJ mol-1. By what factor does the rate constant increase at 300 K, assuming A is unchanged?

    • About 1.6
    • About 1.7 x 10^3
    • About 30
    • About 1.7 x 10^5

  15. Points on a ln k against 1/T plot are (3.00 x 10^-3 K-1, -10.0) and (2.80 x 10^-3 K-1, -6.0). What is Ea?

    • About 166 kJ mol-1
    • About 20 kJ mol-1
    • About 83 kJ mol-1
    • About 2.0 kJ mol-1

  16. In an Arrhenius plot of ln k against 1/T, how is activation energy calculated from the gradient?

    • gradient / R
    • -gradient / R
    • -gradient × R
    • gradient × R

  17. Why does a graph of ln k against 1/T produce a negative gradient?

    • k decreases with T
    • Ea is negative
    • Ea is positive
    • 1/T increases with T

  18. What is the value of the gas constant R used in the Arrhenius equation?

    • 9.81 m s-2
    • 8.31 J K-1 mol-1
    • 1.38 x 10^-23 J K-1
    • 6.02 x 10^23 mol-1

  19. Ea = 60 kJ mol-1. By what factor does k increase when temperature rises from 300 K to 310 K?

    • About 1.3
    • About 10
    • About 4.5
    • About 2.2

  20. Why does adding a catalyst not change the position of equilibrium?

    • Increases product yield
    • Speeds both directions
    • Lowers reactant energy
    • Only speeds forward

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