Lesson 3.1.5a

3.1.5a Kinetics Quiz: AQA Chemistry, Unit 1

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 3.1.5a, Kinetics: 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. What parameter of a chemical reaction does kinetics directly study?

    • Equilibrium position
    • Enthalpy change
    • Reaction rate
    • Theoretical yield

  2. Which intrinsic factor of reactants strongly affects the rate of a chemical reaction?

    • Chemical reactivity
    • Empirical formula
    • Standard enthalpy
    • Molar mass

  3. What is defined as the change in reactant concentration per unit time?

    • Reaction rate
    • Equilibrium constant
    • Order of reaction
    • Activation energy

  4. Increasing which variable will increase the rate of a chemical reaction?

    • Product yield
    • Activation energy
    • Container volume
    • Temperature

  5. Which change to conditions causes the rate of a reaction to decrease?

    • Adding a catalyst
    • Increasing pressure
    • Lowering temperature
    • Increasing concentration

  6. Which unit is commonly used for the rate of a reaction measured by concentration?

    • dm3 K-1
    • g mol-1
    • mol dm-3 K
    • mol dm-3 s-1

  7. Compared to a slow reaction, a faster reaction takes how much time to complete?

    • Less time
    • More time
    • Equal time
    • Infinite time

  8. The concentration of a reactant falls from 0.80 mol dm-3 to 0.40 mol dm-3 in 40 s. What is the average rate?

    • 0.0200 mol dm-3 s-1
    • 0.400 mol dm-3 s-1
    • 0.0100 mol dm-3 s-1
    • 0.00500 mol dm-3 s-1

  9. A gas is produced with a mass of 0.24 g in 60 s. What is the average rate of production?

    • 0.24 g s-1
    • 0.0040 mol s-1
    • 60 g s-1
    • 0.004 g s-1

  10. A reaction collects 36 cm3 of gas in 30 s. What is the average rate?

    • 36 cm3 s-1
    • 1080 cm3 s-1
    • 1.2 cm3 s-1
    • 0.83 cm3 s-1

  11. What does a steeper gradient on a mass against time graph represent?

    • Lower yield
    • Higher activation energy
    • Faster rate
    • Slower rate

  12. How is the initial rate calculated from a concentration-time graph?

    • Area under curve
    • Half-life measurement
    • Tangent at start
    • Final concentration value

  13. A reaction takes 50 s. If the rate doubles, roughly how long does the reaction take?

    • 25 s
    • 12.5 s
    • 100 s
    • 50 s

  14. A reaction gives 0.50 mol of product in 25 s. What is the average rate?

    • 0.5 mol s-1
    • 0.02 mol s-1
    • 0.0500 mol s-1
    • 12.5 mol s-1

  15. What is measured per unit time to calculate reaction rate?

    • Change in enthalpy
    • Equilibrium constant
    • Change in concentration
    • Activation energy

  16. Why does reaction rate decrease as a reaction proceeds?

    • Activation energy increases
    • Catalyst is consumed
    • Temperature decreases
    • Reactant concentration falls

  17. The concentration of a reactant falls from 0.50 to 0.20 mol dm-3 in 100 s. What is the average rate?

    • 0.0015 mol dm-3 s-1
    • 0.300 mol dm-3 s-1
    • 0.0030 mol dm-3 s-1
    • 0.0070 mol dm-3 s-1

  18. Why is initial rate preferred when investigating reaction kinetics?

    • Maximum reaction speed
    • Known starting concentrations
    • Constant temperature
    • Zero activation energy

  19. The mass of a flask falls from 2.00 g to 1.20 g in 40 s as gas escapes. What is the average rate?

    • 0.0200 g s-1
    • 0.800 g s-1
    • 0.0800 g s-1
    • 0.0120 g s-1

  20. The rate at condition A is 0.40 mol dm-3 s-1 and the rate at condition B is 0.10 mol dm-3 s-1. How many times faster is A than B?

    • Two times faster
    • Four times faster
    • Ten times faster
    • The same speed

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