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AQA GCSE Chemistry — Energy, Rates and Equilibrium flashcards

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Topics 4.5 and 4.6 of AQA GCSE Chemistry: exothermic and endothermic reactions, reaction profiles and bond energies, cells and fuel cells, rates and collision theory, catalysts, reversible reactions and Le Chatelier's principle. Higher Tier and Chemistry-only cards are marked.

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Learn deck · part of AQA GCSE Chemistry · written against: AQA GCSE Chemistry (8462) specification, version 1.2, 16 January 2026; Higher Tier and separate-science-only cards marked on the front. Updated 2026-10-10.

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  1. In an exothermic reaction, what happens to the temperature of the surroundings, and why?
    It rises, because the reaction transfers energy to the surroundings.
    Energy Changes › Exothermic and Endothermic Reactions
  2. Name three types of reaction that are exothermic.
    Combustion, many oxidation reactions and neutralisation.
    Energy Changes › Exothermic and Endothermic Reactions
  3. Give two examples of endothermic reactions.
    Thermal decomposition (for example of calcium carbonate) and the reaction of citric acid with sodium hydrogencarbonate.
    Energy Changes › Exothermic and Endothermic Reactions
  4. A hand warmer and a sports injury cold pack both work by chemical reactions. Which type of reaction does each use?
    The hand warmer uses an exothermic reaction; the cold pack uses an endothermic reaction.
    Energy Changes › Exothermic and Endothermic Reactions
  5. In an exothermic reaction, how does the energy stored in the products compare with that of the reactants?
    The products have less stored energy than the reactants; the gap equals the energy given out to the surroundings.

    Why: energy is conserved, so the energy released must come from the chemicals.
    Energy Changes › Exothermic and Endothermic Reactions
  6. How is the mean rate of a reaction calculated?
    Mean rate = quantity of reactant used (or product formed) ÷ time taken, in units such as g/s or cm³/s.
    Rate and Extent of Chemical Change › Rate of Reaction
  7. A reaction gives 60 cm³ of gas in 2 minutes. What is the mean rate in cm³/s?
    0.50 cm³/s

    60 cm³ ÷ 120 s.

    Watch out: convert minutes to seconds first.
    Rate and Extent of Chemical Change › Rate of Reaction
  8. A piece of magnesium loses 0.12 g in 40 s as it reacts with acid. What is the mean rate of reaction?
    0.0030 g/s

    0.12 g ÷ 40 s.
    Rate and Extent of Chemical Change › Rate of Reaction
  9. 0.024 g of magnesium reacts completely in 50 s. What is the mean rate of reaction in mol/s (Mg = 24)? (Higher Tier)
    2.0 × 10⁻⁵ mol/s

    0.024 ÷ 24 = 0.0010 mol, and 0.0010 ÷ 50 = 2.0 × 10⁻⁵ mol/s.
    Rate and Extent of Chemical Change › Rate of Reaction
  10. On a graph of volume of gas against time, how do you find the rate at one particular time?
    Draw a tangent to the curve at that time; the gradient (slope) of the tangent is the rate at that moment.
    Rate and Extent of Chemical Change › Rate of Reaction

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About these cards

Review status: Second-reader reviewed, with corrections applied.

Checked against:

  • Topic outline follows the AQA GCSE Chemistry (8462) specification, version 1.2 (16 January 2026) (outline only; no specification text reproduced).
  • OpenStax Chemistry 2e, consulted as a reference; no text copied.
  • Checked against US Department of Energy, Hydrogen Production: Natural Gas Reforming (public domain) (reference only).

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