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3 Physical chemistry

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  1. (a) Energetics

    1. 3.1Exothermic and endothermic changes

      Know that chemical reactions in which heat energy is given out are described as exothermic, and those in which heat energy is taken in are described as endothermic

    2. 3.2Temperature change practical

      Describe simple calorimetry experiments for reactions such as combustion, displacement, dissolving and neutralisation

    3. 3.3Energy level diagrams

      Calculate the heat energy change from a measured temperature change using the expression Q = mcΔT

    4. 3.4Bond energy calculations

      Calculate the molar enthalpy change (ΔH) from the heat energy change, Q

    5. 3.5CAnd explain energy level diagrams to represent

      Draw and explain energy level diagrams to represent exothermic and endothermic reactions

    6. 3.6CBond-breaking is an endothermic process and

      Know that bond-breaking is an endothermic process and that bond-making is an exothermic process

    7. 3.7CBond energies to calculate the enthalpy change

      Use bond energies to calculate the enthalpy change during a chemical reaction

    8. 3.8Calorimetry practical

      Practical: investigate temperature changes accompanying some of the following types of change: • salts dissolving in water • neutralisation reactions • displacement reactions • combustion reactions.

  2. (b) Rates of reaction

    1. Describe experiments to investigate the effects of changes in surface area of a solid, concentration of a solution, temperature and the use of a catalyst on the rate of a reaction

    2. Describe the effects of changes in surface area of a solid, concentration of a solution, pressure of a gas, temperature and the use of a catalyst on the rate of a reaction

    3. Explain the effects of changes in surface area of a solid, concentration of a solution, pressure of a gas and temperature on the rate of a reaction in terms of particle collision theory

    4. Know that a catalyst is a substance that increases the rate of a reaction, but is chemically unchanged at the end of the reaction

    5. Know that a catalyst works by providing an alternative pathway with lower activation energy

    6. Draw and explain reaction profile diagrams showing ΔH and activation energy

    7. Practical: investigate the effect of changing the surface area of marble chips and of changing the concentration of hydrochloric acid on the rate of reaction between marble chips and dilute hydrochloric acid

    8. Practical: investigate the effect of different solids on the catalytic decomposition of hydrogen peroxide solution

  3. (c) Reversible reactions and equilibria

    1. Know that some reactions are reversible and this is indicated by the symbol ⇌ in equations

    2. Describe reversible reactions such as the dehydration of hydrated copper(II) sulfate and the effect of heat on ammonium chloride

    3. Know that a reversible reaction can reach dynamic equilibrium in a sealed container

    4. Know that the characteristics of a reaction at dynamic equilibrium are: • the forward and reverse reactions occur at the same rate • the concentrations of reactants and products remain constant.

    5. Understand why a catalyst does not affect the position of equilibrium in a reversible reaction

    6. Know the effect of changing either temperature or pressure on the position of equilibrium in a reversible reaction: • an increase (or decrease) in temperature shifts the position of equilibrium in the direction of the endothermic (or exothermic) reaction • an increase (or decrease) in pressure shifts the position of equilibrium in the direction that produces fewer (or more) moles of gas References to Le Chatelier's principle are not required