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Thermodynamics

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Quiz your students on thermodynamic topics

The topics covered in this Starter for ten activity are: thermodymanic definitions, calorimetry, Hess’s law and using bond enthalpies.

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Starters for 10: Advanced level 1 (16–18)

Level

Use

Category

Specification

Republic of Ireland
- Leaving Certificate
  - Chemistry
    - 5. Fuels and heats of reactions
      - 5.4 Exothermic and Endothermic Reactions
        Activities
        Mandatory experiment 5.1 - Determination of the heat of reaction of hydrochloric acid with sodium hydroxide.
        Depth of treatment
        Heat of reaction (general term).
        Sign of ΔH
        Bond energy (concept only - no calculations except for the illustrative example indicated).
        Hess's law.
England
- GCSE
  - AQA Chemistry
    - 4.5 Energy changes
      - 4.5.1 Exothermic and endothermic reactions
        4.5.1.3 The energy change of reactions (HT only)
        Students should be able to calculate the energy transferred in chemical reactions using bond energies supplied.
- A/AS level
Scotland
- Higher
  - SQA Chemistry
    - 3. Chemistry in society
      - (c) Chemical energy
        The enthalpy change associated with a reaction can be calculated from the quantity of heat energy released.
        The quantity of heat energy released can be determined experimentally and calculated using Eₕ=cmΔT.
        The quantities Eₕ, c, m or ΔT can be calculated, in the correct units, given relevant data.
        The enthalpy of combustion of a substance is the enthalpy change when one mole of the substance burns completely in oxygen.
        Hess’s law states that the enthalpy change for a chemical reaction is independent of the route taken. The enthalpy change for a reaction can be calculated using Hess’s law, given appropriate data.
        The molar bond enthalpy is the energy required to break one mole of bonds in a diatomic molecule. A mean molar bond enthalpy is the average energy required to break one mole of bonds, for a bond that occurs in a number of compounds.
        Bond enthalpies can be used to estimate the enthalpy change occurring for a gas phase reaction, by calculating the energy required to break bonds in the reactants and the energy released when new bonds are formed in the products.
Wales
- A/AS level
  - WJEC Chemistry
    - Unit 2: ENERGY, RATE AND CHEMISTRY OF CARBON COMPOUNDS
      - 2.1 Thermochemistry
        (a) enthalpy change of reaction, enthalpy change of combustion and standard molar enthalpy change of formation, ΔfHᵒ
        (b) Hess’s law and energy cycles
        (c) concept of average bond enthalpies and how they are used to carry out simple calculations
        (d) how to calculate enthalpy changes
        (e) simple procedures to determine enthalpy changes
Northern Ireland
- GCSE
  - CCEA Chemistry
    - Unit 2: Further Chemical Reactions, Rates and Equilibrium, Calculations and Organic Chemistry
      - 2.8 Energy changes in chemistry
        2.8.5 calculate energy changes in a chemical reaction from bond energies by considering bond making and bond breaking energies.
  - CCEA Double award science
    - Unit C2: Further Chemical Reactions, Rates and Equilibrium, Calculations and Organic Chemistry
      - 2.8 Energy changes in chemistry
        2.8.5 calculate energy changes in a chemical reaction from bond energies by considering bond making and bond breaking energies.
- A/AS level
  - CCEA Chemistry
    - Unit AS 2: Further Physical and inorganic Chemistry and an Introdution to Organic Chemistry
      - 2.8 Energetics
        2.8.3 define the term standard enthalpy change, ΔHӨ;
        2.8.5 define the standard enthalpy of combustion, formation and neutralisation, namely ΔcHӨ, ΔfHӨ and ΔnHӨ;
        2.8.6 recall experimental methods to determine enthalpy changes;
        2.8.10 calculate enthalpy changes indirectly using Hess’s Law;
        2.8.11 define the term average bond enthalpy and calculate the enthalpy change of a reaction using average bond enthalpies;

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