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Reactivity 1. What drives chemical reactions?

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  1. 1.1 Measuring enthalpy changes

    1. • Chemical reactions transfer energy between system and surroundings • Total energy conserved • Heat vs. temperature

    2. • Endothermic: energy absorbed (T decreases) • Exothermic: energy released (T increases)

    3. • Relative stability determines endo/exothermic nature • Energy profiles • Sketch and interpret labelled energy profiles for endothermic and exothermic reactions

    4. • Heat transferred at constant pressure, standard conditions • Q = mcΔT • ΔH = −Q/n • Calculate enthalpy change from calorimetry data

  2. 1.2 Energy cycles

    1. 1.2.1Bond energies

      • Bond-breaking absorbs energy • Bond-forming releases energy • Calculate enthalpy change from average bond enthalpies

    2. 1.2.2Hess's law

      • Enthalpy change independent of pathway • Apply Hess's law to multistep reaction cycles

  3. 1.3 Energy from fuels

    1. • Reactive metals, non-metals, organic compounds + O₂ • Deduce complete combustion equations for hydrocarbons and alcohols

    2. • Produces CO and C • Deduce incomplete combustion equations for hydrocarbons and alcohols

    3. • Coal, crude oil, natural gas • CO₂ emissions and greenhouse effect • Compare fuels by carbon dioxide released and energy output

    4. • From biological carbon fixation (photosynthesis) • Renewable vs. non-renewable • Consider advantages and disadvantages of biofuels compared with fossil fuels

    5. • Convert chemical energy directly to electrical energy • Half-equations for electrode reactions • Include hydrogen and methanol fuel cells; PEM details are not assessed