7 Chemical Energetics
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Candidates should be able to:
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7.1 Enthalpy changes of reaction, ΔH
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(a) Explain that most chemical reactions are accompanied by enthalpy changes (exothermic or endothermic);
(b) Define enthalpy change of reaction, ΔH, and state the standard conditions;
(c) Define enthalpy change of formation, combustion, hydration, solution, neutralisation, atomisation, bond energy, ionisation energy and electron affinity;
(d) Calculate the heat energy change from experimental measurements using the relationship: heat change, q mc T or q = mc ;
(e) Calculate enthalpy changes from experimental results.
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7.2 Hess’ law
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(a) State Hess’ law, and its use to find enthalpy changes that cannot be determined directly, e.g. an enthalpy change of formation from enthalpy changes of combustion;
(b) Construct energy level diagrams relating the enthalpy to reaction path and activation energy;
(c) Calculate enthalpy changes from energy cycles.
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7.3 Born-Haber cycle
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(a) Define lattice energy for simple ionic crystals in terms of the change from gaseous ions to solid lattice;
(b) Explain qualitatively the effects of ionic charge and ionic radius on the numerical magnitude of lattice energy values;
(c) Construct Born-Haber cycle for the formation of simple ionic crystals.
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7.4 The solubility of solids in liquids
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(a) Construct energy cycles for the formation of aqueous solutions of ionic compounds;
(b) Explain qualitatively the influence on solubility of the relationship between enthalpy change of solution, lattice energy of solid and enthalpy change of hydration or other solvent-solute interaction.
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Thermochemistry.pdf by Mr.Yi on Scribd
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