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27 July, 22:26

What is the standard gibbs free energy for the transformation of diamond to graphite at 298 k? cdiamondâcgraphite?

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  1. 28 July, 00:31
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    Considering; graphite; standard enthalpy = 0 and entropy = 5.740; diamond standard enthalpy = 1.897 and entropy = 2.38.

    Using the equation Delta G = Delta H - Temperature (DeltaS)

    Delta H = enthalpy sum of products - enthalpy sum of reactants

    Which will be; 0 - 1.897 = - 1.897 kJ/Mol

    Delta S is the entropy sum; given by

    5.740 - 2.38 = 3.36 J/Mol

    We can convert Delta S from Joules to kilo Joules by dividing by 1000

    we get; 0.00336 kJ/mol

    We are given a temperature in kelvin which suits the calculations ((298 k)

    Therefore; using the equation;

    = - 1.897 - (298 * 0.00336) = - 2.90 kJ

    Thus; the standard gibbs free energy will be; - 2.9 kJ
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