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3 January, 15:54

What is the ΔG under standard temperature for the following reaction between? NH3 (s) → NH3 (l) Given: NH3 (s) : ΔHf = - 46.11 kJ; ΔSf=192.45 J/K NH3 (l) : ΔHf = - 80.29 kJ; ΔSf=111.3 J/K

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  1. 3 January, 17:34
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    We are given the reaction:

    NH3 (s) → NH3 (l)

    NH3 (s) : ΔHf = - 46.11 kJ; ΔSf=192.45 J/K

    NH3 (l) : ΔHf = - 80.29 kJ; ΔSf=111.3 J/K

    The formula of the Gibbs' Free Energy ΔG is

    ΔG = ΔHf - TΔS

    Assume T = 25 degrees C

    For NH3 (s):

    ΔG = - 46.11 kJ * 1000 - (192.45 J/K*298K)

    ΔG = - 103.460 kJ

    For NH3 (l)

    ΔG = - 80.29 kJ * 1000 - (111.3 J/K*298K)

    ΔG = - 113.457 kJ

    Therefore the ΔG under standard temperature for the reaction is the difference between the products - reactants. Solve for this.
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