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17 July, 10:23

If _H = - 60.0kJ and _S = - 0.200kJ/K, the reaction is spontaneous below a certain temperature. Calculate that temperature.

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  1. 17 July, 10:28
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    delta G = delta H - T delta S where T is the Kelvin temperature

    delta G is the change in Gibbs Free Energy and must be negative for a spontaneous reaction. Set delta G = 0 (for equilibrium) and solve for T

    0 = delta H - T delta S

    T delta S = delta H

    T (-0.200kJ/K) = - 60.0kJ

    T (-200J/K) = - 60,000J

    T = 300K

    delta S is negative, so (-T delta S) is positive and G is more positive for higher temperatures

    This reaction is spontaneous for temperatures less than 300K.
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