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18 November, 19:21

A reaction has a ΔH value of + 120 kJ and a ΔS value of - 42 J/K. At which of the following temperatures is the reaction spontaneous (meaning ΔG is negative) ?

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  1. 18 November, 21:29
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    the reaction is spontaneous at T > 2900 K

    Explanation:

    ΔG = ΔH - TΔS

    ∴ ΔH = + 120 KJ

    ∴ ΔS = (-42 J/K) * (KJ/1000 J) = - 0.042 KJ/K

    ∴ ΔG < 0 ⇒ the reaction is spontaneous

    ⇒ at T = 2900 K:

    ⇒ ΔG = 120 - (2900) (-0.042) = 120 - 121.8 = - 1.8 KJ < 0
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