For a phase change, H0 = 2 kJ/mol and A S0 = 0.017 kJ/(K•mol). What are AG and the spontaneity of the phase change at 500 K?

Question

For a phase change, H0 = 2 kJ/mol and A S0 = 0.017 kJ/(K•mol). What are
AG and the spontaneity of the phase change at 500 K?

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Delwyn 6 months 2021-07-17T08:29:56+00:00 1 Answers 20 views 0

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    2021-07-17T08:31:04+00:00

    Answer:

    ΔG = -6.5kJ/mol at 500K

    Explanation:

    We can find ΔG of a reaction using ΔH, ΔS and absolute temperature with the equation:

    ΔG = ΔH – TΔS

    Computing the values in the problem:

    ΔG = ?

    ΔH = 2kJ/mol

    T = 500K

    And ΔS = 0.017kJ/(K•mol)

    Replacing:

    ΔG = 2kJ/mol – 500K*0.017kJ/(K•mol)

    ΔG = 2kJ/mol – 8.5kJ/mol

    ΔG = -6.5kJ/mol at 500K

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Giải phương trình 1 ẩn: x + 2 - 2(x + 1) = -x . Hỏi x = ? ( )