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Question

The value of ΔHtransition of C(graphite)C(diamond) is 1.9kJ/mol at 25C. Entropy of graphite is higher than entropy of diamond. This implies that:

A
C(diamond) is more thermodynamically stable than C(graphite) at 25C
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B
C(graphite) is more thermodynamically stable than C(diamond) at 25C
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C
Diamond will provide more heat on complete combustion at 25C
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D
ΔGtransition of C(diamond)C(graphite) is ve
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Solution

The correct options are
B C(graphite) is more thermodynamically stable than C(diamond) at 25C
C Diamond will provide more heat on complete combustion at 25C
D ΔGtransition of C(diamond)C(graphite) is ve
C (graphite) is more thermodynamically stable than C (graphite).
For the reverse process, ΔH<0, Also ΔSchanges very negligible due to this transition.
Hence, ΔG is <0 for the transition from C(diamond) to C (graphite)
More heat is evolved due to combustion of less stable form.
Hence, options B, C, D are the appropriate answers.

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