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Question

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

A
C(diamond) is more thermodynamically stable than C(graphite) at 25oC
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B
C(graphite) is more thermodynamically stable than C(diamond) at 25oC
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C
diamond will provide more heat on complete combustion at 25oC
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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 25oC
C diamond will provide more heat on complete combustion at 25oC
D ΔGtransition of C(diamond)C(graphite) is ve
ΔHtransition of C(graphite)C(diamond) is 1.9kJ/mol at 25oC so its an endothermic process.
Internal energy of diamond is more than graphite so it has higher combustion energy.
Also, as internal energy of graphite is less than diamond so C(graphite) is more thermodynamically stable than C(diamond) at 25oC.
ΔGtransition of C(diamond)C(graphite) is ve as for this process ΔH is negative and ΔS is positive so ΔG=ΔHTΔS will always negative.

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