The value of $Δ H_{t r a n s i t i o n}$ of C (graphite) $\to$ C (diamond) is 1.9 kJ/mol at $25^{o} C$ . Entropy of graphite is higher than entropy of diamond. This implies that

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C (diamond) is more thermodynamically stable than C (graphite) at $25^{o} C$

$Δ G_{t r a n s i t i o n}$ of C (diamond) $\to$ C (graphite) is - ve

Diamond will provide more heat on complete combustion at $25^{o} C$

C (Graphite) is more thermodynamically stable than C (diamond) at $25^{o} C$

answer is B, C, D.

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Detailed Solution

$Δ G = Δ H - T Δ S$

$= 1.9 - 298 (- v e) = + v e$

Graphite is more stable than diamond thermodynamically

Diamond provides more heat on complete combustion in comparison of graphite.

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