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The value ∆H transition of C (graphite) → C (diamond) is 1.9 kJ/mol at 25℃ entropy of graphite is higher than entropy of diamond. This implies that?

The value ∆H transition of C (graphite) → C (diamond) is 1.9 kJ/mol at 25℃ entropy of graphite is higher than entropy of diamond. This implies that? Correct Answer

C(graphite) → C(diamond) trans ∆H = 1.9 kJ /mole Sgraphite > Sdiamond As, Sgraphite is higher so C (graphite) is more stable. Diamond will provide more heat on complete combustion because it is more stable and have 3–D structure. C diamond → Cgraphite ∆Gtransition = -ve then process is spontaneous.

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