Assertion: Graphite is thermodynamically more stable than dimond.
Reason: `C_(D) to C_(G), DeltaH=-19 kJ mol^(-1)`.

Although graphite is thermodynamically most stable allotrope of Carbon but it has more entropy than diamond Because:

Although graphite is thermodynamically most stable allotrope of Carbon but it has more entropy than diamond Because:

Thermodynamically the most stable form of carbon is (a) diamond , (b) graphite (c) fullerenes , (d) coal

Thermodynamically the most stable form of carbon is (a) diamond , (b) graphite (c) fullerenes , (d) coal

Thermodynamically graphite is more stable than diamond but diamond does not transform into graphite on its own. Why?

Using the data provided, calculate the multiple bond energy ( kJ "mol"^(-1) ) of a C equiv C bond in C_(2)H_(2) .That energy is (take the bond enrgy of a C-H bond as 350 kJ "mol"^(-1) ): 2C(s) + H_(2)(g) to C_(2)H_(2)(g), DeltaH = 225 kJ "mol"^(-1) 2C(s) to 2C(g), DeltaH = 1410 kJ "mol"^(-1) H_(2)(g) to 2H(g), DeltaH = 330 kJ "mol"^(-1)

For the transition C_("(diamond)") rarr C_("(graphite)"), DeltaH=-1.5 kJ . It follows that

For the transition C_("(diamond)") rarr C_("(graphite)"), DeltaH=-1.5 kJ . It follows that