48 g of C (diamond) on complete combustion evolves 1584 kJ of heat. The standard heat of formation of gaseous carbon is 725 kJ/mol. The energies required for the process (i)C (graphite) $\rightarrow$ C(gas) (ii)C (diamond) $\rightarrow$ C(gas)are:

Question

Dr. Abubacker · Accepted Answer

(c)
As graphite is thermodynamically more stable than diamond hence, more heat is required to convert graphite to gaseous carbon

Q. 48 g of C (diamond) on complete combustion evolves 1584 kJ of heat. The standard heat of formation of gaseous carbon is 725 kJ/mol. The energies required for the process (i)C (graphite) $\rightarrow$ C(gas) (ii)C (diamond) $\rightarrow$ C(gas)are:

Explanation

Reviewed by Dr. Abubacker

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