The conversion of graphite into diamond is an endothermic reaction (∆H = +3 kJ mol–1).
C(graphite) → C(diamond)
Which statements are correct?
1 The enthalpy change of atomisation of diamond is smaller than that of graphite.
2 The bond energy of the C–C bonds in graphite is greater than that in diamond.
3 The enthalpy change of combustion of diamond is greater than that of graphite.

Question

The conversion of graphite into diamond is an endothermic reaction (∆H = +3 kJ mol–1).
C(graphite) → C(diamond)
Which statements are correct?
1 The enthalpy change of atomisation of diamond is smaller than that of graphite.
2 The bond energy of the C–C bonds in graphite is greater than that in diamond.
3 The enthalpy change of combustion of diamond is greater than that of graphite.

abmon98 · Answer

Diamond has greater energy than graphite because reaction is endothermic so it will require less energy to transform into gaseous state.