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OpenStudy (abmon98):
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.
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OpenStudy (abmon98):
Diamond has greater energy than graphite because reaction is endothermic so it will require less energy to transform into gaseous state.
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