A student determines the standard enthalpy change, \(\Delta H^\circ\), for the conversion of graphite to diamond:
\[\text{C(s, graphite)} \rightarrow \text{C(s, diamond)}\]
The student is provided with the following standard enthalpies of combustion:
\[\text{C(s, graphite)} + \text{O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} \quad \Delta H^\circ = -393.5 \text{ kJ/mol}_{rxn}\]
\[\text{C(s, diamond)} + \text{O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} \quad \Delta H^\circ = -395.4 \text{ kJ/mol}_{rxn}\]
Based on these data, what is the value of \(\Delta H^\circ\) for the conversion of graphite to diamond?