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For the following reaction,
\[
\begin{array}{l}
\mathrm{C} \text { (diamond })+\mathrm{O}_{2} \longrightarrow \mathrm{CO}_{2}(\mathrm{~g}) ; \Delta \mathrm{H}=-94.3 \mathrm{kcal} \\
\mathrm{C} \text { (graphite })+\mathrm{O}_{2} \longrightarrow \mathrm{CO}_{2}(\mathrm{~g}) ; \Delta \mathrm{H}=-97.6 \mathrm{kcal}
\end{array}
\]
The heat required to change \( 1 \mathrm{~g} \) of \( \mathrm{C} \) (diamond) \( \longrightarrow \mathrm{C} \) (graphite) is:
(a) \( 1.59 \mathrm{kcal} \)
(b) \( 0.1375 \mathrm{kcal} \)
(c) \( 0.55 \mathrm{kcal} \)
(d) \( 0.275 \mathrm{kcal} \)
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