The following two reactions are known :
\[
\begin{array}{l}
\mathrm...
The following two reactions are known :
\[
\begin{array}{l}
\mathrm{Fe}_{2} \mathrm{O}_{3(\mathrm{~s})}+3 \mathrm{CO}_{(\mathrm{g})} \longrightarrow 2 \mathrm{Fe}_{(\mathrm{s})}+3 \mathrm{CO}_{2(\mathrm{~g})} ; \Delta \mathrm{H}=-26.8 \mathrm{~kJ} \\
\mathrm{FeO}_{(\mathrm{s})}+\mathrm{CO}_{(\mathrm{g})} \longrightarrow \mathrm{Fe}_{(\mathrm{s})}+\mathrm{CO}_{2(\mathrm{~g})} ; \Delta \mathrm{H}=-16.5 \mathrm{~kJ}
\end{array}
\]
- The value of \( \Delta \mathrm{H} \) for the following reaction
\( -\mathrm{Fe}_{2} \mathrm{O}_{3(\mathrm{~s})}+\mathrm{CO}_{(\mathrm{g})} \longrightarrow 2 \mathrm{FeO}_{(\mathrm{s})}+\mathrm{CO}_{2(\mathrm{~g})} \) is
(a) \( +6.2 \mathrm{~kJ} \)
(b) \( +10.3 \mathrm{~kJ} \)
(c) \( -43.3 \mathrm{~kJ} \)
(d) \( -10.3 \mathrm{~kJ} \)
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