\[ \begin{array}{l} \text { If S }+\mathrm{O}_{2} \rightarrow \math...
0\[
\begin{array}{l}
\text { If S }+\mathrm{O}_{2} \rightarrow \mathrm{SO}_{2} ; \Delta \mathrm{H}=-298.2 \mathrm{~kJ} \mathrm{~mol}^{-1} \\
\mathrm{SO}_{2}+\frac{1}{2} \mathrm{O}_{2} \rightarrow \mathrm{SO}_{3} ; \Delta \mathrm{H}=-98.7 \mathrm{~kJ} \mathrm{~mol}^{-1} \\
\mathrm{SO}_{3}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4} ; \Delta \mathrm{H}=-130.2 \mathrm{~kJ} \mathrm{~mol}^{-1} \\
\mathrm{H}_{2}+\frac{1}{2} \mathrm{O}_{2} \rightarrow \mathrm{H}_{2} \mathrm{O} ; \Delta \mathrm{H}=-287.3 \mathrm{~kJ} \mathrm{~mol}^{-1}
\end{array}
\]
\( \mathrm{P} \)
W
Then the enthalpy of formation of \( \mathrm{H}_{2} \mathrm{SO}_{4} \) at \( 298 \mathrm{~K} \) will be-
(1) \( -814.4 \mathrm{~kJ} \mathrm{~mol}-1 \)
(2) \( -650.3 \mathrm{~kJ} \mathrm{~mol}{ }^{-1} \)
(3) \( -320.5 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
(4) \( -433.5 \mathrm{~kJ} \mathrm{~mol}{ }^{-1} \)
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