The reaction \( \mathrm{NH}_{2} \mathrm{CN}(\mathrm{s})+\frac{3}{2} \mathrm{O}_{2}(\mathrm{~g}) ...

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The reaction \( \mathrm{NH}_{2} \mathrm{CN}(\mathrm{s})+\frac{3}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{N}_{2}(\mathrm{~g})+\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\ell) \) was carried out at \( 300 \mathrm{~K} \) in a bomb calorimeter. The heat released was \( 743 \mathrm{~kJ} \mathrm{~mol}^{-1} \). The value of \( \Delta \mathrm{H}_{300 \mathrm{~K}} \) for this reaction would be :-
(A) \( -740.5 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
(B) \( -741.75 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
(C) \( -743.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
(D) \( -744.25 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
\( \mathrm{W} \)
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