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Consider the following reaction between zinc and oxygen and choose the correct options out of the options given below:
\( P \)
\[
2 \mathrm{Zn}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{ZnO}(\mathrm{s}) \quad ; \quad \Delta \mathrm{H}=-693.8 \mathrm{~kJ} \mathrm{~mol}^{-1}
\]
(A) The enthalpyof two moles of \( \mathrm{ZnO} \) is less than the total enthalpyof two moles of \( \mathrm{Zn} \) and one mole of
W. oxygen by \( 693.8 \mathrm{~kJ} \).
(B) The enthalpyof two moles of \( \mathrm{ZnO} \) is more than the total enthalpyof two moles of \( \mathrm{Zn} \) and one mole
- of oxygen by \( 693.8 \mathrm{~kJ} \).
(C) \( 693.8 \mathrm{~kJ} \mathrm{~mol}^{-1} \) energy is evolved in the reaction.
(D) \( 693.8 \mathrm{~kJ} \mathrm{~mol}^{-1} \) energy is absorbed in the reaction.
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