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Consider the reaction between zinc and oxygen to form corresponding oxide and choose the correct answers out of the options given thereafter.
\[
2 \mathrm{Zn}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{ZnO}(s)
\]
\( \Delta \mathrm{H}=-694.0 \mathrm{~kJ} \mathrm{~mol}^{-1} . \)
(A) The enthalpy of two moles of \( \mathrm{ZnO} \) is less than the total enthalpy of two moles of \( \mathrm{Zn} \) and one mole of oxygen by \( 694.0 \mathrm{~kJ} \).
(B) The enthalpy of two moles of \( \mathrm{ZnO} \) is more than the total enthalpy of two moles of Zn and one mole of oxygen by \( 694.0 \mathrm{~kJ} \).
(C) \( 694.0 \mathrm{k.J} \mathrm{mol}^{-1} \) of energy is evolved in the reaction.
(D) \( 694.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \) of energy is absorbed in the reaction.
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