Consider the following reaction between zinc and oxygen and choose the correct options out of the options given below:
2Zn(s) + O_{2}(g) \rightarrow 2ZnO(s); \Delta H=-693.8 \; kJ \; mol^{-1}
(i) The enthalpy of two moles ZnO is less than the total enthalpy of two moles of Zn and one mole of oxygen by 693.8 kJ.
(ii) The enthalpy of two moles of ZnO is more than the total enthalpy of two moles of Zn and one mole of oxygen by 693.8 kJ.
(iii) 8 kJ mol -1 energy is evolved in the reaction.
(iv) 693.8 kJ mol-1 energy is absorbed in the reaction.

Answers (1)

The answers is options (i) and (iii).

Explanation:

\Delta _{f}H=\sum _{i}a_{i}\Delta _{f}H-\sum _{i}b_{i}\Delta _{f}H

The reaction depicted above is exothermic in nature, and, hence, the reactant enthalpy is more than the product enthalpy.

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