Consider the following reaction between zine and oxygen and choose the correct options out of the options given below :

$2\mathrm{Zn}\left(s\right)+{\mathrm{O}}_2\left(g\right)⟶2\mathrm{ZnO}\left(s\right);\mathrm{\Delta }H=-693.8\mathrm{kJ}{\mathrm{mol}}^{-1}$

The enthalpy of two moles of $\mathrm{ZnO}$ is less than the total enthalpy of two moles of Zn and one mole of oxygen by 693.8 kJ.

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, 693.8 kJ.

$693.8\mathrm{kJ}{\mathrm{mol}}^{-1}$ energy is evolved in the reaction.

$693.8\mathrm{kJ}{\mathrm{mol}}^{-1}$ energy is absorbed in the reaction