Consider the following reaction at 1000° C :

(a)  $\mathrm{Zn}\left(s\right)+\frac{1}{2}{\mathrm{O}}_2\left(g\right)⟶\mathrm{ZnO}\left(s\right);\mathrm{\Delta }{G}^{\circ }=-360\mathrm{kJmol}{\mathrm{mol}}^{-1}$

(b) $\mathrm{C}\left(s\right)+\frac{1}{2}{\mathrm{O}}_2\left(g\right)⟶\mathrm{CO}\left(g\right);\mathrm{\Delta }{G}^{\circ }=-460{\mathrm{kJmol}}^{-1}$

Choose the correct statement at 1000° C.

Zinc oxide can be reduced by C.

$\mathrm{ZnO}+\mathrm{C}⟶\mathrm{Zn}+\mathrm{CO}$

 $\mathrm{\Delta }{G}_{{\mathrm{Rx}}^n}^{\circ }=-460+360<0$(spontaneous)

The formation of $\mathrm{CO}$ is more thermodynamically favourable at ${1000}^{°} \mathrm{C}$, as may be observed from reactions.
So at this temperature, C can be reduced in zinc oxide.