Consider the ${ΔG}_{f}^{\circ}$ and ${ΔH}_{f}^{\circ} (kJ / mol)$ for the following oxides. Which oxide can be most easily decomposed to form the metal and oxygen gas?

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$\begin{array}{l} HgO ({ΔG}^{\circ} = - 58 .5, {ΔH}^{\circ} = - 90 .8) \end{array}$

$PbO ({ΔG}^{\circ} = - 187 .9, {ΔH}^{\circ} = - 217 .3)$

$\begin{array}{l} {Cu}_{2} O ({ΔG}^{\circ} = - 146 .0, {ΔH}^{\circ} = - 168 .8) \end{array}$

$\begin{array}{lll} ZnO ({ΔG}^{\circ} = - 318 .4, {ΔH}^{\circ} = - 348 .3) \end{array}$

answer is C.

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Detailed Solution

$HgO ⟶ Hg + \frac{1}{2} O_{2}$

$\begin{aligned} {ΔG}^{\circ} = + 58 .5 \\ {ΔH}^{\circ} = + 90 .8 \end{aligned}$

Hence, $HgO$ decomposes more easily at a lower temperature than other oxides.

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