A sulphide ore like ZnS is first roasted into its oxide prior to reduction by carbon because:

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a sulphide ore cannot be reduced to metal at all

no reducing agent is found suitable for reducing a sulphide ore

the Gibb's free energy of formation of most sulphide are greater than that for ${CS}_{2}$ .

a metal oxide is generally less stable than the metal sulphide

answer is C.

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Detailed Solution

Because the Gibbs free energy of production of most sulphides is larger than that of ${CS}_{2}$ , a sulphide ore such as ZnS is first roasted into its oxide before being reduced by carbon.

Most sulphides have Gibb's free energies that are higher than those of ${CS}_{2}$ during their production.

In actuality ${CS}_{2}$ , is an endothermic substance. This indicates that it is not advantageous to reduce a metal sulphide by carbon to produce metal and carbon disulfide.

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