Sulphur dioxide required for the manufacture of sulphuric acid is mainly obtained by burning iron pyrites; $F e S_{2} .$ Regarding $F e S_{2}$ the correct statements are

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The oxidation state of sulphur in the anion is – 1

The oxidation state of iron in $F e S_{2}$ is + 2

The structure of the anion in $F e S_{2}$ is analogous to peroxide ion

Similar to peroxide ion, the anion in $F e S_{2}$ can act as good oxidising agent

answer is A, B, C.

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Detailed Solution

$F e S_{2}$ contain $F e^{2 +}$ and $S_{2}^{2 -}$ ion. $S_{2}^{2 -}$ structure is similar to peroxide ion $O_{2}^{2 -} .$ Peroxide ions are easily reduced by a two – electron process to $O^{2 -} .$ The standard reduction potention for hydrogen peroxide in acid is nearly 1.8 V. Unlike the weak O – O bond in peroxide ion, the S – S bond in disulphide is strong and hence cannot be reduced to $S^{2 -}$ by two electron process.