One mole of sulphur monochloride S2Cl2 loses six moles of electrons to form a compound of sulphur. Oxidation state of sulphur in the product is (Assume chlorine atoms doesn’t show any change in oxidation state and both sulphur atoms appear in the product)

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One mole of sulphur monochloride $(S_{2} {Cl}_{2})$ loses six moles of electrons to form a compound of sulphur. Oxidation state of sulphur in the product is (Assume chlorine atoms doesn’t show any change in oxidation state and both sulphur atoms appear in the product)

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Detailed Solution

${\overset{+ 1}{S}}_{2} {Cl}_{2}$

Total oxidation number of sulphur/mole of $S_{2} {Cl}_{2}$ = +2
1 mole of $S_{2} {Cl}_{2}$ loses ‘6’ moles of electrons
$∴$ Total increase in oxidation number = 6
Sum of oxidation numbers of two sulphur atoms in one mole of product = 2+6 = +8
$∴$ 2x = +8
x = +4
Oxidation number of sulphur in the product = +4