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12.53 cm^(3) of 0.51 M SeO(2) reacts ex...

12.53 `cm^(3)` of 0.51 M `SeO_(2)` reacts exactly with 25.5 `cm^(3)` of 0.1 M `CrSO_(4)` which is oxidised `Cr(SO_(4))_(3)` To what oxidation state is the selenium converted during the reaction ?

Text Solution

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Let O.N of se in the new compound =x

Now 12.53 `cm^(3)` of 0.051 M `SeO_(2)=12.53xx0.51=0.63` millimoles of `SeO_(2)`
and 25.5 `cm^(3)` of 0.1 M `CrSO_(4)=25.5xx0.1=2.55` millimole of `CrSO_(2)`
But according to balanced redox equation (4-x) moles of `CrSO_(4)` reduce 1 mole of `SeO_(2)`
`therefore2.55` millimoles of `CrSO_(4)` it reduce `SeO_(2)=(2.55)/(4-x)` millimoles
But `SeO_(2)` actually reduced = 0.64 millimoles
Equating these two values we have`(2.55)/(4-x)=0.64 or x=0`
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