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All the energy released from the reactio...

All the energy released from the reaction `XrarrY,Delta_(r)G^(@)=-193kJ"mol"^(-1)` is used for oxidising `M^(@)` as `M^(+)rarrM^(3+)+2e^(-),E^(@)=-0.25V`.
Under standard conditions, the number of moles of `M^(+)`oxidised when one mole of X is converted to Y is `[F=96500C "mol"^(-1)]`

Text Solution

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Given data is :
`X to Y , Delta_(r)G^(@)=-193" kJ "mol^(-1)`
`M^(+) to M^(3+)+2e^(-) , E^(@)=-0.25" V"`
`193" kJ"` of energy is used to oxidise x mol of `M^(+)` ions to `M^(3+)` ions.
For 1 mole of `M^(+)`
`DeltaG^(@)=-nFE^(@)=(- mol)xx96500" C")xx(0.25" V")`
`=48250" J "mol ^(-1)=48.25" kJ "mol^(-1)`
`48.25" kJ"` of energy is used oxidise =1 mol
193.0 kJ of energy is used to oxidise
`=(1 mol)xx((193.0" kJ"))/((48.25" kJ"))=4 mol " ":. x=4`
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