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All the energy realesed from the reation...

All the energy realesed from the reation `X rarr Y, Delta_(r) G^(@) = -193 kJ mol^(-1)`, is used for oxidizing `M^(+)` as `M^(+) rarr M^(3+) + 2e^(-), E^(@) = -0.25 V`. Under standard consistions, the number of moles of `M^(+)` oxidized when on e mol of `X` is converted to `Y` is `[F = 96,500 C "mol"^(-1)]`

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The correct Answer is:
4
`X to Y, DeltaG^(@) =-193 kJ mol^(-1)`
`M^(+) to M^(3+) + 2e^(-) , E^(@) = -0.25` V
Hence, `DeltaG^(@)` for oxidation will be
`DeltaG^(@) = -nFE^(@)`
`=-2 xx 96500 xx (-0.25) = 48250 J = 48.25` kJ
`therefore 193 kJ` energy oxidises `(193/48.25)` mole `M^(+) =4` mole `M^(+)`
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