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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)]`

A

`4`

B

`3`

C

`1`

D

`5`

Text Solution

Verified by Experts

The correct Answer is:
A
`M^(+) rarr M^(3+)+2e^(-), E^(@) = -0.25 V`
Thus, `DeltaG^(@)` for this reaction is
`DeltaG^(@) = -nfE^(@)`
`= -(2 "mol")(96,500 C "mol"^(-1)(-0.25 V)`
`= 48250 J mol^(-1)`
`= 48.25 kJ mol^(-1)`
We have
`X rarr Y, Delta_(r) G^(@) = -193 kJ/mol`
Thus, The number of moles of `M^(+)` oxidized when one mol of `X` is converted to `Y` is
`(193 kJ)/(48.25 kJ/mol) = 4 "mol"`
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