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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)]`

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The correct Answer is:
4
`x rarr y`
`/_\_t,G^0-193kJmol^(-1)`
`M^+ rarr m^(+3)+2e`
`E^0=-0.25V`
`/_\ G=+2xxFxx1//4`
`/_\GF/2=96500/2`
`/_\G=48250/1000 kJ//"mole"`
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All the energy released from the reaction XtoY,Delta _(r)G^(@) = -193KJmol^(-1) is used for oxidizing M^(+) as M^(+)toM^(3+)+ 2e^(-) , e^(@) =-0.25V . Under standard conditions, the number of moles of oxidized when one mole of X is converted to Y is [F = 96500Cmol^(-1)]

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)]

All the energy released from the reaction Xto Y , Delta_(r) G^(@) = -330.03KJ//mol is used for of moles of M ^(+) oxidisesd when one mol of X is converted to Y is: (F= 96500Cm1^(-1) )

For a call reaction DeltaG^(@)=-1930(kJ)/(mol) and the cell e.m.f (E^(@)) at standard condition is 2.5 V. What is value of (DeltaG^(@))/(2FE^(@)) ?

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