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Efficiency of a cell reaction under stan...

Efficiency of a cell reaction under standard conditions,
`A_((s)) + B^(+) rarr A^(+) + B_(s), DeltaH^(@) = -300 kJ`
is `70%`. The standard electrode potential of cell is :

A

`2.176 V`

B

`+ 2 .876 V`

C

`1.248 V`

D

`+ 1.648 V`

Text Solution

Verified by Experts

The correct Answer is:
A
Efficiency `= (DeltaG^(@))/(DeltaH^(@)) = (nE^(@)F)/(DeltaH^(@))`
`E^(@) = ("Efficiency" xx DeltaH^(@))/(-nF)`
`= (70 xx (-300 xx 10^(+3)))/(1000 xx (-1) xx 96500) = 2.176 V`
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