The efficiency of a hypothetical cell is about `84%` which involves the following reactions:
`A(s) + B^(2+)(aq) rightarrow A^(2+)(aq) _ B(s)` `DeltaH = -285kJ`
Then, the standard electrode potential of the cell will be: (Asume `DeltaS = 0)

Options

A. 1.20 V
B. 2.40 V
C. 1.10 V
D. 1.24 V

Answer

D

Explanation

Efficiency `= (Delta G^(@))/(Delta H^(@)) = (-nFE^(@))/(Delta H^(@))`
`0.84 = - (2 xx E^(@) xx 96500)/(-285 xx 1000)`
`E^(@) = + 1.24 V`