Consider the following reaction,
`Zn(s)+Cu^(2+) (0.1 M) rarr Zn^(2+) (1 M)+Cu(s)` above reaction, taking place in a cell, `E_("cell")^(@)` is `1.10 V. E_("cell")` for the cell will be `(2.303 (RT)/(F)=0.0591)`

Options

A. `1.07` volt
B. `0.82` volt
C. `2.14` volt
D. `1.80` volt

Answer

A

Explanation

Applying Nernst equation
`E_(cell) = E_(cell)^(@) =- (0.0591)/(2)log. |(Sn^(2+))/(Cu^(2+))|`
`=1.1 -(0.0591)/(2)log.(1)/(0.1)`
`1.1 - 0.02955`
`=1.07`