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

Options

A. 2.14V
B. 1.80V
C. 1.07V
D. 0.82V

Answer

C

Explanation

According to Nernst equation, at STP we have `E_("cell") = E_("cell")^(@)- (0.0591)/(n) log ([Zn^(2+)])/([Cu^(2+)])= 1.1 - (0.0591)/(2) "log" (1)/(0.1)= 1.07V`