In electronic watch zinc/silver oxidation cell is used, which gives following reactioni :
`Zn^(2+)+2e^(-) to Zn,E^(@)=-0.760V`
`Ag_(2)O+H_(2)O+2e^(-) to 2Ag+2OH^(-),E^(@)=0.344V`
If F=96500 C `mol^(-1)` then find out `DeltaG^(@) ` of cell.

Options

A. 113.072 kJ `mol^(-1)`
B. 213.072 kJ `mol^(-1)`
C. `313.082" kJ "mol^(-1)`
D. 413.021 kJ `mol^(-1)`

Answer

B

Explanation

`E_(cell)^(0)=0.344-(-0.76)=1.104`
`DeltaG^(@)=-nFE_(cell)^(@)`
`=-2xx96500xx1.104`
`=213072" J "mol^(-1)=213.072` kJ/mol