1.

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.

Answer»

113.072 KJ `mol^(-1)`
213.072 kJ `mol^(-1)`
`313.082" kJ "mol^(-1)`
413.021 kJ `mol^(-1)`

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


Discussion

No Comment Found

Related InterviewSolutions