1.

The rusting of iron takes place as follows 2H^(+)+2e^(-)+1//2O_(2)rarrH_(2)O(l), E^(@)=+1.23 VFe^(2+)+2e^(-)rarrFe(s), E^(@)=-0.44VCalculate DeltaG^(@)for the net process

Answer»

`-322 kJ mol^(-1)`
`-161 kJ mol^(-1)`
`-152 kJ mol^(-1)`
`-76 kJ mol^(-1)`

Solution :`FE(s)RARRFE^(2+)+2e^(-), ""E^(@)=0.44 V`
`(2H^(+)+2e^(-)+1//2O_(2)rarrH_(2)O(l),""E^(@)=+1.23 V)/(Fe(s)+2H^(+)+1//2O_(2)rarrFe^(2+)+H_(2)O,)`
`E_("CELL")^(@)=0.44+1.23=1.67 V`
`thereforeDeltaG^(@)="-nF " E_("cell")^(@)=-2xx96500xx1.67=-322 kJ`.


Discussion

No Comment Found

Related InterviewSolutions