1.

The rusting of iron takes place as follows: 2H^(+) + 2e + 1//2O(2) rarr H_(2)O_((l)), E^(@) = +1.23 V Fe^(2+) + 2e rarr Fe_((s)), E^(@) = -0.44 V The DeltaG^(@) for the net process is :

Answer»

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

SOLUTION :`E_(cell)^(@) = E_(OPFe)^(@) + E_(RPH_(2)O)^(@)`
`:. DELTAG^(@) = -nE^(@)F`
`= -2 XX 1.67 xx 96500 J`
`= -322.31 kJ mol^(-1)`


Discussion

No Comment Found

Related InterviewSolutions