1.

The half-cell reactions for rusting of iron are 2H^(+)+(1)/(2)+2e^(-)toH_(2),E^(@)=+1.23V, Fe^(2+)+2e^(-)toFe(s),E^(@)=-0.44V DeltaG^(@) (in kJ) for the reaction is

Answer»

`-76`
`-322`
`-122`
`-176`

Solution :For emf to be +ve, oxidation should OCCUR at iron electrode.
`E_(cell)=1.23+0.44V=1.67V`
`DeltaG^(@)=-nFE_(cell)^(@)=-2xx96500xx1.67J`
=-322kJ.


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