1.

The rusting of iron takes place as follows 2H^(+)+2e^(-)+1//2O_(2)toH_(2)O_((l)),E^(@)=+1.23V Fe^(2+)+2e^(-)toFe_((s)),E^(@)=-0.44V Calculate DeltaG^(@) for the net process

Answer»

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

Solution :`Fe(s)toFe^(2+)+2E^(-),DeltaG_(1)^(o)`
`underline("2H^(+)+2e^(-)+1//2O_(2)toH_(2)O(l),DeltaG_(2)^(o)"")`
`Fe(s)+2H^(+)+1//2O_(2)toFe^(2+)+H_(2)O,DeltaG_(3)^(o)`
APPLYING, `DeltaG_(1)^(o)+DeltaG_(2)^(o)=DeltaG_(3)^(o)`
`DeltaG_(3)^(o)=(-2Fxx0.44)+(-2Fxx1.23)`
`DeltaG_(3)^(o)=-(2xx96500xx0.44+2xx96500xx1.23)`
`DeltaG_(3)^(o)=-322310J`
`thereforeG_(3)^(o)=-322kJ`


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