1.

If the E_(cell)^(@) for a given reaction has negative value, which of the following gives the correct relationships for the value of DeltaG^(@) and K_(eq)

Answer»

`DELTAG^(@)lt0,K_(eq)lt1`
`DeltaG^(@)gt0,K_(eq)lt1`
`DeltaG^(@)gt0,K_(eq)GT1`
`DeltaG^(@)lt0,K_(eq)gt1`

Solution :`E_(cell)^(o)lt0`, so it is a non spontaneous process.
`DeltaG^(o)=-NFE^(@)=+ve,` so `DeltaG^(o)gt0`
`DeltaG^(@)=-2.303RT` log K
So, `K lt 1`


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