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If the E("cell")^(@) for a given reactio...

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

A

`DeltaG^(ɵ) gt 0, K_(eq) lt 1`

B

`DeltaG^(ɵ) gt 0, K_(eq) gt 1`

C

`DeltaG^(ɵ) lt 0, K_(eq) gt 1`

D

`DeltaG^(ɵ) lt 0, K_(eq) lt 1`

Text Solution

Verified by Experts

The correct Answer is:
A
`DeltaG=-nFE^(ɵ)` or `E^(@)=(-DeltaG)/(nF)`
`:. DeltaG^(ɵ) gt 0` and `DeltaG^(ɵ)=-nRT In K_(p)`
`:. K_(eq) lt1`
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