Question

If the `E_(cell)^(o)` for a given reaction has a negative value, then whih of the following gives the correct relationships for the value of `DeltaG^(@) and K_(eq)`
A. `DeltaG^(@)gt0,K_(eq)lt1`
B. `Delta^(@)gt0,K_(eq)gt1`
C. `DeltaG^(+)lt0,K_(eq)gt1`
D. `DeltaG^(@)lt0,K_(eq)lt1`

Answer 1

Correct Answer - A
`ThereforeDeltaG^(@)=-nFE^(@) and DeltaG^(@)=-Rtlog_(e)K_(eq)`