Question

If `E_(cell)^(ɵ)` for a given reaction is negative, which gives the correct relationships for the values of `DeltaG^(ɵ)` and `K_(eq)`?
A. `Delta G^(@) gt , K_(eq) gt 1`
B. `Delta G^(@) lt 0 , K_(eq) gt 1`
C. `DeltaG^(@) lt 0 , K_(eq) lt 1`
D. `DeltaG^(@) gt 0 , K_(eq) lt 1`

Answer 1

Correct Answer - D
`Delta G^(@) = - n FE_(cell)^(@)` and `Delta G^(@) = -2.303 RT log K_(eq)`