If `E_(cell)^(ɵ)` for a given reaction is negative, which gives the correct relationships for the values of `DeltaG^(ɵ)` and `K_(eq)`?

Options

A. ` DeltaG^@ gt 0 , K(eq) lt 1`
B. ` Delta G^@ gt 0K_(eq) , K)(eq) gt 1`
C. ` Delta G^@ lt 0, K_(eq) gt 1`
D. ` Zgt X gt Y`

Answer

A

Explanation

`E^@ = (0. 059)/n log K_(eq) and Delta G^@ More si E_(CP)^@`F
`:. Delta G^@ + ve , E^@` will be -and`K_(eq) lt` one shoule not writed Delta `G^@ gt 0`.