If the `E_(cell)^(@)` for a given reaction has a positive value, then which of the following gives the correct relationship for the values of `DeltaG^(@)` and `K_(eq)` :-

Options

A. `DeltaG^@ gt 0 ,K_(eq) lt 1 `
B. `DeltaG^@ gt 0 ,K_(eq) gt 1 `
C. `DeltaG^@ lt 0 ,K_(eq) gt 1 `
D. `DeltaG^@ lt 0 ,K_(eq) lt 1 `

Answer

A

Explanation

`:. DeltaG^@=-nFE^@ and DeltaG^@ = -RTlog_eK_(eq)`