Question

If the E°꜀ₑₗₗ for a given reaction has a negative value, then
which of the following gives the correct relationships for
the values of ∆G° and Kₑq ?
(a) ∆G° > 0 ; Kₑq > 1 (b) ∆G° < 0 ; Kₑq > 1
(c) ∆G° < 0 ; Kₑq < 1 (d) ∆G° > 0 ; Kₑq < 1

Answer 1

$\huge{\boxed{\mathfrak\pink{\fcolorbox{red}{purple}{Mr\:Awesome}}}}$

❤.option D is correct

Answer 2

If the E°꜀ₑₗₗ for a given reaction has a negative value, then the  correct relationships for the values of ∆G° and Kₑq is :

(d) ∆G° > 0 ; Kₑq < 1

• We know that,

       ∆G° = - nFE°

• Since, E°꜀ₑₗₗ  is negative, i.e E°꜀ₑₗₗ  <0

• Therefore,

       ∆G° = - nF(-E°)

              = +ve

• Hence, ∆G° >0

• Also,

        ∆G° = -RT ln Kₑq

        ⇒ - nFE° = -RT ln Kₑq

• Since, R and T can't be negative, thus, Kₑq <0