Assume the cell reaction, A ( s ) + B ( aq ) + 2 → A ( aq ) + 2 + B ( s ) if Δ G ∘ = − 386 kJ at 298 K . What is E cell ∘ ?

Question

Assume the cell reaction, A ( s ) ​ + B ( aq ) + 2 ​ → A ( aq ) + 2 ​ + B ( s ) ​ if Δ G ∘ = − 386 kJ at 298 K . What is E cell ∘ ​ ?

TestHub · Accepted Answer

The relationship between standard Gibbs free energy change and standard cell potential is given by $Δ G^{\circ} = - n F E_{cell}^{\circ}$ .

For the given cell reaction, the number of electrons transferred is $n = 2$ .

Given $Δ G^{\circ} = - 386 kJ = - 386000 J$ and $F = 96500 C mol^{- 1}$ .

Substituting the values into the equation:

$- 386000 = - 2 \times 96500 \times E_{cell}^{\circ}$

$- 386000 = - 193000 \times E_{cell}^{\circ}$

$E_{cell}^{\circ} = \frac{- 386000}{- 193000} = 2 V$

Answer: 2 V

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