Question

Calculate the standard potential, E ∘ , E°, for this reaction from its Δ G ∘ ΔG° value. X ( s ) + Y 4 + ( aq ) ⟶ X 4 + ( aq ) + Y ( s ) Δ G ∘ = − 48.0 kJ

Answer 1

Answer: 0.124 V

Explanation:

$X(s)+Y^{4+}(aq)\rightarrow X^{4+}(aq)+Y(s)$

To calculate standard Gibbs free energy, we use the equation:

$\Delta G^o=-nFE^o_{cell}$

Where,

n = number of electrons transferred = 4

F = Faradays constant = 96500 C

$E^o_{cell}$ = standard cell potential = ?

Putting values in above equation, we get:

$-48.0\times 1000=-4\times 96500\times E^0{cell}$

$E^o_{cell}=0.124$

Thus the standard potential E°, for this reaction is 0.124 V