For a certain redox reaction in galvanic cell X ( s ) + Y ( a q ) 2 + ⟶ X ( a q ) 2 + + Y ( s ) , E ∘ cell is 0.0296 V at 298 K . What is equilibrium constant of reaction?

Question

For a certain redox reaction in galvanic cell X ( s ) ​ + Y ( a q ) 2 + ​ ⟶ X ( a q ) 2 + ​ + Y ( s ) ​ , E ∘ cell is 0.0296 V at 298 K . What is equilibrium constant of reaction?

TestHub · Accepted Answer

The relation between standard cell potential and equilibrium constant at $298 K$ is given by:

$E_{cell}^{\circ} = \frac{0.0591}{n} lo g K_{c}$

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

Substituting the given values:

$0.0296 = \frac{0.0591}{2} lo g K_{c}$

$0.0296 \approx 0.02955 lo g K_{c}$

$lo g K_{c} = \frac{0.0296}{0.02955} \approx 1$

$K_{c} = 1 0^{1} = 10$

Answer: $10$

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