Question

The standard emf of the galvanic cell involving $3$ mole of electron in a redox reaction ${\text{0}}{\text{.59V}}$. The equilibrium constant in the cell reaction is _________.

Answer 1

Standard electrode potential (${E^0}$) is defined as the value of the standard emf of a cell in which molecular hydrogen is oxidised to solvated protons at the left-hand electrode under standard pressure.

Complete answer:
The equilibrium constant, K, describes the relationship between a reaction's products and reactants when it is at equilibrium with respect to a particular unit. A chemical reaction's equilibrium constant is the value of its reaction quotient at chemical equilibrium, a condition reached by a dynamic chemical system after a period of time has passed in which its composition shows no discernible propensity to alter.
The equilibrium constant is independent of the initial analytical concentrations of the reactant and product species in the mixture for a given set of reaction conditions. As a result, provided a system's initial composition, known equilibrium constant values can be used to calculate the system's equilibrium composition.
According to the question, we can understand that
The standard emf of a galvanic cell with a redox reaction involving $3$ moles of electrons is ${\text{0}}{\text{.59V}}$ volt.

$${{\text{E}}_{{\text{cell}}}}{\text{ = 0}}{\text{.59}}\,{\text{volt}} \\\ {\text{n = 3}} \\\$$

The following is the equilibrium constant for the cell's reaction:
${\text{lnK = }}\dfrac{{3 \times 96500 \times 0.59}}{{8.314 \times 298}}$
So we have got the equation for lnK.
Now we can look at how lnK is calculated.
${\text{lnK}} = \dfrac{{3 \times 96500 \times 0.59}}{{8.314 \times 298}}$
Substituting the values , we get lnK=$68.9$
Therefore, K=${10^{30}}$
As a result, the equilibrium constant for the cell reaction is ${10^{30}}$.

Note:
The value of the equilibrium constant can be influenced by reaction parameters such as temperature, solvent, and ionic pressure. Equilibrium constants include stability constants, formation constants, binding constants, interaction constants, and dissociation constants.