The standard emf of a galvanic cell involving cell reaction with n=2 is found to be 0.295 V at

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The standard emf of a galvanic cell involving cell reaction...

The standard emf of a galvanic cell involving cell reaction with $\mathrm{n}=2$ is found to be $0.295 \mathrm{~V}$ at $25^{\circ} \mathrm{C}$. The equilibrium constant of the reaction would be (Given $\left.F=96500 \mathrm{C} \mathrm{mol}^{-1} ; \mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)$ (a) $2.0 \times 10^{11}$ (b) $4.0 \times 10^{12}$ (c) $1.0 \times 10^{2}$ (d) $1.0 \times 10^{10}$

The standard emf of a galvanic cell involving cell reaction with $\mathrm{n}=2$ is found to be $0.295 \mathrm{~V}$ at $25^{\circ} \mathrm{C}$. The equilibrium constant of the reaction would be (Given $\left.F=96500 \mathrm{C} \mathrm{mol}^{-1} ; \mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)$
(a) $2.0 \times 10^{11}$
(b) $4.0 \times 10^{12}$
(c) $1.0 \times 10^{2}$
(d) $1.0 \times 10^{10}$

Key Concepts

Galvanic Cell

A galvanic cell is an electrochemical cell that converts chemical energy into electrical energy through a spontaneous redox reaction. It operates under standard or non-standard conditions to produce a potential difference between electrodes, allowing for the calculation of reaction parameters such as free energy change and equilibrium constant.

Standard Electromotive Force (emf)

The standard electromotive force (emf) refers to the cell potential measured under standard conditions (usually 1 M concentration, 1 atm pressure, and 25°C). It is a critical parameter that quantifies the driving force of the redox reaction in the cell and is directly linked to the maximum achievable work from the cell reaction.

Gibbs Free Energy and Equilibrium Constant Relationship

The relationship between Gibbs free energy and the equilibrium constant is fundamental in thermodynamics. The standard free energy change (?G°) is related to the standard emf by the equation ?G° = -nFE°, and is also linked to the equilibrium constant (K) via the equation ?G° = -RTlnK. This relationship allows the calculation of the equilibrium constant of a reaction using electrical measurements.

Nernst Equation

The Nernst equation relates the cell potential to the reaction quotient, accounting for non-standard conditions. It provides a way to calculate the cell potential at any given moment, which is useful for understanding reaction dynamics and the shift to equilibrium. Although the standard emf applies to equilibrium conditions, the Nernst equation is pivotal in linking real-time measurements to thermodynamic parameters.

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