The standard emf of a cell, involving one electron change is...

The standard emf of a cell, involving one electron change is found to be $0.591 \mathrm{~V}$ at $25^{\circ} \mathrm{C}$. The equilibrium constant of the reaction is $\left(F=96500 \mathrm{C} \mathrm{mol}^{-1}, \mathrm{R}\right.$ $\left.=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)$ (a) $1.0 \times 10^{30}$ (b) $1.0 \times 10^{1}$ (c) $1.0 \times 10^{5}$ (d) $1.0 \times 10^{10}$

The standard emf of a cell, involving one electron change is found to be $0.591 \mathrm{~V}$ at $25^{\circ} \mathrm{C}$. The equilibrium constant of the reaction is $\left(F=96500 \mathrm{C} \mathrm{mol}^{-1}, \mathrm{R}\right.$ $\left.=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)$
(a) $1.0 \times 10^{30}$
(b) $1.0 \times 10^{1}$
(c) $1.0 \times 10^{5}$
(d) $1.0 \times 10^{10}$

Key Concepts

Relation Between Cell Potential and Equilibrium Constant

This key concept involves using the relationship between the Gibbs free energy change and the cell’s electromotive force to determine the equilibrium constant. The equation ?G° = –nFE° leads to ln K = (nFE°)/(RT), illustrating how a higher standard cell potential corresponds to a more thermodynamically favorable reaction and a larger equilibrium constant.

Nernst Equation

The Nernst equation is a fundamental relation in electrochemistry that links the cell potential to the concentrations (or activities) of the redox species, temperature, and the number of electrons transferred in the reaction. It allows for the calculation of the cell potential under non-standard conditions and underpins the connection between cell potential and reaction equilibrium.

Standard Electromotive Force (emf)

This concept refers to the inherent voltage difference between two electrodes in an electrochemical cell when all species are at their standard states. It serves as a measure of the chemical potential driving the redox reaction and is determined under conditions where the reactants and products are at unit activity.

Electrochemical Cells

Electrochemical cells are devices that convert chemical energy to electrical energy through redox reactions. They consist of two electrodes where oxidation and reduction reactions occur separately, and their behavior and efficiency are characterized by parameters such as the standard state potentials and cell emf.

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