Chemistry > Electrochemistry > 15.0 Thermodynamics of the Cells
Electrochemistry
1.0 Introduction
2.0 Conductors and Non-Conductors
3.0 Electrochemical Cells
4.0 Electrolysis and electrode Reactions
5.0 Electrochemical Cell
6.0 Electrode Potential
7.0 Nature of Electrodes
8.0 IUPAC Cell Representation and Convention
9.0 Standard Cell EMF and Standard Reduction Potential
10.0 Electropositive Character of Metals
11.0 Difference between EMF and potential difference
12.0 Nernst Equation
13.0 Laws of Electrolysis
14.0 Electromotive Force
15.0 Thermodynamics of the Cells
16.0 Concentration Cells
17.0 Battery
18.0 Fuel Cell
15.1 Condition of Equilibrium
When ${E_{cell}} = 0.0V$ i.e., no potential difference is obtained between two terminals of the cell battery, the cell reaction is said to be in equilibrium, So from nernst equation, we have
$$\begin{equation} \begin{aligned} {E_{cell}} = {E_{cell}}^0 - \frac{{0.0591}}{n}{\log _{10}}Q \\ 0 = {E_{cell}}^0 - \frac{{0.0591}}{n}{\log _{10}}Q \\ {E_{cell}}^0 = \frac{{0.0591}}{n}{\log _{10}}Q \\ {E_{cell}}^0 = 2.303\frac{{RT}}{{nF}}{\log _{10}}{K_{eq}} \\\end{aligned} \end{equation} $$
As at equilibrium $Q$ (i.e., quotient) will be equilibrium constant.
