To find out how the variation of equilibrium constant would be plotted against cell potential, if the logarithmic scale is not used, we have. Concept Introduction : The equilibrium constant for an electrochemical cell is determined by taking into consideration the two factors mentioned below: a) The standard state potential for the electrochemical cell b) The half-reactions involved in the electrochemical cell. The Nernst equation is used in determining the equilibrium constant. E c e l l = E o c e l l − ( R T n F ) log Q E o c e l l = Standard cell potential R = 8.3145J/mol-K (gas constant) T = temperature n=number of moles of electrons that gets transferred by the reaction of the electrochemical cell F=96484.56 C/mol Q= reaction quotient. At equilibrium, the value of the reaction quotient is equal to the value of the equilibrium constant.

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Chapter 13, Problem 13.50PAE

Interpretation Introduction

Interpretation: To find out how the variation of equilibrium constant would be plotted against cell potential, if the logarithmic scale is not used, we have.

Concept Introduction:

The equilibrium constant for an electrochemical cell is determined by taking into consideration the two factors mentioned below:

a) The standard state potential for the electrochemical cell

b) The half-reactions involved in the electrochemical cell.

The Nernst equation is used in determining the equilibrium constant.

Ecell=Eocell−(RTnF)logQ

Eocell = Standard cell potential

R = 8.3145J/mol-K (gas constant)

T = temperature

n=number of moles of electrons that gets transferred by the reaction of the electrochemical cell

F=96484.56 C/mol

Q= reaction quotient.

At equilibrium, the value of the reaction quotient is equal to the value of the equilibrium constant.

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