Chemistry class - Topic taught as on 21/4/21

Expression of Nernst Equation
Nernst equation is an equation relating the capacity of an atom/ion to take up one or more electrons (reduction potential) measured at any conditions to that measured at standard conditions (standard reduction potentials) of 298K and one molar or one atmospheric pressure.
Nernst Equation for Single Electrode Potential
Ecell = E0 – [RT/nF] ln Q
Where,
Ecell = cell potential of the cell
E0 = cell potential under standard conditions
R = universal gas constant
T = temperature
n = number of electrons transferred in the redox reaction
F = Faraday constant
Q = reaction quotient
The calculation of single electrode reduction potential (Ered) from the standard single electrode reduction potential (E°red) for an atom/ion is given by the Nernst equation.
For a reduction reaction, Nernst equation for a single electrode reduction potential for a reduction reaction
Mn+ + ne– → nM is;
Ered = EMn+/M = EoMn+/M – [2.303RT/nF] log [1/[Mn+]]
Where,
R is the gas constant = 8.314 J/K Mole
T = absolute temperature,
n = number of mole of electron involved,
F = 96487 (≈96500) coulomb/mole = charged carried by one mole of electrons.
[Mn+] = active mass of the ions. For simplicity, it may be taken as equal to the molar concentration of the salt.
Nernst Equation at 25oC
For measurements carried out 298K, the Nernst equation can be expressed as follows.
E = E0 – 0.0592/n log10 Q
Therefore, as per the Nernst equation, the overall potential of an electrochemical cell is dependent on the reaction quotient.
Classwork
Derivation of Nernst Equation
Homework
1. Nernst Equation Applications
2. Limitations of Nernst Equation


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