Question

what is nernst equation?

Answer 1

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$\underline\color{Green}{NERST\: EQUATION}$

☆Nernst equation is an important relation which is used to determine reaction equilibrium constants and concentration potentials

as well as to calculate the minimum energy required in electrodialysis as will be shown later.

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Answer 2

Answer:

Explanation:

NERST EQUATION;

The Nernst equation provides a relation between the cell potential of an electrochemical cell, the standard cell potential, temperature, and the reaction quotient. Even under non-standard conditions, the cell potentials of electrochemical cells can be determined with the help of the Nernst equation.

The Nernst equation is often used to calculate the cell potential of an electrochemical cell at any given temperature, pressure, and reactant concentration. The equation was introduced by a German chemist Walther Hermann Nernst.

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.

⇒ Also Read: Redox Reactions

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 25°C

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.