Question

What is Nernst equation. How can Nernst equation be applied in calculating the equilibrium constant for any cell reaction?

Answer 1

Explanation:

At least 17 elements are known to be essential nutrients for plants. In relatively large amounts, the soil supplies nitrogen, phosphorus, potassium, calcium, magnesium, and sulfur; these are often called the macronutrients. ... Carbon and oxygen are absorbed from the air while other nutrients are absorbed from the soil

Answer 2

Answer:

Nernst equation is an equation in electrochemistry that enables the determination of cell potential under non-standard conditions.

Equilibrium constant for any cell reaction can be calculated using Nernst equation by the following formula :

$log K _{eq}$ = $\frac{nE^{0} }{0.0592}$

Explanation:

Nernst equation relates the reduction potential of a reaction (half-cell or full cell reaction) to the standard electrode potential, temperature, and activities of the chemical species that is undergoing reduction and oxidation.

E = E° - $\frac{2.303 RT}{nF}$ $log_{10}$ Q

E - Cell potential

E° - Standard cell potential

R - Gas constant

T - Temperature

n  - Number of electrons transferred in the reaction (from balanced reaction)

F - Faraday constant (96,500 C/mol)

Q - Reaction quotient

At standard temperature T = 298 K, $\frac{2.303 RT}{F}$ = 0.0592 V

Then the Nernst equation can ne rewritten as :

E = E° - $\frac{0.0592}{n}$ $log_{10}$ Q

At equilibrium, E = 0 and Q = $K_{eq}$

where $K_{eq}$ is the equilibrium constant.

Equation can be rearranged to obtain the following relation:

$log K_{eq}$ = $\frac{nE^{0} }{0.0592}$