ChemistryFor a cell reaction involving a two-electron change, the standard e.m.f. of the cell is found to be 0.295 V at 25 0 C. The equilibrium constant of the reaction at 25 0 C will be

For a cell reaction involving a two-electron change, the standard e.m.f. of the cell is found to be 0.295 V at 25⁰C. The equilibrium constant of the reaction at 25⁰C will be

A
1 × 10–10
B
29.5 × 10–2
C
10
D
1 × 1010

Solution:

From Thermodynamics ${ΔG}^{o} = - 2.303 {RTlogK}_{c}$

${ΔG}^{O} = - {nFE}^{o}$

Equating both and simplifying

${logK}_{c} = \frac{{nFE}^{o}}{2.303 RT} = \frac{{nE}^{o}}{0.0591} = \frac{2 \times 0.295}{0.0591} = 10$

$K_{c} = 10^{10}$

Related content

Prepare M/20 Solution of Ferrous Ammonium Sulphate

Difference Between Thermoplastic And Thermosetting Plastic

Bleaching Powder

pH Full Form

Difference Between Metals and Nonmetals

Difference Between Orbit and Orbital

Difference between Homogeneous and Heterogeneous

Differences & Comparisons Articles in Chemistry

Magnesium oxide Formula

Barium Chloride Formula

For a cell reaction involving a two-electron change, the standard e.m.f. of the cell is found to be 0.295 V at 25⁰C. The equilibrium constant of the reaction at 25⁰C will be

Solution:

Related content

Company

Support

Courses

More

JEE

NEET

CBSE

NCERT solutions

NCERT exemplar

State Board

Subject

Rank Predictor

Engineering Entrance Exam

follow us