Which of the following equations is correct for the relation between standard cell potential and equilibrium constant?
- A$E_{cell}^0 = \log_{10} K \frac{n}{0.0592}$
- B$E_{cell}^0 = \frac{0.0592}{n} \log_{10} K$
- C$E_{cell} = \frac{0.0592}{n} \log_{10} K$
- D$E_{cell} = \log_{10} K \frac{n}{0.0592}$
Explore More
Similar Questions
If a solution of $Cu^{+2}/Cu$ at $298 \, K$ is diluted $100$ times,how will the electrode potential change?
Difficult
View SolutionWhich is the proper value of $x$ for the following to increase the cell potential of $Zn_{(s)} | Zn_{(x \ M)}^{2+} || Cu_{(0.02 \ M)}^{2+} | Cu_{(s)}$?
Derive the Nernst equation for the following galvanic cell: $Ni_{(s)}|Ni_{(aq)}^{2+}\parallel Ag_{(aq)}^{+}|Ag_{(s)}$
Medium
View SolutionThe Nernst equation is related to:
Easy
View SolutionFor a cell reaction involving a two-electron change,the standard emf of the cell is found to be $0.295 \ V$ at $25 \ ^oC$. The equilibrium constant of the reaction at $25 \ ^oC$ will be
DifficultAIPMT 2004
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo