MHT CET202416 May 2024Evening ShiftChemistryElectrochemistryActual
Which from following equations represents a correct relationship between standard cell potential and equilibrium constant for cell reaction?
Options
- AE _ cell ^ =- 2.303 RT nF
- BE _ cell ^ = 0.0592 nF ₁₀ ~K
- CE _ cell ^ = 0.0592 n ₁₀ ~K
- DE _ cell ^ = 0.0592 n K
Correct answer
C. E _ cell ^ = 0.0592 n ₁₀ ~K
Step-by-step solution
The correct equation that represents the relationship between the standard cell potential and the equilibrium constant for the cell reaction is: (3) E_ cell ^ = 0.0592 n ₁₀(K) The general relationship between the standard cell potential E_ cell ^ and the equilibrium constant K is given by the Nernst equation, specifically in its standard form: E_ cell ^ = 0.0592 n ₁₀(K)