calculate the electromotive force of the cell assumed cell reaction at 20:05 degrees celsius with the reaction cu plus 2 ag plus 2 cu 2 plus plus 2 ag e note of cell is 2.97 volt
Free calculate electromotive force (emf) and cell potential for electrochemical cells using nernst equation.
Enter Cell Data
V
Standard cell potential
Electrons transferred in reaction
Products/Reactants concentration ratio
J/mol·K
Default: 8.314 J/mol·K
Results
Enter cell data to calculate EMF
Nernst Equation
Nernst Equation
E = E° - (RT/nF) × ln(Q)
- • E = Cell potential (V)
- • E° = Standard cell potential (V)
- • R = Gas constant (8.314 J/mol·K)
- • T = Temperature (K)
- • n = Number of electrons
- • F = Faraday constant (96485 C/mol)
- • Q = Reaction quotient
Key Concepts
- • EMF drives electron flow
- • Higher EMF = stronger driving force
- • Q = 1 at standard conditions
- • Positive EMF = spontaneous reaction
- • Used in batteries, fuel cells