Electrochemistry Calculator
Nernst Equation
Calculate non-standard cell potential
Standard Cell Potential
Calculate E°cell from two half-reactions
Faraday's Law of Electrolysis
Calculate mass deposited during electrolysis
Formula
E = E° - (RT/nF)ln(Q) | E°cell = E°cathode - E°anode | m = (ItM)/(nF) | F = 96,485 C/mol
Frequently Asked Questions
What is the Nernst equation?
E = E° - (RT/nF)ln(Q), or at 25°C: E = E° - (0.0592/n)log(Q). It calculates the cell potential under non-standard conditions. E° is standard potential, n is electrons transferred, Q is reaction quotient.
How do I calculate standard cell potential?
E°cell = E°cathode - E°anode, where both values are standard reduction potentials. The cathode is where reduction occurs (higher E°) and the anode is where oxidation occurs (lower E°). E°cell > 0 means the reaction is spontaneous.
What is Faraday's law?
Faraday's law relates charge passed to mass deposited: m = (Q × M)/(n × F), where Q = I × t (charge in coulombs), M is molar mass, n is electrons per ion, and F = 96,485 C/mol (Faraday constant).
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