Enter your Anode Standard Potential (E°) and Cathode Standard Potential (E°), then provide the Temperature, Electrons Transferred (n), and Reaction Quotient (Q) to calculate the Cell Potential (Ecell) via the Nernst equation — along with the Standard Cell Potential (E°cell), Nernst Correction, and whether your reaction is feasible.
Cell Potential (Ecell)
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Standard Cell Potential (E°cell)
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Nernst Correction
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Reaction Feasibility
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A galvanic cell is an electrochemical cell that generates electrical energy from spontaneous chemical reactions. It consists of two electrodes (anode and cathode) connected by a salt bridge, where oxidation occurs at the anode and reduction at the cathode.
The electrode with the lower standard reduction potential becomes the anode (oxidation site), while the electrode with the higher standard reduction potential becomes the cathode (reduction site). The anode potential is reversed in sign when calculating cell potential.
The Nernst equation calculates cell potential at non-standard conditions: E = E° - (RT/nF)lnQ. Use it when temperature is not 25°C or when ion concentrations differ from 1 M standard conditions.
Q is the ratio of product concentrations to reactant concentrations, each raised to their stoichiometric coefficients: Q = [products]^coefficients / [reactants]^coefficients. For standard conditions, Q = 1.
A positive cell potential indicates a spontaneous reaction that can generate electrical energy. A negative cell potential means the reaction is non-spontaneous and requires external energy to proceed.
Temperature affects cell potential through the Nernst equation. Higher temperatures generally decrease cell potential for most galvanic cells, while lower temperatures increase it.
Yes, for concentration cells with identical electrodes but different concentrations, set both standard potentials to the same value and adjust the reaction quotient to reflect the concentration difference.