Nernst Equation Using Reaction Quotient

The Nernst equation is an equation that relates the reduction potential of an electrochemical reaction (half-cell or full-cell reaction) to the standard electrode potential, temperature and activities (often approximated by concentrations) of the chemical species undergoing reduction and oxidation.

The cell potential equals the standard cell potential minus the logarithm of the reaction quotient times the product of the molar gas constant and temperature divided by the product of the number of electrons transferred and the Faraday constant.

Formula

QuantityVariable[Subscript["E", "cell"], "ElectricPotential"] == QuantityVariable[Superscript["E", "0"], "ElectricPotential"] - Row[{Log[QuantityVariable["Q", "Unitless"]]}]*Row[{(Quantity[1, "MolarGasConstant"/"FaradayConstant"]*QuantityVariable["T", "Temperature"])/QuantityVariable["n", "Unitless"]}]

symbol	description	physical quantity
E_cell	cell potential	"ElectricPotential"
E⁰	standard cell potential	"ElectricPotential"
Q	reaction quotient	"Unitless"
n	number of electrons transferred	"Unitless"
T	temperature	"Temperature"

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$FormulaData[ ResourceObject[ "Nernst Equation Using Reaction Quotient"], {QuantityVariable[ "n","Unitless"] -> 1, QuantityVariable["Q","Unitless"] -> 3.33`3.*^13, QuantityVariable["T","Temperature"] -> Quantity[298.15`, "Kelvins"]}]$

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Nernst Equation Using Reaction Quotient

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