Which equation is fundamental to understanding the effect of reactant concentration on cell potential?

The Nernst equation is fundamental to understanding the effect of reactant concentration on cell potential because it quantitatively relates the concentration of reactants and products to the electromotive force (EMF) of an electrochemical cell. It provides a way to calculate the cell potential under non-standard conditions by taking into account the concentrations of the chemical species involved in the redox reaction.

The Nernst equation is expressed as:

[ E = E^\circ - \frac{RT}{nF} \ln Q ]

where ( E ) is the cell potential, ( E^\circ ) is the standard cell potential, ( R ) is the universal gas constant, ( T ) is the temperature in Kelvin, ( n ) is the number of moles of electrons transferred in the reaction, ( F ) is Faraday's constant, and ( Q ) is the reaction quotient, which depends on the concentrations of the reactants and products.

This relationship demonstrates how fluctuations in concentration can lead to changes in the cell potential, enabling predictions about how the cell behaves under varying conditions. Understanding this dynamic is crucial for the design and optimization of electrochemical cells for various applications, such as batteries and fuel cells.

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