What factor does the Nernst equation relate to in electrochemistry?

What factor does the Nernst equation relate to in electrochemistry?

• A. The concentration of reactants and products
• B. The temperature of the reaction
• C. The type of electrode used
• D. The presence of catalysts

Answer: (A)

The Nernst equation primarily relates the electrochemical potential of a cell to the concentrations of the reactants and products involved in the redox reaction. Its form shows that the cell potential (E) depends on the standard cell potential (Eº) and a logarithmic term that incorporates the ratio of the concentrations of products to reactants, effectively reflecting how changes in concentration can shift the cell potential according to the principles of chemical equilibria. By incorporating the concentrations, the Nernst equation allows us to calculate the potential under non-standard conditions, making it a powerful tool in predicting how the voltage of a galvanic cell varies with changes in the concentration of solution components. The central focus on concentrations illustrates the relationship between thermodynamics and electrochemistry, emphasizing that even in redox reactions, the cell’s performance is directly tied to the species’ availability.

The Nernst equation primarily relates the electrochemical potential of a cell to the concentrations of the reactants and products involved in the redox reaction. Its form shows that the cell potential (E) depends on the standard cell potential (Eº) and a logarithmic term that incorporates the ratio of the concentrations of products to reactants, effectively reflecting how changes in concentration can shift the cell potential according to the principles of chemical equilibria.

By incorporating the concentrations, the Nernst equation allows us to calculate the potential under non-standard conditions, making it a powerful tool in predicting how the voltage of a galvanic cell varies with changes in the concentration of solution components. The central focus on concentrations illustrates the relationship between thermodynamics and electrochemistry, emphasizing that even in redox reactions, the cell’s performance is directly tied to the species’ availability.