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Nernst Equation: Application & Numerical (Part - 13)- Electrochemistry, Chemistry, Class 12 Video Lecture

FAQs on Nernst Equation: Application & Numerical (Part - 13)- Electrochemistry, Chemistry, Class 12 Video Lecture

1. What is the Nernst equation and how is it used in electrochemistry?

Ans. The Nernst equation is a mathematical equation that relates the equilibrium potential of an electrochemical cell to the concentration of reactants and products. It is given by E = E° - (0.0592/n)log(Q), where E is the cell potential, E° is the standard cell potential, n is the number of moles of electrons transferred, and Q is the reaction quotient. This equation is used to calculate the cell potential under non-standard conditions and determine the feasibility of a redox reaction.

2. How can the Nernst equation be applied to calculate the cell potential at non-standard conditions?

Ans. The Nernst equation can be applied by substituting the appropriate values for E°, n, and Q. First, determine the values of the concentrations of reactants and products involved in the redox reaction. Then, calculate the reaction quotient (Q) by dividing the concentration of products by the concentration of reactants. Finally, substitute these values into the Nernst equation to calculate the cell potential (E) at non-standard conditions.

3. What role does temperature play in the Nernst equation?

Ans. Temperature plays a crucial role in the Nernst equation as it affects the cell potential. The Nernst equation includes a term (0.0592/n)log(Q), where n is the number of moles of electrons transferred. The logarithm term is multiplied by a constant (0.0592/n) that incorporates the effect of temperature. As temperature increases, the value of the constant decreases, resulting in a larger contribution from the logarithm term. Therefore, temperature influences the cell potential by altering the concentration-dependent term of the Nernst equation.

4. How does the Nernst equation help determine the feasibility of a redox reaction?

Ans. The Nernst equation helps determine the feasibility of a redox reaction by comparing the calculated cell potential (E) to the standard cell potential (E°). If the calculated cell potential is positive, it means that the reaction is feasible and spontaneous under the given conditions. Conversely, if the calculated cell potential is negative, the reaction is not feasible and non-spontaneous. The Nernst equation provides a quantitative measure of the driving force behind the redox reaction and allows for the prediction of its feasibility.

5. Can the Nernst equation be used to calculate the standard cell potential of a redox reaction?

Ans. No, the Nernst equation cannot be used to directly calculate the standard cell potential (E°) of a redox reaction. The Nernst equation is applicable for calculating the cell potential at non-standard conditions, where the concentrations of reactants and products are not at their standard states. The standard cell potential, on the other hand, is a thermodynamic property that represents the cell potential under standard conditions (concentrations of 1 M and pressure of 1 atm). The standard cell potential can be determined experimentally or obtained from reference tables.

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