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Video: Nernst Equation Video Lecture - NEET
FAQs on Video: Nernst Equation Video Lecture - NEET
| 1. What is the Nernst equation? |  |
Ans. The Nernst equation is an equation that relates the concentration of reactants and products in an electrochemical cell to the cell potential. It is commonly used to calculate the equilibrium potential of a half-cell or to determine the concentration of an ion in a solution.
| 2. How is the Nernst equation derived? | |
Ans. The Nernst equation is derived from the principles of thermodynamics and electrochemistry. It is based on the concept of the standard electrode potential and the activities of the ions involved in the redox reaction. By considering the concentration of reactants and products, the equation provides a way to calculate the potential of an electrochemical cell under non-standard conditions.
| 3. What does the Nernst equation tell us about a cell's potential? | |
Ans. The Nernst equation allows us to calculate the cell potential at non-standard conditions, i.e., when the concentrations of reactants and products are not at their standard states. It tells us that the cell potential is directly proportional to the logarithm of the ratio of product concentrations to reactant concentrations. This relationship helps in understanding how changes in concentration affect the overall potential of the cell.
| 4. How is the Nernst equation used in practice? | |
Ans. The Nernst equation is widely used in various fields, especially in electrochemistry and analytical chemistry. It is used to determine the concentration of ions in a solution by measuring the cell potential and known concentrations of other species. It is also used to predict the behavior of electrochemical cells under different conditions and to optimize the performance of batteries and fuel cells.
| 5. Can the Nernst equation be applied to all electrochemical cells? | |
Ans. The Nernst equation is applicable to most electrochemical cells, as long as the reaction is a redox reaction involving ions. However, there are some limitations. It assumes that the system is at equilibrium, and it may not accurately predict the behavior of cells with high current densities or complex reactions. Additionally, it does not account for factors such as resistance, polarization, and kinetic limitations, which may affect the actual potential of the cell.
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