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Use the Nernst equation to determine cell potentials at nonstandard conditions; Perform calculations that involve converting between cell potentials, free energy changes, and equilibrium constants
The Nernst equation accurately predicts cell potentials only when the equilibrium quotient term Q is expressed in activities. Ionic activities depart increasingly from concentrations when the latter exceed 10 –4 to 10 –5 M, depending on the sizes and charges of the ions.
Nernst Equation Questions and Answers - Practice questions, MCQs, PYQs, NCERT Questions, Question Bank, Class 11 and Class 12 Questions, NCERT Exemplar Questions, and PDF Questions with answers, solutions, explanations, NCERT reference, and difficulty level in Nernst Equation chemistry.
Nernst Equation at 25 o C. For measurements carried out 298 K, the Nernst equation can be expressed as follows: E = E 0 – 0.0592/n log 10 Q. Therefore, as per the Nernst equation, the overall potential of an electrochemical cell is dependent on the reaction quotient. Derivation of Nernst Equation. Consider a metal in contact with its own salt ...
Use the Nernst equation to determine cell potentials at nonstandard conditions; Perform calculations that involve converting between cell potentials, free energy changes, and equilibrium constants
Use the Nernst equation to determine cell potentials at nonstandard conditions; Perform calculations that involve converting between cell potentials, free energy changes, and equilibrium constants
The equation is E = E° – (RT/nF) × ln(Q), where E is the observed electrode potential, E° is the standard electrode potential, R is the gas constant, T is the temperature in Kelvin, n is the number of electrons transferred in the reaction, F is Faraday’s constant, and ln(Q) is the natural logarithm of the reaction quotient.
The Nernst equation relates the instantaneous potential, E, to the standard potential, E°, and the reaction quotient, Q: E = E° - (0.0592 V/n)logQ at 298 K. When all reactants and products are in their standard states, Q = 1 and E = E°. When the reaction is at equilibrium, Q = K and E = 0.
The Nernst equation is used to calculate the electrochemical cell potential at any known pressure, temperature, and concentration. This equation relates the reduction potential of a cell at a non-standard condition to that at the standard conditions.
Use the Nernst equation to determine cell potentials at nonstandard conditions; Perform calculations that involve converting between cell potentials, free energy changes, and equilibrium constants