Electrochemistry Basics - Numerical Applications
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Q. Calculate the Gibbs free energy change (ΔG) for a cell with E° = 0.75 V and n = 2 moles of electrons transferred.
Q. For a redox reaction with E° = 0.45 V and n = 3, what is the maximum work (W) obtainable from the reaction if 1 mole of reactants is used?
Q. If the concentration of Cu²⁺ in a cell is 0.01 M and the standard reduction potential is +0.34 V, what is the cell potential at 25°C using the Nernst equation?
Q. If the standard reduction potential for the half-reaction Fe³⁺ + 3e⁻ → Fe is +0.77 V, what is the potential when [Fe³⁺] = 0.001 M?
Q. In a concentration cell with Ag⁺ at 0.1 M and Ag⁺ at 1 M, what is the cell potential at 25°C?
Q. What is the effect of increasing the temperature on the cell potential of an electrochemical cell?
Q. What is the equilibrium constant (K) for a reaction with ΔG° = -40 kJ at 298 K?
Q. What is the Nernst equation for a half-reaction involving 2 electrons at 25°C?
Q. What is the pH of a solution where the concentration of H⁺ ions is 1.0 x 10⁻⁷ M?
Q. What is the standard cell potential (E°) for a galvanic cell with half-reactions: Zn²⁺ + 2e⁻ → Zn (E° = -0.76 V) and Cu²⁺ + 2e⁻ → Cu (E° = +0.34 V)?
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