Calculate the cell potential at 25 °C for the following overall reaction. Zn²⁺(aq) + 2 Fe²⁺(aq) → Zn(s) + 2 Fe³⁺(aq)
[Zn²⁺] = 1.50 × 10^-4 M,[Fe³⁺] = 0.0200 M,and [Fe²⁺] = 0.0100 M.The standard reduction potentials are as follows:
Zn²⁺(aq) + 2 e^- → Zn(s)
E° = -0.763 V
Fe³⁺(aq) + e^- → Fe²⁺(aq)
E° = +0.771 V

Question

Quizplus · Accepted Answer

The correct answer is A because the cell potential is calculated using the Nernst equation:E = E° - (RT/nF)ln(Q)where E is the cell potential, E° is the standard cell potential, R is the gas constant (8.314 J/mol·K), T is the temperature in Kelvin (298 K), n is the number of electrons transferred (2 in this case), F is the Faraday constant (96,485 C/mol), and Q is the reaction quotient.The reaction quotient is calculated using the concentrations of the reactants and products:Q = [Fe3+]/[Fe2+]^2[Zn2+]Substituting the given values into the Nernst equation, we get:E = -0.763 V - (8.314 J/mol·K * 298 K / 2 * 96,485 C/mol)ln(0.0200 M / (0.0100 M)^2 * 1.50 × 10^-4 M)E = -0.763 V - (-0.0592 V/n)ln(3.00 × 10^3)E = -0.763 V + 0.895 VE = -1.665 VTherefore, the cell potential at 25 °C for the given overall reaction is -1.665 V.

Calculate the Cell Potential at 25 °C for the Following