A voltaic cell consists of a Hg/Hg₂²⁺ electrode (E°= 0.85 V) and a Sn/Sn²⁺ electrode (E°= -0.14 V). Calculate [Sn²⁺] if [Hg₂²⁺] = 0.24 M and E_cell = 1.04 V at 25°C.

Question

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The Nernst equation can be used to calculate the concentration of Sn²⁺: E = E° - (RT/nF) * ln(Q) where E is the cell potential, E° is the standard cell potential, R is the gas constant, T is the temperature, n is the number of electrons transferred in the balanced equation, F is Faraday's constant, and Q is the reaction quotient. For this cell, the balanced equation is: Hg₂²⁺ + Sn²⁺ → Hg + Sn₂²⁺ and the reaction quotient is: Q = [Sn²⁺] / [Hg₂²⁺] Substituting the given values into the Nernst equation, we get: 1.04 V = (0.85 V - (-0.14 V)) - (8.314 J/mol∙K * 298 K / (2 * 96485 C/mol)) * ln([Sn²⁺] / 0.24 M) Solving for [Sn²⁺], we get: [Sn²⁺] = 0.0049 M Therefore, the best answer is C, with the concentration of Sn²⁺ being 0.0049 M.

A Voltaic Cell Consists of a Hg/Hg22+ Electrode (E°= 0

A Voltaic Cell Consists of a Hg/Hg₂²⁺ Electrode (E°= 0