Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C:
$\quad$ $\quad$ $\quad$ Sn(s) | Sn²⁺(aq,0.022 mol L^-1) $\|$ Ag⁺(aq,2.7 mol L^-1) | Ag(s)
E°(Sn²⁺/Sn) = -0.14 V and E°(Ag⁺/Ag) = +0.80 V

Question

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C:

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Sn(s) | Sn²⁺(aq,0.022 mol L^-1)

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Ag⁺(aq,2.7 mol L^-1) | Ag(s)
E°(Sn²⁺/Sn) = -0.14 V and E°(Ag⁺/Ag) = +0.80 V

Quizplus · Accepted Answer

The cell potential is calculated using the Nernst equation. The standard cell potential (E°cell) is the difference between the standard reduction potentials of the cathode and anode: E°cell = E°(Ag⁺/Ag) - E°(Sn²⁺/Sn) = 0.80 V - (-0.14 V) = 0.94 V. The reaction quotient Q = [Sn²⁺]/[Ag⁺]² = 0.022/(2.7)². Using the Nernst equation, Ecell = E°cell - (RT/nF)ln(Q), where n = 2, R = 8.314 J/mol·K, T = 298 K, and F = 96485 C/mol. Calculating gives Ecell ≈ 1.01 V.

Calculate the Cell Potential for the Following Reaction That Takes \quad

Calculate the Cell Potential for the Following Reaction That Takes $\quad$