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20. Electrochemistry
Cell Potential: The Nernst Equation
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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Cu(s) | Cu2+(aq, 3.2×10^(-3) mol L^-1) || Cu2+(aq, 4.48 mol L^-1) | Cu(s). Given E°(Cu2+/Cu) = +0.34 V, express your answer to two significant figures.
A
+0.41 V
B
+0.34 V
C
+0.27 V
D
+0.20 V
Verified step by step guidance1
Identify the components of the electrochemical cell: The cell consists of two half-cells, both involving the Cu/Cu²⁺ redox couple. The concentrations of Cu²⁺ in the two half-cells are 3.2×10⁻³ mol L⁻¹ and 4.48 mol L⁻¹, respectively.
Use the Nernst equation to calculate the cell potential under non-standard conditions. The Nernst equation is: , where is the reaction quotient.
Calculate the reaction quotient for the cell reaction. Since the reaction involves the transfer of electrons between Cu²⁺ ions, is given by the ratio of the concentrations of Cu²⁺ in the two half-cells: .
Substitute the values into the Nernst equation. Use the given standard cell potential , the temperature (which is ), and the number of electrons transferred . The gas constant is , and the Faraday constant is .
Calculate the cell potential using the Nernst equation and express the answer to two significant figures.
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