A concentration cell is constructed with copper electrodes and Cu²⁺ in each compartment.In one compartment,the [Cu²⁺] = 1.0 $\times$ 10^-³ M and in the other compartment,the [Cu²⁺] = 2.0 M.Calculate the potential for this cell at 25°C.The standard reduction potential for Cu²⁺ is +0.34 V.

Question

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The Nernst equation is used to calculate the potential of a concentration cell: E = E° - (RT/nF) * ln(Q), where E° is the standard reduction potential, R is the gas constant, T is the temperature in Kelvin, n is the number of moles of electrons transferred, F is the Faraday constant, and Q is the reaction quotient. For a copper concentration cell with Cu^2+ ions, E° = 0.34 V, n = 2 (since Cu^2+ gains 2 electrons to become Cu), and Q = [Cu^2+]cathode/[Cu^2+]anode. At 25°C (298 K), and given concentrations, the potential can be calculated. The fact that the potential is positive (0.098 V) indicates a spontaneous reaction in the direction written.

A Concentration Cell Is Constructed with Copper Electrodes and Cu2+ ×\times×

A Concentration Cell Is Constructed with Copper Electrodes and Cu²⁺ $\times$