The standard reduction potentials of Cu²⁺(aq) |Cu(s) and Ag⁺(aq) |Ag(s) are +0.34 and+0.80 V, respectively. Determine the value of the actual cell potential, E_cell, (in V) for the following cell at 25.0 °C.
Cu(s) |Cu²⁺(0.250 M) ||Ag⁺(0.0010 M) |Ag(s) Hint: First calculate E°, then apply the solution concentrations of the galvanic cell using the Nernst equation.

Question

Quizplus · Accepted Answer

The correct answer is A because the actual cell potential, Ecell, can be calculated using the Nernst equation:Ecell = E° - (RT/nF)ln(Q)where E° is the standard cell potential, R is the gas constant (8.314 J/mol·K), T is the temperature in Kelvin (25.0 °C = 298 K), n is the number of electrons transferred in the balanced cell reaction (2 in this case), F is the Faraday constant (96,485 C/mol), and Q is the reaction quotient.The reaction quotient is calculated as follows:Q = [Cu2+]/[Ag+] = (0.250 M)/(0.0010 M) = 250Substituting these values into the Nernst equation, we get:Ecell = +0.34 V - (8.314 J/mol·K * 298 K / (2 * 96,485 C/mol)) * ln(250) = +0.30 VTherefore, the actual cell potential, Ecell, is +0.30 V.

The Standard Reduction Potentials of Cu2+(aq)|Cu(s)and Ag+(aq)|Ag(s)are +0

The Standard Reduction Potentials of Cu²⁺(aq)|Cu(s)and Ag⁺(aq)|Ag(s)are +0