To calculate the resistance of the cell, we need to know the current flowing through the cell. However, the information provided does not give us the current directly. In an electrochemical cell, the potential difference voltage is related to the Gibbs free energy change G and the number of moles of electrons transferred n in the redox reaction, as well as the Faraday constant F :G = -nFEThe Nernst equation can be used to determine the potential difference E in the cell based on the concentrations of the species involved:E = E - RT/nF * ln Q Where E is the standard potential difference, 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-copper II sulfate cell, the standard potential difference E is 0 V, as both electrodes are made of copper. The reaction quotient Q can be calculated as the ratio of the concentrations of the products and reactants. In this case, the concentration of copper II sulfate is 0.1 M, and the concentration of copper is 1 since it is a solid :Q = [Cu]/[Cu] = 0.1/1 = 0.1Now we can plug the values into the Nernst equation:E = 0 - 8.314 J/molK * 298 K / 2 * 96485 C/mol * ln 0.1 E -0.0295 VHowever, the student measures a potential difference of 0.54 V, which is significantly higher than the calculated value. This suggests that there is an additional potential difference due to the resistance in the cell. To find the resistance, we need to determine the current flowing through the cell.Unfortunately, we cannot determine the current or the resistance with the given information. We would need additional data, such as the current flowing through the cell or the rate of the redox reaction, to calculate the resistance using Ohm's law V = IR .