To calculate the resistance of the electrochemical cell, we first need to determine the cell potential E_cell using the Nernst equation. The Nernst equation is given by:E_cell = E_cell - RT/nF * ln Q where:E_cell = standard cell potentialR = gas constant 8.314 J/molK T = temperature in Kelvin 25C = 298.15 K n = number of electrons transferred in the redox reactionF = Faraday's constant 96485 C/mol Q = reaction quotientFirst, we need to find the standard cell potential E_cell . This can be calculated by subtracting the standard reduction potential of the anode from the standard reduction potential of the cathode:E_cell = E_cathode - E_anodeE_cell = 0.40 V - -1.36 V E_cell = 1.76 VNext, we need to determine the number of electrons transferred in the redox reaction n . In this case, both Cu and Zn are involved in a two-electron transfer process:Cu + 2e Cu reduction Zn Zn + 2e oxidation So, n = 2.Now, we need to calculate the reaction quotient Q . The reaction quotient is given by:Q = [Zn]/[Cu]Using the given concentrations of CuSO and ZnSO:Q = 0.01 M / 0.1 M Q = 0.1Now we can plug all the values into the Nernst equation:E_cell = 1.76 V - 8.314 J/molK * 298.15 K / 2 * 96485 C/mol * ln 0.1 E_cell 1.76 V - 0.0296 VE_cell 1.7304 VNow that we have the cell potential, we can calculate the resistance of the electrochemical cell using Ohm's law:V = IRwhere:V = voltage E_cell I = currentR = resistanceIn this case, we don't have the current I value. However, we can still express the resistance R in terms of the cell potential E_cell and current I :R = V/IR = E_cell/IWithout the current value, we cannot calculate the exact resistance of the electrochemical cell. However, we have determined the cell potential E_cell to be approximately 1.7304 V, which can be used to calculate the resistance once the current value is known.