9) Which of the following(s) is/are correct for the following cell? Cd^+2(0.25M)vert Cd(s)Vert Cu^+2(0.45M)vert Cu(s) (E^circ Cu^+2/Cu=0.337V;E^circ Cu^+2/Cd=-0.403V) I- The cell type is an electrolytic cell II- Cell Voltage is -0.421V III- The Free energy of the reaction is -144.25kJ A) I and II B) I and III C II and III D)Only I Only III

To determine which statements are correct for the given cell, we need to analyze the cell notation and the provided standard reduction potentials.The given cell notation is: I- The cell type is an electrolytic cell.This statement is incorrect. The given cell is a galvanic (or voltaic) cell, not an electrolytic cell. In a galvanic cell, the spontaneous redox reaction generates an electric current.II- Cell Voltage is .To calculate the cell voltage, we can use the Nernst equation: Where: is the standard cell potential, which can be calculated using the standard reduction potentials: is the number of moles of electrons transferred, which is 2 in this case (since and both involve a 2-electron transfer). is the reaction quotient, which can be calculated as: Substituting the values into the Nernst equation: Therefore, the cell voltage is not , so statement II is incorrect.III- The Free energy of the reaction is .To calculate the free energy of the reaction, we can use the formula: Where: is the number of moles of electrons transferred, which is 2 in this case. is the Faraday constant, which is approximately . is the cell voltage, which we calculated as .Substituting the values into the formula: Therefore, the free energy of the reaction is not , so statement III is incorrect.Based on the analysis, none of the statements I, II, or III are correct. Therefore, the correct answer is D) Only III.