To determine the rate of the electrochemical reaction, we need to consider the stoichiometry of the reaction and the number of electrons transferred in the reaction. The balanced redox reaction between Zinc and Copper in a galvanic cell is:Zn s + Cu aq Zn aq + Cu s In this reaction, Zinc loses 2 electrons oxidation and Copper gains 2 electrons reduction . The number of electrons transferred, n, is 2.Now, we can use Faraday's law of electrolysis to determine the rate of the reaction:rate = current * time / n * Faraday's constant where current is given as 0.50 A, n is 2, and Faraday's constant is approximately 96485 C/mol coulombs per mole of electrons .Since we want to find the rate of the reaction, we can consider the reaction occurring for 1 second time = 1 s to find the rate in moles per second:rate = 0.50 A * 1 s / 2 * 96485 C/mol rate = 0.50 C / 2 * 96485 C/mol rate 2.59 10 mol/sSo, the rate of the electrochemical reaction occurring in the cell is approximately 2.59 10 moles per second.