To find the mass of silver metal deposited, we can use Faraday's laws of electrolysis. First, we need to find the total charge passed through the molten silver chloride.Total charge Q = Current I Time t Q = 2.5 A 5 h 3600 s/h = 45000 C Coulombs Now, we need to find the number of moles of electrons n passed through the molten silver chloride using Faraday's constant F = 96485 C/mol .n = Q / Fn = 45000 C / 96485 C/mol 0.466 mol of electronsThe balanced half-reaction for the reduction of silver chloride is:AgCl + e Ag + ClFrom the balanced half-reaction, we can see that 1 mole of electrons reduces 1 mole of silver ions Ag to 1 mole of silver metal Ag . Therefore, the number of moles of silver metal deposited is equal to the number of moles of electrons passed through the molten silver chloride.Moles of silver metal = 0.466 molNow, we can find the mass of silver metal deposited using the atomic mass of silver 107.87 g/mol .Mass of silver metal = Moles of silver metal Atomic mass of silverMass of silver metal = 0.466 mol 107.87 g/mol 50.25 gSo, approximately 50.25 grams of silver metal will be deposited.