To calculate the mass of silver deposited onto the cathode, we can use Faraday's law of electrolysis. First, we need to find the total charge passed through the solution.Total charge Q = Current I Time t Time needs to be converted to seconds: 20 minutes 60 seconds/minute = 1200 secondsQ = 2.5 A 1200 s = 3000 CNow, we need to find the number of moles of electrons n transferred during the electrolysis process.n = Q / Faraday constantn = 3000 C / 96,485 C/mol = 0.0311 molSince the reaction for the deposition of silver is Ag+ + e- Ag, one mole of electrons deposits one mole of silver. Therefore, the number of moles of silver deposited is equal to the number of moles of electrons transferred.Moles of silver deposited = 0.0311 molNow, we can find the mass of silver deposited using the molar mass of silver.Mass of silver deposited = Moles of silver deposited Molar mass of silverMass of silver deposited = 0.0311 mol 107.868 g/mol = 3.355 gSo, 3.355 grams of silver will be deposited onto the cathode during the electrolysis of the silver nitrate solution using a current of 2.5 A for 20 minutes.