To calculate the rate of electroplating of copper on a metallic surface, we need to determine the amount of copper deposited during the electroplating process. We can use Faraday's law of electrolysis to do this.Faraday's law states that the amount of substance deposited during electrolysis is directly proportional to the amount of charge passed through the solution. Mathematically, it can be represented as:mass of substance deposited m = current I time t molar mass M / n Faraday's constant F where:- m is the mass of the substance deposited in grams - I is the current in amperes - t is the time in seconds - M is the molar mass of the substance in grams per mole - n is the number of electrons involved in the redox reaction in moles - F is Faraday's constant 96500 C/mol First, we need to determine the number of electrons involved in the reduction reaction of Cu to Cu. The balanced half-reaction is:Cu + 2e CuSo, n = 2 moles of electrons are involved in the reaction.Next, we need to convert the time from hours to seconds:3 hours 3600 seconds/hour = 10800 secondsNow, we can use Faraday's law to calculate the mass of copper deposited:m = I t M / n F m = 2.5 A 10800 s 63.55 g/mol / 2 mol 96500 C/mol m = 2.5 10800 63.55 / 2 96500 m 45.6 gSo, 45.6 grams of copper are deposited on the metallic surface during the electroplating process.To calculate the rate of electroplating, we can divide the mass of copper deposited by the total time:rate of electroplating = mass of copper deposited / timerate of electroplating = 45.6 g / 3 hoursrate of electroplating 15.2 g/hourTherefore, the rate of electroplating of copper on the metallic surface is approximately 15.2 grams per hour.