In a classroom demonstration of a redox reaction, Professor Smith set up a voltaic cell with a copper metal anode and a silver metal cathode. The two electrodes were in contact with solutions of the corresponding metal ions, Cu²⁺ and Ag⁺. During the illuminating lecture on redox chemistry, the crystals of silver metal deposited on the silver electrode as the copper solution turned a darker blue. The added silver crystals had a mass of 2.68 g after 50.0 minutes of lecture. What was the average current that the cell produced?

Question

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The correct answer is A.The average current can be calculated using Faraday's law of electrolysis:$$I = \frac{m}{Mt}$$where:* I is the current in amperes* m is the mass of the deposited metal in grams* M is the molar mass of the deposited metal in grams per mole* t is the time in secondsIn this case, the deposited metal is silver, which has a molar mass of 107.87 g/mol. The time is 50.0 minutes, which is 3000 seconds. The mass of the deposited silver is 2.68 g.Substituting these values into the equation, we get:$$I = \frac{2.68 g}{107.87 g/mol * 3000 s} = 0.799 A$$Therefore, the average current that the cell produced is 0.799 A.

In a Classroom Demonstration of a Redox Reaction, Professor Smith