A current of 0.80 A was applied to an electrolytic cell containing molten CdCl₂ for 2.5 hours.Calculate the mass of cadmium metal deposited.

Question

Quizplus · Accepted Answer

The mass of cadmium metal deposited can be calculated using Faraday's law of electrolysis:m = (ItM)/nFwhere:m is the mass of the metal deposited (in grams)I is the current (in amperes)t is the time (in seconds)M is the molar mass of the metal (in grams per mole)n is the number of electrons transferred per metal ionF is the Faraday constant (96,485 coulombs per mole)In this case, we have:I = 0.80 At = 2.5 hours = 9000 sM = 112.41 g/moln = 2 (Cd2+ + 2e- -> Cd)F = 96,485 C/molSubstituting these values into the equation, we get:m = (0.80 A * 9000 s * 112.41 g/mol) / (2 * 96,485 C/mol)= 4.2 gTherefore, the mass of cadmium metal deposited is 4.2 g.

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