33. A direct current of 0.1 A is passed for 2 hours through a solution of cuprocyanide (), resulting in the deposition of 0.3745 g of Copper at the cathode. Calculate the exact industrial current effi

Question

33. A direct current of 0.1 A is passed for 2 hours through a solution of cuprocyanide ($[Cu(CN)_2]^-$), resulting in the deposition of 0.3745 g of Copper at the cathode. Calculate the exact industrial current efficiency. (Atomic mass Cu = 63.5)

Prashant Kotian · Accepted Answer

Correct answer: C. . Cu is in +1 state. . Theoretical moles = mol. Theoretical mass = . Efficiency = .

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