In an electroplating process, copper (ionic charge +2e, atomic weight 63.6 g/mol) is deposited using a current of 10.0 A. What mass of copper is deposited in 10.0 minutes? Avogadro's number is 6.022 × 10²³ molecules/mol and e = 1.60 × 10^-19 C. A) 3.96 g B) 2.52 g C) 0.99 g D) 2.520 g E) 1.98 g

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Quizplus · Accepted Answer

The mass of copper deposited can be calculated using Faraday's laws of electrolysis. The charge passed is 10 A × 600 s = 6000 C. The number of moles of electrons is 6000 C / (2 × 1.60 × 10^-19 C/electron) / 6.022 × 10^23 electrons/mol = 0.03125 mol. The mass of copper deposited is 0.03125 mol × 63.6 g/mol = 1.98 g.

In an Electroplating Process, Copper (Ionic Charge +2e, Atomic Weight