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)1.52 g E)1.98 g

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The mass of copper deposited can be calculated using Faraday's laws of electrolysis. First, calculate the total charge passed: Q = I × t = 10 A × 600 s = 6000 C. The number of moles of electrons is Q / (F), where F (Faraday's constant) = 96485 C/mol. So, moles of electrons = 6000 / 96485. Since copper has a charge of +2, it requires 2 moles of electrons to deposit 1 mole of copper. Therefore, moles of copper = (6000 / 96485) / 2. Finally, mass of copper = moles of copper × atomic weight = (6000 / 96485 / 2) × 63.6 g/mol = 1.98 g.

In an Electroplating Process,copper (Ionic Charge +2e,atomic Weight 63