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^-19C. A) 3.96 g B) 2.52 g C) 0.99 g D) 2 .52 g E) 1.98 g

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Quizplus · Accepted Answer

The mass of copper deposited can be calculated using the formula: mass = (current × time × molar mass) / (n × F), where n is the number of electrons (2 for Cu²⁺) and F is Faraday's constant (96485 C/mol). Substituting the given values, the mass is approximately 1.98 g.

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