Current: 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.

Question

Quizplus · Accepted Answer

First, we need to calculate the amount of charge that passes through the electroplating cell in 10.0 minutes:

Q = I*t = (10.0 A)(10.0 min)(60 s/min) = 6,000 C

Next, we can use the Faraday's law of electrolysis to calculate the amount of copper deposited:

moles of Cu = Q/(n*F)

where n is the number of electrons transferred (in this case, n = 2 because Cu has a charge of +2e), and F is the Faraday constant, which is equal to 96,485 C/mol e-. Therefore,

moles of Cu = 6,000 C/(2*96,485 C/mol e-) = 0.0311 mol

Finally, we can convert moles of Cu to mass using its molar mass:

mass of Cu = moles of Cu * molar mass = 0.0311 mol * 63.6 g/mol = 1.98 g

Therefore, the answer is E) 1.98 g.

Current: in an Electroplating Process, Copper (Ionic Charge +2e, Atomic