Question

How many
** minutes** will it take to
electroplate 0.334 grams of copper metal, Cu(s), from a solution
containing Cu

1 A = 1 C/s

F = 96,500 C/mole electron

Answer #1

**ANSWER:**

Given,

current, I = 3.17 A

weight of copper metal = 0.334 g

atomic mass of copper metal = 63.5 g/mol

number of moles of copper metal = (0.334 g)/(63.5 g/mol) = 0.00526 mol

1 mole of copper releases = 2 mole electrons

0.00526 moles of copper releases = 0.01052 moles electrons

Faradays constant, F =96500 C/mole electron

From electrochemistry:

Q = I x t = nF

where,

Q = charge

I = current

t = time

n = moles of electrons

F = faradays constant

Q = 3.17 C/s x t = 0.01052 mole electron x 96500 C/mole electron

**time, t = 320.24 s = 5.34
min**

**Hence, 5.34 minutes will take to electroplate 0.334
grams of copper metal, Cu(s), from a solution containing
Cu ^{2+}(aq) with a current of 3.17 A.**

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