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13 January, 14:06

Copper is plated onto the cathode of an electrolytic cell containing CuCl2 (aq). How long does it take to plate 145 mg of copper with a current of 3.6 A

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  1. 13 January, 15:22
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    122 seconds

    Explanation:

    Cu{2+} + 2 e{-} → Cu

    the stoichiometric relationships between miles of the electron and the moles of

    Cu is 2 mol e - : 1 mol Cu

    you are given copper mass (145 mg) and current (3.6 A).

    Remember that,

    1A = 1C/s, 1g = 1000 mg and molar mass of Cu = 63.55 g/mol

    145 mg = 0.145 g

    = (0.145 g Cu) / (63.55 g Cu/mol) x (2 mol e{-} / 1 mol Cu) x (9.64853399 x 10^4 C/mol e{-}) / (3.6 A)

    = 0.00228 x 2 x 26777.7

    = 122 seconds
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