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14 September, 19:40

What mass of aluminum will be deposited on the cathode if an electric current of 0.15 a is run for 4 5s when a solution of al (no3) 3 is subjected to electrolysis?

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  1. 14 September, 21:21
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    Mass of Al, m = ?

    Molar mass of copper Al, M = 27.0 g/mol

    time, t = 45 s

    current, c = 0.15 A

    valency of Al in Al (NO₃) ₃, z = + 3

    From Faraday's 1st law,

    m = Mct/zF

    where F = Faraday constant = 96500 C/mol

    Substitute all the values,

    m = [ (27.0 g/mol) (0.15 A) (45 s) ] / [3] [96500 C/mol]

    = 6.3 x 10⁻⁴ g

    Mass of aluminium = 6.3 x 10⁻⁴ g

    Therefore, mass of aluminium plated on electrode = 6.3 x 10⁻⁴ g
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