Can someone please explain how to tackle this problem?

Cu - Anode electrode
Zn - Cathode electrode

A current of 2 amps is sustained for 16 minutes. what mass of Cu(s) is deposited on the zinc electrode? (Faradays' constant: 96500 C/mol e-)

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  1. Coulombs = amperes x seconds.
    C = 2 x 16 x 60 = 1,920
    For every (63.55/2) g Cu plated it requires 96,500 C. So
    (63.55/2) x (1920 C/96,500 C) = ?g Cu plated.

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  2. Thank you

    Just one more question

    Why is it (63.55/2) g Cu ?

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