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18 August, 20:51

A current of 0.15 A is passed through an aqueous solution of K2PtCl4. How long will it take to deposit 1.00 g Pt (s) (M = 195.1) ?

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  1. 18 August, 21:19
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    First calculate the electric charge used to deposit 1.0 g Pt

    C = (1.0 g Pt) (1 mol Pt / 195.1 g Pt) (2 mol e / 1 mol Pt) (96485 C / 1 mol e)

    C = 989.08 C

    C = It

    Where I is the current

    T is the time

    T = C / i

    T = 989.08 C / 0.15 A

    T = 6593.88 s

    T = 1.83 hrs
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