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14 November, 17:24

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr3 + ions for 320. minutes?

A) 27.6 g

B) 49.2 g

C) 82.4 g

D) 248 g

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  1. 14 November, 17:52
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    A) m = 27.6 g

    Explanation:

    Faraday's law:

    ∴ mass of the substance produced at the electrode (g):

    m = Q/F. M/z

    ∴ Q = I*t

    ⇒ Q = (8.00 A) (320 min) (60s/min) = 153600 A, s = 153600 C

    ∴ F = 96485.3365 C/mol ... Faraday's constant

    ∴ z = 3 ... valence number

    ∴ M Cr = 51.9961 g/mol ... molar mass

    ⇒ m = ((153600 C) / (96485.3365 C/mol)) ((51.9961 g/mol) / (3))

    ⇒ m = 27.592 g ≅ 27.6 g
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