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6 January, 21:25

1. 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 40.0 minutes?

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  1. 6 January, 21:50
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    ion with charge 3⁺, like Cr³⁺ needs 3 Faradays to plate 1 mole

    Amount of electric charge per mole (faraday's constant) = 96500 C mol¹⁻

    Time = 40min = 2400 sec

    you have coulombs = amps x sec = 8 x 2400 coulombs

    molar mass of Cr = 51.9961g

    96500 x 3 coulombs plates 51.9961g Cr

    so 8 x 2400 coulombs gives,

    51.9961 / (96500 x 3) x 8 x 2400 g Cr = 3.45g Cr

    so, 3.45g chromium metal is plated out.
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