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Electrolysis and Faraday's Law

AP Chemistry· difficulty 4/5

A 2.00 A current passes through molten CuCl₂ for 30.0 minutes. (F = 96485 C/mol e⁻)

I = 2.00 A, t = 30.0 min = 1800 s Cu²⁺ + 2 e⁻ → Cu Find mass Cu deposited

What mass of Cu is deposited?

  • A

    2.36 g

  • B

    0.30 g

  • C

    0.59 g

  • D

    1.18 g

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Explanation

Q = It = 2.00·1800 = 3600 C. mol e⁻ = 3600/96485 = 0.0373. mol Cu = 0.0373/2 = 0.01867. mass = 0.01867·63.55 = 1.186 g.

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