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Electrolysis and Faraday's Law

AP Chemistry· difficulty 4/5

A current of 2.50 A is passed through molten AlCl3AlCl_3 for 3.00 hours. What mass of Al is deposited? (F = 96485 C/mol; M(Al) = 26.98)

  • A

    0.840.84 g

  • B

    2.522.52 g

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  • C

    5.045.04 g

  • D

    7.557.55 g

Explanation

Charge = It = (2.50)(10800) = 27000 C. Mol e−^- = 27000/96485 = 0.2798. Al3++3e−→AlAl^{3+} + 3e^- \rightarrow Al: mol Al = 0.2798/3 = 0.0933. Mass = 0.0933×\times26.98 = 2.52 g.

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