The electrolysis of molten AlCl3 for 2.50 hr with an electrical current of 15.0 A produces ________ g of aluminum metal. Group of answer cho

Question

The electrolysis of molten AlCl3 for 2.50 hr with an electrical current of 15.0 A produces ________ g of aluminum metal. Group of answer choices

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Thiên Hương 3 years 2021-07-29T01:36:16+00:00 1 Answers 520 views 0

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    2021-07-29T01:37:26+00:00

    Answer:

    The correct answer is 12.58 grams.

    Explanation:

    Based on the given information, the electrolysis equation will be,

    Al³⁺ + 3e⁻ ⇔ Al

    1 mol of Al needs 3 moles of electron, and the value for 1 mole of electron is 96485 C.

    Thus, 1 mole of Al needs 3 × 96485 C = 289455 C

    Now the amount of charge passed is,

    T = 2.5 hours

    = 2.5 × 3600 s = 9 × 10³ s

    Q = Current × Time

    = 15A × 9 × 10³ s

    = 13.5 × 10⁴ C

    The moles of Al plated will be,

    = 13.5 × 10⁴ / 289455

    = 0.4664 mol

    The molecular mass of Al is 26.98 grams per mole

    Now the mass of Al will be,

    = Number of moles × Molecular mass

    = 0.4664 × 26.98

    = 12.58 grams

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