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JAMB Chemistry 2024 Paper

Question : 96

Total: 138

^{3+}

Solution:

Concept:

The discharge of

\mathrm{Al}^{3+}

ions requires 3 moles of electrons per mole of aluminium atoms.

Explanation:

The cathode reaction is written as:

\mathrm{Al}^{3+} + 3e^- \rightarrow \mathrm{Al}

From this equation, 1 mole of

\mathrm{Al}^{3+}

needs 3 moles of electrons.

Since 1 mole of electrons carries a charge of 1 Faraday (

1\,\mathrm{F}

), 1 mole of

\mathrm{Al}^{3+}

requires

3\,\mathrm{F}

Therefore, 4.5 moles of

\mathrm{Al}^{3+}

requires:

4.5 \times 3 = 13.5\,\mathrm{F}

Answer:

The correct option is A.

13.5\,\mathrm{F}

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