The overall reaction for the electrolytic production of aluminium by means of the Hall Heroult process may be represented as $\mathrm{Al_2O}_3(\mathrm{s})+3 \mathrm{C}(\mathrm{s}) \longrightarrow 2 \mathrm{Al}(\mathrm{s})+3 \mathrm{CO}(\mathrm{g})$ At $1000^{\circ} \mathrm{C}$, the standard free energy change for the process is $-594 \mathrm{~kJ} \mathrm{~mol}^{-1}$. The minimum voltage required to produce one mole aluminium at this temperature is

NEET UG CHEMISTRY MCQ: GENERAL PRINCIPLES AND PROCESSES OF ISOLATION OF ELEMENTS

1 Hard

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The overall reaction for the electrolytic production of aluminium by means of the Hall Heroult process may be represented as

\mathrm{Al_2O}_3(\mathrm{s})+3 \mathrm{C}(\mathrm{s}) \longrightarrow 2 \mathrm{Al}(\mathrm{s})+3 \mathrm{CO}(\mathrm{g})

1000^{\circ} \mathrm{C}

, the standard free energy change for the process is

-594 \mathrm{~kJ} \mathrm{~mol}^{-1}

. The minimum voltage required to produce one mole aluminium at this temperature is

View answer and explanation

Correct option: A

1.02 \mathrm{~V}

Option A (1.02 V) is correct because it is calculated using the formula

\Delta G = -nFE

, where n is the number of moles of electrons transferred, F is Faraday's constant, and E is the cell potential.

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