When some quantity of electricity is passed through $A l C l_{3}$ solution, $5.6$ litres of chlorine is produced at STP. Quantity of $A l$ deposited is:

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4.5

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Solution

The correct option is B 4.5
At anode: $2 C l^{-} \to C l_{2} + 2 e^{-}$
1 Faraday of electricity liberates 0.5 moles of Cl $_{2}$ , which occupies 11.2L at STP.
0.25 moles of Cl $_{2}$ occupying 5.6L at STP is obtained from 0.5 Faradays.
At cathode: $A l^{3 +} + 3 e^{-} \to A l$
1 Faraday deposits 9 g aluminium.
0.5 Faraday deposits 4.5 g aluminium.

Option B is correct.

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When some quantity of electricity is passed through AlCl3 solution, 5.6 litres of chlorine is produced at STP. Quantity of Al deposited is:

When some quantity of electricity is passed through $A l C l_{3}$ solution, $5.6$ litres of chlorine is produced at STP. Quantity of $A l$ deposited is: