A solution of aluminium chloride is electrolysed for 30 minutes using a current of 2 A . The amount of the aluminium deposited at the cathode is ________.
[Given : molar mass of aluminium and chlorine are $27gmo{l}^{-1}$ and $35.5gmo{l}^{-1}$ respectively]

[JEE Main 2025, 22 Jan (Shift 1)]

Question

A solution of aluminium chloride is electrolysed for 30 minutes using a current of 2 A . The amount of the aluminium deposited at the cathode is ________.
[Given : molar mass of aluminium and chlorine are $27gmo{l}^{-1}$ and $35.5gmo{l}^{-1}$ respectively]

[JEE Main 2025, 22 Jan (Shift 1)]

YESPYQ · Accepted Answer

Correct answer: c) 0.336 g. Using Faraday's laws of electrolysis, $W=Z\times I\times t$ Given: $I=2A,t=30min=30\times 60sec$ $∴W=\frac{M}{nF}\times I\times t\left(∵Z=\frac{M}{nF}\right)\ W=\frac{27}{3\times 96500}\times 2\times 30\times 60$ $W=0.336g$

A solution of aluminium chloride is electrolysed for 30 minutes using a current of 2 A . The amount of the aluminium dep…

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