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 $27 \mathrm{~g} \mathrm{~mol}^{-1}$ and $35.5 \mathrm{~g} \mathrm{~mol}^{-1}$ respectively. Faraday constant $\left.=96500 \mathrm{Cmol}^{-1}\right]$
Select the correct option:
A
0.336 b
B
1.007 g
C
0.441 g
D
1.660 g
✓ Correct! Well done.
✗ Incorrect. Try again or view the solution.
Solution
gm equivalent of Al deposited =$\frac{\mathrm{It}}{96500}$
$\frac{\mathrm{w}}{27} \times 3=\frac{2 \times 30 \times 60}{96500}$ ; $\mathrm{w}=0.336 \mathrm{~g}$
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