Question

A solution of aluminium chloride is electrolyzed for 30 minutes using a current of 2A. The amount of the aluminium deposited at the cathode is ____ .
[Given: molar mass of aluminium and chlorine are 27 g mol\(^{-1}\) and 35.5 g mol\(^{-1}\) respectively, Faraday constant = 96500 C mol\(^{-1}\)]

• A. 1.660 g
• B. 1.007 g
• C. 0.336 g
• D. 0.441 g

Hint:

To find the amount of substance deposited during electrolysis, use the formula \( w = \frac{It}{96500} \times \frac{M}{n} \), where \( M \) is the molar mass and \( n \) is the valency.

Answer 1

The Correct Option is C

The gram equivalent of Al deposited is given by: \[ w = \frac{I t}{96500} \times \frac{27}{3} \] where \( I = 2 \, \text{A}, \, t = 30 \times 60 \, \text{s} \). Substituting the values: \[ w = \frac{2 \times 30 \times 60}{96500} \times \frac{27}{3} = 0.336 \, \text{g} \] Thus, the correct answer is \( \boxed{0.336 \, \text{g}} \).