Based on Faraday's 1st law of electrolysis,
total electric current passed in AlCl3 = I = Q X T
where Q = electric charge, T = time (in seconds)
Given, Q = 15 A, T = 3.5 h = 3.5 X 60 X 60 s = 12600 s
∴ I = 15 X 12600 = 189000 C
Now, based on Faraday's 2nd law of electrolysis we have,
W = ZIT
where, W= weight of electrolyte deposited/evolved at any electrode
Z= electrochemical equivalent
T= time (s)
I = electric current
in present case, Electrochemical Equivalent of Al =
![\frac{26.98}{3}](https://tex.z-dn.net/?f=%20%5Cfrac%7B26.98%7D%7B3%7D%20)
= 8.993 g and I = 189000 C
∴ W = 8.993 X 189000 X 12600 = 2.141X
![10^{10}](https://tex.z-dn.net/?f=%2010%5E%7B10%7D%20)
g