The electrolysis of molten alcl3 for 3.25 hr with an electrical current of 15.0 a produces g of aluminum metal.

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 =  = 8.993 g and I = 189000 C
∴ W = 8.993 X 189000 X 12600 = 2.141X  g

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