Redox Reactions And Electrochemistry Question 478
Question: Aluminium oxide may be electrolysed at $ 1000{}^\circ C $ to furnish aluminium metal (At. Mass = 27 amu; 1 Faraday = 96,500 Coulombs). The cathode reaction is - $ A{l^{3+}}+3{e^{-}}\to Al $ To prepare 5.12 kg of aluminium metal by this method we require electricity of
Options:
A) $ 5.49\times 10^{1}C $
B) $ 5.49\times 10^{4}C $
C) $ 1.83\times 10^{7}C $
D) $ 5.49\times 10^{7}C $
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Answer:
Correct Answer: D
Solution:
[d] 1 mole of $ {e^{-}}=1F=96500C $ 27g of Al is deposited by $ 3\times 96500C $ 5120 g of Al will be deposited by $ =\frac{3\times 96500\times 5120}{27}=5.49\times 10^{7}C $
BETA
