Answer to Question #118969 in Inorganic Chemistry for Shania kumar

Question #118969
In a certain electrolysis experiment involving Al3+ ions, 60.2 g of Al was recovered when a current of 0.352 A was used. How many minutes did the electrolysis last?
[Faraday constant = 96500 C/mol]
1
Expert's answer
2020-06-03T13:33:52-0400

Atomic weight of Al = 27

Reaction: Al⁺³ + 3e = Al

3 moles of electron is required by 1 mole of Al

Proportion:

(3 moles×96500 C/mol) of charge – for 27 g of Al

x of charge – for 60.2 g of Al

x = 645.47×10³ C – charge required

Charge = Current×time

Time = charge/current = (645.47×10³ C) / (0.352 A) =1833×10³ s = 30.55×10³ min

Answer: 30.55×10³ min

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Comments

Assignment Expert
05.06.20, 14:55

Dear Shania kumar, an answer is published

Shania kumar
03.06.20, 06:40

By when will the answer be published

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