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alisha [4.7K]
3 years ago
11

g Calculate the number of grams of aluminum that is produced in 1.00 h by the electrolysis of molten AlCl3 if the electrical cur

rent is 10.0A.
Chemistry
2 answers:
Mazyrski [523]3 years ago
7 0
the number of grams is 65.9
MatroZZZ [7]3 years ago
5 0

Answer:

3.36 grams Al°(s)  

Explanation:

Given AlCl₃(s), determine the mass (grams) of Al°(s) produced from electrolysis of Aluminum Chloride at 10.0 amps for 1.00 hour.

AlCl₃(s) + 378.3°F (=192.4°C) => Al⁺³(l) + 3Cl⁻(l)

formula wt. Al° = 27g/mol

Faraday Constant (F°) = 96,500 amp·sec

? grams Al°(s) = 10.0amps x (1 mole e⁻/96,500amp-sec) x (1 mole Al°(s)/3 mole e⁻) x (27g Al°(s)/1 mole Al°(s)) x 3,600 sec = 3.36 grams Al°(s)

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