Answer:
A=[tex]3.5 x10^3 s[/tex]
Step-by-step explanation:
- Write the electrolysis reaction for Al
[tex]Al^+^3 +3e^- -----> Al[/tex]
- Find moles of Al using the molecular weight of Aluminum (26.981 g/mol)
[tex]4 g Al (\frac{1 mol Al}{26.981 g Al}) =0.148 mol Al[/tex]
- Calculate moles of charge using the relation of the electrolysis reaction.
[tex]1 mol Al -----> 3 mol (e^-)[/tex]
[tex]0.148 mol Al(\frac{3 mol e^-}{1 mol Al} )=0.444 mol (e^-)[/tex]
- Using Faraday's Constant to calculate the quantity of electricity (Coulombs)
[tex]0.444 mol (e^-)(\frac{96500 C}{1 mol (e^-)} )=42846 C[/tex]
- Finally, you can obtain the seconds using electrical current of 12 A (12 C/s)
[tex]42846 C (\frac{1 s}{12 C} )=3570.5 s=3.57x10^3 s[/tex]
