...in the following equations.? An industrial electrolytic process for producing aluminum uses the reactions shown in the following equations.
Anode (oxidation): C(s) + 2 O^2- (aq) -----> CO2(g) + 4e- (electrons)
Cathode (reduction): Al3+ (l) + 3e- ------> Al(s)
a) How long would it take to produce enough aluminum to make a case (24 cans) of aluminum soft drink cans if each can used 5.00 g of aluminum, a current of 5.00 x 10^4 A was employed, and the current efficiency was 91.1%?
3a) What current would be needed to electroplate 40.0 g of zinc in exactly 3 hours from a solution of zinc nitrate?
Anode (oxidation): C(s) + 2 O^2- (aq) -----> CO2(g) + 4e- (electrons)
Cathode (reduction): Al3+ (l) + 3e- ------> Al(s)
a) How long would it take to produce enough aluminum to make a case (24 cans) of aluminum soft drink cans if each can used 5.00 g of aluminum, a current of 5.00 x 10^4 A was employed, and the current efficiency was 91.1%?
3a) What current would be needed to electroplate 40.0 g of zinc in exactly 3 hours from a solution of zinc nitrate?