An industrial electrolytic process for producing aluminum uses the reactions shown in the following equations.Anode (oxidation): C(s) + 2 O^2- (aq) -gt; CO2(g) + 4e- (electrons)Cathode (reduction): Al3+ (l) + 3e- -gt; 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?
Start of with a good allroundersee link below and a tripod, once you master the technical stuff through a class or good reading (been to the library lately?) then in a year or two when you've seen your results and had a chance to save some $$$ you might consider advancing to a DSLR.
a college course perhaps at evening classes will teach you the technicals a simple camera/lens combination will be enough to get you thru this basic courseyou should then be in a position after the course to decide what further equipment you need
24 x 5.00120 g moles Al 120 g/ 26.9815 g/mol4.45 4.45 ( 3 faradays/1 mol) 13.4 faradays 13.4 faradays x 96500 coulombs/ faraday 1.29 x 10^6 coulombs 5.00 x 10^4 x 91.1 /100 45550 ampere 1.29 x 10^6 coulombs / 45550 28.3 s moles Zn 40.0 / 65.39 g/mol0.612 the half reaction is : Zn2+ + 2e- Zn 0.612 ( 2 faradays/1mol) 1.24 faradays 1.24 x 965001.18 x 10^5 coulombs 3 hours 10800 s current 1.18 x 10^5 / 10800 s 10.9 ampere
