Hi i am confused about on how to solve this question. The question asks: By the electrolysis of water, 11.2L oxygen at STP was prepared. a) What charge was required? b) if a current of 0.05A was used, how long did it take? I have done the question but i think i did it wrong. 2H2O(l) ---> O2(g) + 4H +(aq) + 4e- (oxidation) 4H +(aq) + 4e- ---> 2H2O(g) (reduction) a) 1mol/22.4L = 0.0446 0.0446* 96500= 4303.9 4.3* 10^3 b) 0.5A = 4.3* 10^3/t 4.3*10^3/0.5A t = 8607.8s Is this completely wrong????