- #1
gymstar
- 3
- 0
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?
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?