The current involved is 44.7 A
What is the current required?
In an electrolytic reaction, we have the situation in which one specie is oxidized and the other specie is reduced in the electrochemical reaction. We have the reaction that occurs as;
2Cl^-(aq) ------> Cl2(g) + 2e
Now;
If 2 * 96500 C liberates 22.4 dm^3 of Cl2
x C liberates 20dm³ of chlorine gas at STP
x = 2 * 96500 C * 20dm³/24 dm³
x = 160833.33 C
Now
Q = It
Q = quantity of electricity
I = current
t = time = 1 hour or 3600 s
I = Q/t = 160833.33 C/ 3600 s
I = 44.7 A
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