Question

Enter your answer in the provided box. A constant current is passed through an electrolytic cell containing molten MgCl2 for 15 h. If 4.88 L of Cl2 (at STP) is produced at the anode, what is the current in amperes?

Answer 1

   mass of Cl2 produced = PVM/RT

                        = 1*4.88*71/(0.0821*273.15)

                        = 15.45 g

faradays first law

equivalent weight of Cl2 (E)= atwt / charge = 71/2 = 35.5 g/equiv

W = Zit

Z= E/F

w = E/Fit

F = faraday = 96500 C

i = current = x

t = time = 15*60*60 = 54000 sec

w = weight of cl2 reacted = 15.45 g

15.45 = (35.5/96500)*x*54000

i = current = 0.78 A