Calculate the amount of chlorine gas evolved during the electrolysis of molten potassium
chloride on passing a current of 0.5 A for two hours through it.
I= 0.5A, t=2hrs= 2x3600s=7200s
Q=It= 0.5x7200=3600C= 3600/96500= 0.037F
The half reaction occurring at the anode is
2Cl- ---> Cl2 + 2e-
2F liberates 1mol of Cl2
0.037F will liberate 1/2 x 0.037= 0.0186mole of Cl2
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