During the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is approximately:
Given
Equivalent weight of chlorine = Molecularweightofchlorinen−factor=35.51=35.5g
Electric current passed = 3 amperes
Number of moles = 0.10 mole
Weight of 2 chlorine ions = Numberofmoles×Molecularmass
Step 1:
At Cathode: 2H2O+2e−⟶H2+2OH−
At Anode: 2Cl−⟶Cl2+2e−
Step 2:
Applying Faraday's Law
W=E×It96500
W is the weight of substance deposited
E is the equivalent weight of the substance
I is the electric current passed
t is the time in sec
0.1×71=35.5×t(sec)×396500
t=6433sec=107.2min≈110min
Hence, option (D) is correct.