In the electrolysis of aqueous NaClNaCl, how many liters of Cl2(g)Cl2(g) (at STP) are generated
by a current of 7.50 A for a period of 100 minutes?
We are given the following data:

The current is: Io=7.50AIo=7.50A.

The time is: t=100min=6000st=100min=6000s.
The Faraday constant is: F=96485C/moleF=96485C/mole.
The molar volume of an ideal gas at STP is: vo=22.40L/molevo=22.40L/mole.
The chemical equation of electrolysis of NaClNaCl is,
NaCl(aq)+H2O(l)→Cl2(g)+H2(g)+NaOH(aq)NaCl(aq)+H2O(l)→Cl2(g)+H2(g)+NaOH(aq
)
The dissociation of chlorine gas is,
2Cl−→Cl2+2e−2Cl−→Cl2+2e−
The expression for the charge flows is,
Qo=IotQo=Iot
The expression for the number of moles of an electron is,
no=QoFno=QoF
Substitute the values and solve the above expression,
no=IotF=7.50×600096485=0.466moleno=IotF=7.50×600096485=0.466mole
The number of electron in dissociation of chlorine gas is: 2.
The expression for the number of moles of chlorine ion is,
na=12nona=12no
Substitute the values and solve the above expression,
na=12×0.466=0.233molena=12×0.466=0.233mole
The expression for the volume of chlorine gas generated is,
Va=navoVa=navo
Substitute the values and solve the above expression,
Va=0.233×22.40=5.21LVa=0.233×22.40=5.21L