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Grade 11Physical Chemistry

A container holds 22.4 litre of a gas at 1 atmospheric pressure and at 0°C. The gas consist of a mixture of argon, oxygen, and sulphur dioxide in which :
(a) Partial Pressure of SO₂= (Partial Pressure of O₂) + (Partial Pressure of Ar).
(b) Partial Pressure of O₂ = 2 × Partial Pressure of Ar.
Calculate the density of the gas mixture under these conditions.

Question image for A container holds 22.4 litre of a gas at 1 atmosp

Rohit Singh

6 Years agoGrade 11

1 Answer

Rahul

Approved Tutor Answer6 Years ago

(a) P_SO2=P_O2+P_{Ar =}3P_Ar.[using (b)]

Now from Dalton's law of partial pressure

P_SO2+P_O2+P_Ar=1

=> 3P_Ar+2P_Ar+P_Ar=1

=> P_Ar=1/6

P_O2=1/3

P_SO2=1/2

Now using PV=nRT

We get no. of moles =PV/RT= 0.9994

Now as we know,

P_Ar=mole fraction of Ar *P_Total

Mole fraction of Ar =1/6

Moles of Ar/ Total no. of moles = 1/6

So, no of moles of Ar = 0.9994/6 = 0.16

Similarly, moles of O₂=0.9994/6 = 0.33

Moles of SO₂= 0.9994/6 = 0.499

Also, moles = Mass/Molecular weight

Mass of Ar = 6.4

Mass of O₂=10.56

Mass of SO₂= 31.36

Total mass =48.32

Density = Mass/volume =48.32/22.4 = 2.157

Hope it helps

Me Rahul from Kurukshetra, Haryana

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