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Class 11

>>Chemistry

>>States of Matter

>>Ideal Gas Equation

>>Equal masses of SO2, CH4 and O2 are mixe

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Equal masses of SO

2

,CH

4

and O

2

are mixed in empty container at 298K, when the total pressure is 2.1 atm. The partial pressures of CH

4

in the mixture is :

Hard

Solution

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Correct option is C)

Let us take x gm of each of the components.

Molecular Mass of SO

2

=64

∴ moles of SO

2

=

64

x

Molecular Mass of CH

4

=16

∴ moles of CH

4

=

16

x

Molecular Mass of O

2

=32

∴ moles of O

2

=

32

x

Total Moles =

64

x

+

16

x

+

32

x

=

64

7x

Mole fraction of CH

4

=

7x/64

x/16

=

7

4

Hence, partial pressure of CH

4

= mole fraction × total pressure =

7

4

×2.1=1.2 atm

A container having a pin-hole contains equal masses of SO2 and CH4.

We have to find the ratio of no of moles of SO2 and CH4 effused out initially.

According to Graham's law of diffusion/effusion, "It states that under specific temperature and pressure, the rate of diffusion or effusion is inversely proportional to the square root of their density."

i.e., r ∝ 1/√d

∵ d = PM/RT and r = no of moles effused or diffused/time taken

∴ n/t ∝ 1/√M    [P , R and T are constant ]

⇒ n₁/n₂ = √M₂/√M₁

Here, M₁ = molar mass of SO2 = 64 g/mol

M₂ = molar mass of CH4 = 16 g/mol

Now, n₁/n₂ = √(16)/√(64) = 1/2

Also read similar questions : a gaseous mixture contain equal mass of O2 and SO2 . the mole fraction of SO2 in the mixture is??

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