We know ideal gas equation
Where V= volume of gas
n=number of moles of gas
P=pressure of gas
Volume inside jar V1= 1.0 × 10–3 m3
Pressure inside jar P1 =1.5 × 105 Pa
Temperature inside jar T1=400K
Pressure of surrounding P2 =1atm=1.0Pa
Temperature of surrounding T2=300K
Let volume of oxygen at T2 and P2 =V2
When jar is in equilibrium with surrounding, temperature and pressure of oxygen gas inside jar will T2 and P2.
Number of moles will be same inside the jar, before and after equilibrium as no new oxygen gas has been added. Just temperature and pressure has been changed. Due to which volume will change.
Assuming there is no leak in jar, applying ideal gas equation before and after equilibrium, we get
Now if we consider leak,
Volume of gas leaked =V2-V1
If n2 are number of moles leaked out, then
Mass of the gas leaked out =n2molar mass of oxygen molecule
Molar mass of oxygen molecule=32g/mol
Mass of gas leaked out=0.00532=0.16g
The mass of the gas that leaked out =0.16g.
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