We have given-
Pressure :
We have a relation of gas as :PV = nRT
n(number of.moles) = given mass(2g)/molecular mass(M)
P= pressure
V= volume (6L)
R= universal gas constant
T= Temperature 268 K
P = (given mass/M) × RT/V
=> P= (2 × R × 268 )/6×M
Only P depends upon M all other factors are same so,
Pressure is inversely proportional to Molar mass.
H2 (2 g/mol) < He (4 g/mol) < CH4 (16 g/mol)
=> pressure is CH4 > He> H2
so, B>C>A.
Average molecular kinetic energy:
Kinetic energy: (1/2)mv2
Ekinetic energy is directly proportional to molar mass.
so,
A>C>B
Diffusion rate after valve open:
as diffusion rate depends upon density.
diffusion rate inversely proportional to density and density = mass/volume .
so,
Diffusion rate is inversely proportional to Molar mass
OR using Graham's law:
Rate1/Rate2 = (mass2/mass1)0.5
So, trend is CH4 > He > H2
then , B> C> A
Total kinetic energy of molecules:
given same temperature .
all molecules have equal total kinetic energy which depends upon temperature
A=B=C
Density:
density = mass/volume
here mass is molar mass.
so, density is proportional to molar mass.
=> A>C>B
Collision frequency:
collision frequency is inversely proportional to molar mass as:
Z(collision frequency) (8kBT/πM)0.5
So, smaller the molar mass more the collision frequency:
=> B>C>A
*for anq query regarding this question feel free to contact in comments section.
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