Pressure is given by (1/3)nmv².
v² = 3v_x² = 3m²/s².
P = (1/3)*20*10^-20*3
= 20*10^-20Pa.

A diatomic gas has 3 translational degrees of freedom and 2 rotational degrees of freedom. Thus, total number of degrees of freedom is 5.

22.4L of a gas at STP has a weight equal to its molar mass.
So, weight of CO₂ will be 12+16+16
= 44g.

Average kinetic energy is given by (3/2)k_BT, which shows that it only depends on temperature.

The value of C_v for a monatomic gas is 3/2 R and
C_P is 5/2 R.
Thus value of γ is:
C_P/C_V= 5/3.

Real gases, unlike ideal gases, consider volume taken up by molecules because of which mean free path decreases or collisions increase and hence pressure increases. So, at low volumes this factor will play a big role and thus for a particular volume in low volume range, pressure of real gases will be higher. To see which graph belongs to whom we can draw a line parallel to pressure axis at very low volume. The one having higher pressure will be that of real gases. Therefore, 2-real gas & 1-ideal gas.

The ratio of partial pressures will be in same ratio as that of moles, i.e: 1:3:5.
Let partial pressure of gas 1 be ?x?.
Thus, x+3x+5x = 54.
x = 6Pa.

The atoms of gas have most interatomic space and can refore travel freely. This is why y travel longer distances without colliding and are refore said to have maximum mean free path.

Using, PV=NkT we get: N = PV/kT
= (3*3*10⁵)/(1.38*10^-23*300)
= 2.17*10^-20.

Internal energy is given by: E = (1/2)Nmv²,
where N is total number of molecules = nV.
E = 0.5*20*0.02*10^-20*4
= 0.8*10^-20J.