NEET Physics Kinetic Theory Class 11 Questions

A gas mixture consists of molecules of A, B and C with masses mₐ > m_b > m_c at a fixed temperature. Statement 1: Rms speed order is (v_rms)_c > (v_rms)_b > (v_rms)_a. Statement 2: Average Kinetic energy order is K_c > K_b > K_a.

A flask contains argon and chlorine in the ratio of 2 : 1 by mass. The temperature of the mixture is 27°C. The ratio of root mean square speed of the molecules of the two gases \( \left( \frac{v_{\text{Ar rms}}}{v_{\text{Cl rms}}} \right) \) is: (Atomic mass of argon = 40.0 u and molecular mass of chlorine = 70.0 u)

A container has two chambers of volumes V₁ = 2 litres and V₂ = 3 litres separated by a partition made of a thermal insulator. The chambers contains n₁ = 5 and n₂ = 4 moles of ideal gas at pressures p₁ = 1 atm and p₂ = 2 atm, respectively. When the partition is removed, the mixture attains an equilibrium pressure of :

The following graph represents the T⁻V curves of an ideal gas (where T is the temperature and V the volume) at three pressures P₁, P₂ and P₃ compared with those of Charles’s law represented as dotted lines. Then the correct relation is:

The temperature of a gas is –50° C. To what temperature the gas should be heated so that the rms speed is increased by 3 times?

A cylinder contains hydrogen gas at pressure of 249 kPa and temperature 27°C. Its density is: (R = 8.3 J mol⁻¹ K⁻¹)

The mean free path for a gas, with molecular diameter d and number density n can be expressed as:

Increase in temperature of a gas filled in a container would lead to:

At what temperature will the r.m.s. speed of oxygen molecules become just sufficient for escaping from the Earth's atmosphere? (Given: Mass of oxygen molecule (m) = 2.76 × 10⁻²⁶ kg, Boltzmann's constant k_B = 1.38 × 10⁻²³ J/K)

The molecules of a given mass of a gas have r.m.s velocity of 200 m s⁻¹ at 27°C and 1.0 × 10⁵ Nm⁻² pressure. When the temperature and pressure of the gas are respectively, 127°C and 0.05 × 10⁵ Nm⁻², the r.m.s. velocity of its molecules in m s⁻¹ is

The mean free path of molecules of a gas (radius r) is inversely proportional to

In a vessel, the gas is at a pressure P. If the mass of all the molecules is halved and their speed is doubled, then the resultant pressure will be: