STANDARD Physics Kinetic Theory Class 11 Questions

An air bubble of volume 1.0 cm³ rises from the bottom of a lake 40 m deep at a temperature of 12°C. To what volume does it grow when it reaches the surface which is at a temperature of 35°C?

Pressure of a gas at constant volume is proportional to

A gas is filled in a container at pressure P₀. If the mass of molecules is halved and their rms speed is doubled, then the resultant pressure would be

Which one of the following is not an assumption of kinetic theory of gases?

0.014 kg of nitrogen is enclosed in a vessel at a temperature of 27°C. At which temperature the rms velocity of nitrogen gas is twice its the rms velocity at 27°C?

At what temperature is the rms velocity of hydrogen molecule equal to that of an oxygen molecule at 47°C?

If vₘₛ is the rms speed of molecules in a gas and v is the speed of sound waves in the gas, then the ratio vₘₛ/v is

The temperature of an ideal gas is increased from 27°C to 127°C, then percentage increase in v_rms is?

The temperature of an ideal gas is increased from 120 K to 480 K. If at 120 K, the rms velocity of the gas molecules is v_rms, then at 480 K, it becomes

If three molecules have velocities 0.5 km s⁻¹, 1 km s⁻¹ and 2 km s⁻¹, the ratio of the rms speed and average speed is

Mean free path of a gas molecule is

Assertion: In case of collision of gas molecules in a given amount of gas, total kinetic energy is conserved. Reason: All collisions of the gas molecules in a given amount of gas are elastic.

Assertion: Average kinetic energy per molecule of any ideal monoatomic gas is \( \frac{3}{2} k T \). Reason: Average kinetic energy depends only on temperature and is independent of the nature of the gas.

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

A mixture of 2 moles of helium gas (atomic mass = 4 u), and 1 mole of argon gas (atomic mass = 40 u) is kept at 300 K in a container. The ratio of their rms speeds \( \frac{v_{\text{rms (helium)}}}{v_{\text{rms (argon)}}} \) is close to

At what temperature will the rms speed of oxygen molecules become just sufficient for escaping the Earth's atmosphere? (Given : Mass of oxygen molecule (m) = 2.76 × 10⁻²⁶ kg, Boltzmann constant k_B = 1.38 × 10⁻²³ J K⁻¹)

Assertion : The total translational kinetic energy of all the molecules of a given mass of an ideal gas is 1.5 times the product of its pressure and its volume. Reason : The molecules of a gas collide with each other and the velocities of the molecules change due to the collision.

The molecules of a given mass of a gas have rms velocity of 200 ms⁻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 N m⁻², the rms velocity of its molecules in ms⁻¹ is:

The average translational kinetic energy of O₂ molecules (relative molar mass 32) at a particular temperature is 0.048 eV. The translational kinetic energy of N₂ molecules (relative molar mass 28) in eV at the same temperature is

For a given gas at 1 atm pressure, rms speed of the molecules is 200 m/s at 127°C. At 2 atm pressure and at 227°C, the rms speed of the molecules will be

The mass of a hydrogen molecule is 3.32 × 10⁻²⁷ kg. If 10²³ hydrogen molecules strike, per second, a fixed wall of area 2 cm² at an angle of 45° to the normal, and rebound elastically with a speed of 10³ m s⁻¹, then the pressure on the wall is nearly

vᵣₘₛ, vₐᵥ and vₘₚ are root mean square, average and most probable speeds of molecules of a gas obeying Maxwell's velocity distribution. Which of the following statements is correct

The root mean square (rms) speed of oxygen molecules O₂ at a certain temperature T (absolute) is v. If the temperature is doubled and oxygen gas dissociates into atomic oxygen, the rms speed:

Match Column - I and Column - II and choose the correct match from the given choices.

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?

The mean free path λ of molecules is given by where n is the number of molecules per unit volume and d is the diameter of the molecules.