The pressure and temperature of an ideal gas in a closed vessel are $720\;kPa$ and ${40^ \circ }C$ respectively. If $\frac{1}{4}$ th of the gas is released from the vessel and the temperature of the remaining gas is raised to ${353^ \circ }C,$, the final pressure of the gas is

The temperature of the mixture of one mole of helium and one mole of hydrogen is increased from ${0^ \circ }C$ to ${100^ \circ }C$ at constant pressure. The amount of heat delivered will be

Mean free path of a gas molecule is

The average translational kinetic energy of a hydrogen gas molecules at NTP will be

[Boltzmann’s constant ${k_B} = 1.38 imes {10^{ - 23}}J/K$]

KE per unit volume is $E$. The pressure exerted by the gas is given by

The average kinetic energy of hydrogen molecules at $300\;K$ is $E.$ At the same temperature, the average kinetic energy of oxygen molecules will be

An ideal gas has molecules with 5 degrees of freedom. The ratio of specific heats at constant pressure $\left( {{C_P}} \right)$ and at constant volume $\left( {{C_V}} \right)$ is:

If the pressure of an ideal gas is doubled while keeping the volume constant, what happens to the rms speed of the gas molecules?

Two identical containers hold equal moles of different ideal gases, A and B, at the same temperature. Which of the following statements is true about the pressure exerted by the gases?

Relationship between $P,V,$ and $E$ for a gas is

Pressure of an ideal gas is increased by keeping temperature constant. What is the effect on kinetic energy of molecules?