The temperature of an ideal gas is increased from $27°$ to $927°C$. The r.m.s. speed of its molecules becomes-

An ideal gas is filled in a vessel, then

Molecular weight of two gases are $M_1 and M_{2.}$ At any temperature, the ratio of root mean square velocities $v_1 and v_2$ will be: 

According to the kinetic theory of gases, at absolute zero temperature: [AIIM 1998; UPSEAT 2000]

PV versus T graphs of equal masses of ${\mathrm{H}}_2, \mathrm{He} \mathrm{and} {\mathrm{O}}_2$ are shown in the figure. Choose the correct alternative:

The root-mean-square speed of hydrogen molecules at 300 K is 1930 m/s. Then the root mean square speed of oxygen molecules at 900 K will be: [MH CET 2002; Odisha JEE 2010]

What is the mass of 2 liters of nitrogen at 22.4 atmospheric pressure and 273 K?

Mean kinetic energy per degree of freedom of gas molecules is

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

If P is the pressure of the gas then the KE per unit volume of the gas is:

The variation of pressure versus temperature of an ideal gas is shown in the given diagram. From this diagram, one can conclude that

Maxwell's velocity distribution curve is given for two different temperatures. For the given curves-
                    

${\mathrm{n}}_1$ mole of monoatomic gas is mixed with ${\mathrm{n}}_2$ mole of diatomic gas such that ${\gamma }_{mix}=1.5$, then:

$\mathrm{Molar} \mathrm{heat} \mathrm{capacity} \mathrm{of} \mathrm{the} \mathrm{process} \mathrm{P} = \frac{\mathrm{a}}{\mathrm{T}} \mathrm{for} \mathrm{a} \mathrm{monoatomic} \mathrm{gas}, \text{'}\mathrm{a}\text{'} \mathrm{being} \mathrm{positive} \mathrm{constant} is-$

A rocket is propelled by a gas which is initially at a temperature of 4000 K. The temperature of the gas falls to 1000 K as it leaves the exhaust nozzle. The gas which will acquire the largest momentum while leaving the nozzle is:

A gas mixture consist of 2 moles of $O_2$ and 4 moles of Ar at temperature T. Neglecting all vibrational modes, the total internal energy of the system is:

One mole of an ideal monatomic gas undergoes a process described by the equation $P{V}^3=$ constant. The heat capacity of the gas during this process is:

A given sample of an ideal gas occupies a volume V at a pressure p and absolute temperature T. The mass of each molecule of the gas is m. Which of the following gives the density of the gas?

The molecules of a given mass of gas have r.m.s velocity of 200 ms^-1 at 27°C and 1.0 x 10⁵ Nm^-2 pressure. When the temperature and pressure of the gas are increased to ,respectively, 127°C and 0.05 X 10⁵ Nm^-2 , r.m.s velocity of its molecules in ms^-1 will become :

Two vessels separately contain two ideal gases A and B at the same temperature, the pressure of A being twice that of B. Under such conditions, the density of A is found to be 1.5 times the density of B. The ratio of molecular weight of A and B is:

A monoatomic gas at a pressure p, having a volume V expands isothermally to a volume 2 V and then adiabatically to a volume 16 V. The final pressure of the gas is: (take  γ=5/3)

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

The molar specific heats of an ideal gas at constant pressure and volume are denoted by C_P and C_V respectively. If γ=C_P/C_V and R is the universal gas constant, then CV is equal to
 

If ${\mathrm{C}}_{\mathrm{p}}$ and ${\mathrm{C}}_{\mathrm{v}}$ denote the specific heats (per unit mass) of an ideal gas of molecular weight M

At ${10}^{°}C$ the value of the density of a fixed mass of an ideal gas divided by its pressure is x. At ${110}^{°}C$ this ratio is 

The ratio of two specific heats of gas $C_p/C_v$ for argon is 1.6 and for hydrogen is 1.4. Adiabatic elasticity of argon at pressure P is E. Adiabatic elasticity of hydrogen will also be equal to E at the pressure :

One mole of a perfect gas in a cylinder fitted with a piston has a pressure P, volume V and temperature 273 K. If the temperature is increased by 1 K keeping pressure constant, the increase in volume is

If 300 ml of a gas at 27°C is cooled to 7°C at constant pressure, then its final volume will be -

Which one of the following gases possesses the largest internal energy?

Two gases of equal mass are in thermal equilibrium. If ${\mathrm{P}}_{\mathrm{a}}, {\mathrm{P}}_{\mathrm{b}}$ and ${\mathrm{V}}_{\mathrm{a}}$ and ${\mathrm{V}}_{\mathrm{b}}$ are their respective pressures and volumes, then which relation is true