Kinetic theory of gases practice · Mixed difficulty

Assertion: Absolute zero is the temperature corresponding to zero energy.
Reason: The temperature at which no molecular temperature.

A balloon carries a total load of 185 kg at normal pressure and temperature of $\mathrm{2}{\mathrm{7}^ \circ }\,\mathrm{C}\,$.
What load will the balloon carry on rising to a height at which the barometric pressure is 45 cm of Hg and the temperature is $- {\mathrm{7}^ \circ }\,\mathrm{C}$ ?
[Assuming, the volume constant.]

$N$ moles of a polyatomic gas $(f=6)$ must be mixed with two moles of a monoatomic gas so that the mixture behaves as a diatomic gas. The value of $N$ is :

Two identical containers $\mathrm{A}$ and $\mathrm{B}$ have frictionless pistons. They contain the same volume of a ideal gas at the same temperature. The mass of the gas in $\mathrm{A}$ is $\mathrm{m}_{\mathrm{A}}$ and that in $\mathrm{B}$ is $\mathrm{mB}$. The gas in each cylinder is now allowed to expand isothermally to double the initial volume. The changes in the pressure in A and B are found to be $\Delta p$ and $1.5 \Delta p$ respectively.

Assertion: ${V}_{\mathrm{rms}}$ and ${V}_{\mathrm{mean}}$ of gaseous molecules is nearly of the order of velocity of sound.
Reason: The sound travels in air because of vibrational molecular motion.

In the absence of intermolecular forces of attraction, the observed pressure $p$ will be

The critical volume of a gas obeying van der Waals' equation is

The root mean square speed of molecules of a gas is 1260 m/s. The average speed of the gas molecules is

If number of molecules of ${H_2}$ are double than that of ${O_2},$ then ratio of kinetic energy of hydrogen and that of oxygen at $300\;K$ is

If the rms velocity of the molecules of a gas in a container be doubled than pressure of gas will

The root mean square velocity, $v_{\text {rms}}$, the average velocity, $v_{{av}}$ and the most probable velocity, $v_{{mp}}$ of the molecules of the gas are in the order:

The value closest to the thermal velocity of a Helium atom at room temperature (300K) in $m{s^{ - 1}}$ is $\left[ {{k_B} = 1.4 \times {{10}^{ - 23}}J/K;{m_{He}} = 7 \times {{10}^{ - 27}}kg} \right]$

At constant pressure, which of the following is true?

Two gases $A$ and $B$ having same pressure $p$, volume $V\;$ and absolute temperature $T$ are mixed. If the mixture has the volume and temperature as $V$ and $T$ respectively, then the pressure of the mixture is

The rate of diffusion is

The specific heat of an ideal gas is

The root mean square velocity of the gas molecules is $300 \mathrm{~m} / \mathrm{s}$. What will be the root mean square speed of the molecules if the atomic weight is doubled and absolute temperature is halved?

A gas is taken through a number of thermodynamic states. What happens to its specific heat?

If the molecular weight of two gases are ${M_1}$ and ${M_2}$, then at a temperature the ratio of root mean square velocity ${v_1}$ and ${v_2}$ will be

To raise the temperature of a certain mass of gas by $5{\mathrm{0}^\mathrm{o}}\mathrm{C}$ at a constant pressure, 160 cal of heat is required. When the same mass of gas is cooled by $10{\mathrm{0}^\mathrm{o}}\mathrm{C}$ at constant volume, 240 cal of heat is released. How many degrees of freedom does each molecule of this gas have (assume gas to be ideal)?

The root mean square speeds of molecules of ideal gases at the same temperature are:

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:

The root mean square speed of smoke particles of mass $5 \times 10^{-17} \mathrm{~kg}$ in their Brownian motion in air at NTP is approximately. [Given $k=1.38 \times 10^{-23} \mathrm{JK}^{-1}$ ]

Find the number of molecules in $1 \mathrm{~cm}^3$ of an ideal gas at $0^{\circ} \mathrm{C}$ and at a pressure of $10^{-5} \mathrm{~mm}$ of mercury.

The diameter of oxygen atom is $3\mathop A\limits^ \circ$. The fraction of molecular volume to the actual volume occupied by oxygen at STP is

The absolute temperature of a gas is determined by

If the mean free path of atoms is doubled then the pressure of gas will become

At O K which of the following properties of a gas will be zero

The parameter that remains the same for molecules
of all gases at a given temperature is :

Supposing the distance between the atoms of a diatomic gas to be constant, its specific heat at constant volume per mole (gram mole) is