An increase in temperature of a gas-filled in a container would lead to:

For a gas, if the ratio of  specific heats at constant pressure and constant volume is $\gamma$, then the value of degree of freedom is

The value $\mathrm{\gamma }=\left(\frac{{\mathrm{C}}_{\mathrm{p}}}{{\mathrm{C}}_{\mathrm{v}}}\right)$ for hydrogen, helium, and another ideal diatomic gas X (whose molecules are not rigid but have an additional vibrational mode), are respectively equal to:

What is the ratio of temperatures ${\mathrm{T}}_1 \mathrm{and} {\mathrm{T}}_2?$

How does the temperature change when the state of an ideal gas is changed according to the process shown in the figure?

From the following V-T diagram, we can conclude

When the gas in an open container is heated, the mean free path:

Maxwell's speed distribution graph is drawn as shown below. The most probable speed of the gas molecules is:
                        

A closed container having an ideal gas is heated gradually to increase the temperature by 20%  The mean free path will become/remain:

Two ideal gases have the same number of molecules per unit volume and the radii of their molecules are r and 3r respectively. The ratio of their mean free path in identical containers will be:

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

A cylinder contains hydrogen gas at a pressure of 249 kPa and temperature $27°C$

The average thermal energy for a mono-atomic gas is:

(${\mathrm{k}}_{\mathrm{B}}$ is Boltzmann constant and T absolute temperature)

Molar specific heat at constant volume, for a non-linear triatomic gas is: (vibration mode neglected)

An ideal gas equation can be written as $\mathrm{P}=\frac{\mathrm{\rho RT}}{{\mathrm{M}}_0}$ where $\mathrm{\rho }$ and ${\mathrm{M}}_0$ are respectively,

The fraction of molecular volume to the actual volume occupied by oxygen gas at STP is: (Take the diameter of an oxygen molecule to be 3 Å).

$$\begin{gathered} \left(1\right) 4\times {10}^{-4} \\ \left(2\right) 5\times {10}^{-4} \\ \left(3\right) 3\times {10}^{-4} \\ \left(4\right) 1\times {10}^{-4} \end{gathered}$$

Molar volume is the volume occupied by 1 mol of any (ideal) gas at standard temperature and pressure (STP: 1 atmospheric pressure, $0 °\mathrm{C}$) is:

The figure shows a plot of PV/T versus P for $1.00\times {10}^{-3} kg$ of oxygen gas at two different temperatures.

Then relation between $T_1 and T_2 is:$

$$\begin{gathered} 1. T_1=T_2 \\ 2. T_1<T_2 \\ 3. T_1>T_2 \\ 4. T_1\ge T_2 \end{gathered}$$

The figure shows a plot of PV/T versus P for $1.00\times {10}^{-3} kg$ of oxygen gas at two different temperatures.

The value of PV/T where the curves meet on the y-axis is:

$$\begin{gathered} 1. 0.06 J K^{-1} \\ 2. 0.36 J K^{-1} \\ 3. 0.16 J K^{-1} \\ 4. 0.26 J K^{-1} \end{gathered}$$

An oxygen cylinder of volume 30 litres has an initial gauge pressure of 15 atm and a temperature of 27 °C. After some oxygen is withdrawn from the cylinder, the gauge pressure drops to 11 atm, and its temperature drops to 17 °C. The mass of oxygen taken out of the cylinder is: $\left(\mathrm{R}=8.31 {\mathrm{mol}}^{-1}{\mathrm{K}}^{-1}, \mathrm{molecular} \mathrm{mass} \mathrm{of} {\mathrm{O}}_2=32 \mathrm{u}\right)$

An air bubble of volume 1.0 $c{m}^3$ 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?

$$\begin{gathered} \left(1\right) 5.3 c{m}^3 \\ \left(2\right) 4.0 c{m}^3 \\ \left(3\right) 3.7 c{m}^3 \\ \left(4\right) 4.9 c{m}^3 \end{gathered}$$

What is the total number of air molecules (inclusive of oxygen, nitrogen, water vapor, and other constituents) in a room of capacity 25.0 $m^3$ at a temperature of 27 °C and 1 atm pressure?

$\begin{array}{l}1. 6.1\times {10}^{23} \mathrm{molecules}\\ 2. 6.1\times {10}^{26} \mathrm{molecules}\\ 3. 7.1\times {10}^{23} \mathrm{molecules}\\ 4. 7.1\times {10}^{26} \mathrm{molecules}\end{array}$

What is the average thermal energy of a helium atom at room temperature (27 °C)?

$\begin{array}{rcl}& & 1. 11.21\times {10}^{-20} J\\ & & 2. 3.09\times {10}^{-16} J\\ & & 3. 6.21\times {10}^{-21} J\\ & & 4. 5.97\times {10}^{-19} J\end{array}$

At what temperature is the root mean square speed of an atom in an argon gas cylinder equal to the RMS speed of a helium gas atom at – 20 °C? (atomic mass of Ar = 39.9 u & of He = 4.0 u).

$$\begin{gathered} \left(1\right) 1.01\times {10}^3 K \\ \left(2\right) 3.15\times {10}^3 K \\ \left(3\right) 1.91\times {10}^3 K \\ \left(4\right) 2.52\times {10}^3 K \end{gathered}$$

Select the incorrect statement about Maxwell's speed distribution curve.

By increasing the temperature of a gas by 6 ^oC, its pressure increases by 0.4% at constant volume. Then the initial temperature of the gas is:

Boyle's law is obeyed by:

For an ideal gas, the fractional change in its volume per degree rise in temperature at constant pressure is equal to [T is the absolute temperature of the gas]:

The rise in the temperature of a given mass of an ideal gas at constant pressure and at temperature 27 ^oC to double its volume is: