The minimum pressure required to compress 600 dm³ of a gas at 1 bar to 150 dm³ at 40°C is

A certain gas takes three times as long to effuse out as helium. Its molecular mass will be:

A bubble of air is underwater at a temperature15°C and the pressure 1.5 bar. If the bubble rises to the surface where the temperature is 25°C and the pressure is 1.0 bar, what will happen to the volume of the bubble?

The pressure exerted by 6.0 g of methane gas in a 0.03 m³ vessel at 129 ºC is
(Atomic masses : C = 12.01, H = 1.01 and R = 8.314 JK^–1mol^–1)

For real gases van der Waals equation is written as

$(P+\frac{a{n}^2}{V^2}) (V-nb) = nRT$

Where 'a' and 'b' are van der Waals constants.

Two sets of gases are :
(I) $O_2, C{O}_2 , H_2 and He$        (II)$C{H}_4, O_2 and H_2$ 
The gases given in set-I in increasing order of 'b' and gases given in set-II in decreasing order of 'a', are arranged below. Select the correct order from the following :

Average molar kinetic energy of CO and N₂ at same temperature is :

In a gaseous mixture which of $N{O}_2 , C{O}_2 , and N_{2}O$ gases have same rate of diffusion :

If 400 ml gas at 500 torrs and 666.6 ml gas at 600 torrs is taken in a container of 3 liters, the total pressure of the mixture is

The temperature of 4.0 mole of a gas occupying 5 dm³ at 3.32 bar is -
(R = 0.083 bar dm³ K^–1 mol^–1).

The volume occupied by 8.8 g of CO₂ at 31.1°C and 1 bar pressure is -
(R = 0.083 bar L K^–1 mol^–1)

 As per Charles's law ,–273° C is the lowest possible temperature because-

The correct relation between density ($\mathrm{\rho }$) and pressure of gas (P) is-

A vessel of 120 mL capacity contains a certain amount of gas at 35 °C and 1.2 bar pressure. The gas is transferred to another vessel of volume 180 mL at 35 °C. The pressure would be-

The plots of different values of pressure versus temperature are shown in the given figure. The correct order of volume for the following plot is-

Pressure versus volume graph for a real gas and an ideal gas is shown below: 

The correct statement among the following is -

Consider the following graph:

The curve that represents CO₂ gas is - 

The variation of pressure with the volume of the gas at different temperatures can be
graphically represented as per the following graph:

If the temperature increases from 200K to 400K (at constant pressure), the volume of a
gas would-  

A plot of pressure versus $\frac{1}{\mathrm{V}}$ for a gas at constant temperature is given below:

The relation between ${\mathrm{T}}_1, {\mathrm{T}}_2, \mathrm{and} {\mathrm{T}}_3$ is- 

 $$\begin{gathered} 1. {\mathrm{T}}_1>{\mathrm{T}}_2>{\mathrm{T}}_3 \\ 2. {\mathrm{T}}_1<{\mathrm{T}}_2<{\mathrm{T}}_3 \\ 3. {\mathrm{T}}_1>{\mathrm{T}}_2<{\mathrm{T}}_3 \\ 4. \mathrm{None} \mathrm{of} \mathrm{the} \mathrm{above} \end{gathered}$$

Choose the correct option for graphical representation of Boyle's law, which shows a graph of pressure vs. volume of a gas at different temperatures :

Choose the correct option for the total pressure (in atm) in a mixture of 4 g O₂ and 2 g H₂ confined in a total volume of one litre at 0$°$C is :

A neon-dioxygen mixture contains 70.6 g dioxygen and 167.5 g neon. If the pressure of the mixture of gases in the cylinder is 25 bar. The partial pressure of dioxygen and neon in the mixture are respectively-

Gases possess characteristic critical temperature which depends upon the magnitude of intermolecular forces between the gas particles. Critical temperatures of ammonia and carbon dioxide are 405.5 K and 304.10 K respectively. The gas liquify first when cooling start from 500 K to their critical temperature, is-

Two different gases 'A' and 'B' are filled in separate containers of equal capacity under the same conditions of temperature and pressure. On increasing the pressure slightly, the gas 'A' liquifies but gas 'B' does not liquefy even on applying high pressure until it is cooled. Incorrect statement among the following regarding above observation is -

The correct sequence of increasing order of viscosity among the following is -