The molecular weight of a gas which diffuses through a porous plug of 1/6th of the speed of hydrogen under identical condition is:

If one mole of a monoatomic gas ($\gamma =5/3$) is mixed with one mole of a diatomic gas ($\gamma =7/5$), the value of $\gamma$ for the mixture is:

A gas is heated from $0°C to 100°C$ at 1.0 atm pressure. If the initial volume of the gas is 10 litre, its final volume would be:

The rates of diffusion of $O_2 and H_2$ at same P and T are in the ratio:

As the temperature is raised from $20°C to 40°C$, the average kinetic energy of neon atoms changes by a factor:

The density of neon will be highest at:

At 27$°$ C, the ratio of root mean square speeds of ozone to oxygen is-

How many mole of He gas occupy 22.4 litre at 30 C and one atmospheric pressure?

The rms speed of the molecules of a gas of density 4 kg$m^{-3} and pressure 1.2 \times {10}^5\times N{m}^{-2} is;$

$$\begin{gathered} \left(a\right) 120 m{s}^{-1} \\ \left(b\right) 300 m{s}^{-1} \\ \left(c\right) 600 m{s}^{-1} \\ \left(d\right) 900 m{s}^{-1} \end{gathered}$$

4.0 g of argon gas pressure P and temperature T K in a vessel. On increasing the temperature by 50^o, 0.8 g of argon was given out to maintain the pressure P.

The original temperature was:

Correct statement regarding heating of a liquid is - 

Which of the following law leads us to arrive at the conclusion that 1 g-molecule of each gas at STP occupies a volume of 22.4 L?

0.1 mole of gas absorbs 41.75 J of heat, the rise in temperature occurs $20°\mathrm{C}$, the gas must be

Van der Waals real gas, act as an ideal gas, at :

By the ideal gas law the pressure of 0.60 mol ${\mathrm{NH}}_3$ gas in a 3.00 litre vessel at $25°\mathrm{C}$ is

The pressure of a mixture of 4 g of ${\mathrm{O}}_2$ and 2 g of ${\mathrm{H}}_2$ confined in a bulb of 1.0 L capacity at $0°\mathrm{C}$

The volume occupied by 9.0 g of nitrogen gas at 300 K and 750 mmHg pressure is

The rms velocity of ${\mathrm{CO}}_2$ at a temperature T (in Kelvin) is X cm ${\sec }^{-1}$. At what temperature (in Kelvin), the rms velocity of nitrous oxide would be 4 X ${\sec }^{-1}$?

( Atomic weights of C, N, and O are respectively 12, 14 and 16)

7.5 grams of gas occupy 5.6 liters of volume at STP. The gas is..

(Atomic weight of C, N, and O are 12, 14, 16 respectively)

The compressibility factor for 1 mol of a van der Waals gas at $0°\mathrm{C}$ and 100 atmospheric pressure is found to be 0.5. The volume of gas is-

4 grams of an ideal gas occupies 5.6035 liters of volume at 546 K and 2 atm pressure. What is its molecular weight?

The kinetic energy of 4 moles of nitrogen gas at 127$°$C is ......... Kcals. (R=2 cal $mo{l}^{-1} K^{-1}$)

A gaseous mixture contains 56 g of $N_2, 44 g of C{O}_2 and 16 g of C{H}_4.$ The pressure of mixture is 720 mm of Hg. The partial pressure of methane is

At $25°C and 730 mm pressure, 380 mL of dry$ oxygen was collected. If the temperature is constant, what volume will the oxygen occupy at 760 mm pressure?

At a certain pressure, volume of a gas at $27°$C is 20 litre. If the pressure and temperature are doubled, its volume will be

A gas has double the average velocity of $S{O}_2$ gas at any temperature. The gas may be

The densities of two gases are in the ratio of 1:16. The ratio of their rates of diffusion is

The critical temperature of the water is higher than that of ${\mathrm{O}}_2$ because the ${\mathrm{H}}_2\mathrm{O}$ molecule has

56 g of nitrogen and 96 g of oxygen are mixed iso-thermally and a total pressure of 10 atm. The partial pressures of oxygen and nitrogen (in atm) are respectively

A bottle of dry ammonia and a bottle of dry hydrogen chloride connected through a long tube are opened simultaneously at both ends, the white ammonium chloride ring first formed will be