Gaseous State

Equal masses of methane and oxygen are mixed in an empty container at 25^oC. The fraction of the total pressure exerted by oxygen is

A mixture of one mole each of H₂ , He and O₂ each are enclosed in a cylinder of volume V at temperature T. If the partial pressure of H₂ is 2 atm, the total pressure of the gases in the cylinder is :

Value of gas constant R is

For an ideal gas, number of moles per litre in terms of its pressure P, gas constant R and temperature T is

If 10^–4 dm³ of water is introduced into a 1.0 dm³ flask to 300 K, how many moles of water are in the vapour phase when equilibrium is established ? (Given : Vapour pressure of H₂O at 300 K is 3170 Pa ; R = 8.314 J K^–1 mol^–1)

At 300 K, the density of a certain gaseous molecule at 2 bar is double to that of dinitrogen (N₂ ) at 4 bar. The molar mass of gaseous molecule is :

Assuming ideal gas behaviour, the ratio of density of ammonia to that of hydrogen chloride at same temperature and pressure is : (Atomic wt. of Cl = 35.5 u)

0.5 moles of gas A and x moles of gas B exert a pressure of 200 Pa in a container of volume 10 m³ at 1000 K. Given R is the gas constant in JK^$$-$$1mol^$$-$$1, x is :

An open vessel at 27^oC is heated until two fifth of the air (assumed as an ideal gas) it has escaped from the vessel assuming that the volume of the vessel remains constant, the temperature at which the vessel has been heated is -

An evacuated glass vessel weighs 40.0 g when empty, 135.0 g when filled with a liquid of density 0.95 g mL^$$-$$1 and 40.5 g when filled with an ideal gas at 0.82 atm at 250 K. The molar mass of the gas in g mol^$$-$$1 is : (Given : R = 0.082 L atm K^$$-$$1 mol^$$-$$1)

Kinetic theory of gases proves

According to the kinetic theory of gases, in an ideal gas, between two successive collisions of a gas molecule travels

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

Which one of the following statements is NOT true about the effect of an increase in temperature on the distribution of molecular speeds in a gas?

For gaseous state, if most probable speed is denoted by C*, average speed by $$\mathop C\limits^{\_\_}$$ and mean square speed by C, then for a large number of molecules the ratios of these speeds are:

Initially, the root mean square (rms) velocity of N₂ molecules at certain temperature is $$u$$. If this temperature is doubled and all the nitrogen molecules dissociate into nitrogen atoms, then the new rms velocity will be :

In Van der Waals equation of state of the gas law, the constant ‘b’ is a measure of

'a’ and `b’ are van der Waals’ constants for gases. Chlorine is more easily liquefied than ethane because

The compressibility factor for a real gas at high pressure is :