Gasesous State - Class 11 MCQ

At 100 ºC a gas has 1 atm. pressure and 10 L volume. Its volume at NTP would be -

If 500 ml of a gas 'A' at 1000 torr and 1000 ml of gas B at 800 torr are placed in a 2L container, the final pressure will be-?

Two flasks A and B of 500 ml each are respectively filled with O2 and SO2 at 300 K and 1 atm. pressure. The flasks will contain-

In the gas equation PV = nRT, the value of universal gas constant would depend only on -?

8.2 L of an ideal gas weight 9.0 gm at 300 K and 1 atm pressure. The molecular mass of gas is

A 0.5 dm³ flask contains gas 'A' and 1 dm ³ flask contains gas 'B' at the same temperature. If density of  A = 3.0 gm dm ^-3 and that of B = 1.5 gm dm ^-3 and the molar mass of A = 1/2 of B, then the ratio of pressure exerted by gases is- 

The density of a gas is equal to ?

(P = pressure ; V = volume ; T = temperature, R = gas constant, n = number of moles and M = molecular wt) -

One litre of an unknown gas weighs 1.25 gm at N.T.P. which of the following gas pertains to the above data -

If the density of a gas A is 1.5 times that of B then the molecular mass of A is M. The molecular mass of B will be-

When the pressure of 5L of N2 is doubled and its temperature is raised from 300K to 600K, the final volume of the gas would be-

The value of gas constant R is 8.314 X. Here X is represented by

The value of gas constant per mole is approximate-

A gas is found to have a formula [CO]_x. If its vapour density is 70 the value of x is-

A cylinder is filled with a gaseous mixture containing equal masses of CO and N₂. The ratio of their partial pressure is-

At room temperature Dalton's law of partial pressure is not applicable to -

The total pressure of a mixture of two gases is -

Air contains 79% N₂ and 21% O₂ by volume. If the pressure is 750 mm Hg, the partial pressure of O₂ is -