Three flasks of equal volumes contain CH4, CO2 and Cl2 gases respectively. They will contain equal number of molecules if -
1 Crore+ students have signed up on EduRev. Have you? Download the App |
A certain mass of a gas occupies a volume of 2 litres at STP. Keeping the pressure constant at what temperature would the gas occupy a volume of 4 litres
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-
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 -
Air contains 79% N2 and 21% O2 by volume. If the pressure is 750 mm Hg, the partial pressure of O2 is -