The total pressure exerted by the mixture of equal moles of two gases is `5xx10^(3)NM^(-2)` in a container of volume 2 litres at 273K. Calculate the number of moles of the gases mixed.

The total pressure exerted by the mixture of equal moles of two gases is 5xx10^(3) Nm^(-2) in a container of volume 2 litres at 273 K. Calculate the number of the gases mixed.

One mole of gas A and three moles of a gas B are placed in flask of volume 100 litres at 27°C. Calculate the total partial pressure of the gases in the mixture.

Equal volume of all gases always contains equal number of moles.

The total pressure exerted by the mixture of non reactive gases is equal to the sum of the partial pressure of individual gases above statement represent the

A mixture of CH_(4), N_(2) and O_(2) is enclosed in a container of 1 litre capacity at 0^(@)C . Total pressure of gaseous mixture is 2660 mm Hg. If the ratio of partial pressures of the gases is 1 : 4 : 2 respectively, the number of moles of oxygen present in the vessel is:

STATEMENT-1 : Reacting gases react to form a new gas having pressure equal to the sum of their partial pressure. STATEMENT-2 : Pressure exerted by a mixture of non-reacting gases present in a container is equal to the sum of their partial pressures.

STATEMENT-1 : Reacting gases react to form a new gas having pressure equal to the sum of their partial pressure. STATEMENT-2 : Pressure exerted by a mixture of non-reacting gases present in a container is equal to the sum of their partial pressures.

If for a given volume and temperature, partial pressure of monatomic and diatomic gases maintain the ratio 3 : 2 then compare the number of moles of gases.