Two gases A and B having molecular masses 60 and 45, respectively are enclosed in a vessel. The mass of A is 0.50 g and that of B is 0.2 g. The total pressure of the mixture is 750 mm. Calculate partial pressures of the two gases.

Two gases A and B having molecular weight 60 and 45 respectively are enclosed in a vessel. The weight of A is 0.5 g and that of B is 0.2 g. The total pressure of the mixture is 750 mm. Calculate the partial pressure (in mm) of gas A.

The total pressure of a mixture of two gases is:

A gaseous mixture contains 56 g of N_2 , 44 g CO_2 and 16 g of CH_4 The total pressure of the mixture is 720 mm Hg. The partial pressure of CH_4 is

4 g of O_2 and 2g of H_2 are confined in a vessel of capacity 1 litre at 0^@C . Calculate the partial pressure of each gas, and

A mixture of N_2 and Ar gases in a cylinder contains 7g of N_2 & 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27bar, the partial pressure of N_2 is:

Two gases A and B having the same pressure P, volume V and temperature T are mixed. If mixture has volume and temperature as V and T respectively, then the pressure of the mixture will be

The mass of 750 mL of a gas collected at 25°Cand 716.2 mm pressure is found to be equal to 0.809 g. Calculate the molecular mass of the gas.

4g of O_(2) and 2g " of " H_(2) are confined in a vessel of capacity 1 litre at 0^(@)C . Calculate the total pressure of the gaseous mixture.

If partial pressure of N_2 in gaseous mixture containing equal mass of CO and N_2 is 0.5 atm then the total pressure of gaseous mixture is

In a mixture of N_2 and CO_2 gases, the partial pressure of CO_(2) is 1.25 atm. The total pressure of the mixture is 5 atm. The mole fraction of N_(2) in the mixture is