The total pressure of a gaseous mixture of `2.8 g N_(2)`, `3.2 g O_(2)`, and `0.5 g H_(2)` is `4.5 atm`. Calculate the partial pressure of each gas.

In a ten litre vessel, the total pressure of a gaseous mixture containing H_(2), N_(2) and CO_(2) is 9.8atm. The partial pressures of H_(2) and N_(2) are 3.7 and 4.2 atm respectively. Then the partial pressure of CO_(2) is

In a ten litre vessel, the total pressure of a gaseous mixture containing H_(2), N_(2) and CO_(2) is 9.8atm. The partial pressures of H_(2) and N_(2) are 3.7 and 4.2 atm respectively. Then the partial pressure of CO_(2) is

The total pressure of a mixture of 604 g of O_(2) and 5.6 g of N_(2) present in a 2 L vessel is 1200 mm. What is the partial pressure (in mm) of nitrogen ?

A 2L flask contains 0.4 g O_(2) and 0.6 g H_(2) at 100^(@)C . Calculate the total pressure of the gas mixture in the flask.

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

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

If the pressure of a mixture of 56 g of N_(2) and 44.0 g CO_(2) is 3 atm , the partial pressure of N_(2) in the mixture is :