A five litre flask contains `3.5gm` of `N_(2), 3g` of `H_(2)` and `8g` of `O_(2)` at `27^(0)C` . The total pressure exerted by the mixture of these gases

A vessel of volume 4 litres contains a mixture of 8g of O_(2), 14g of N_(2) and 22 g of CO_(2) at 27^(0)C . The pressure exerted by the mixture is

A 1.0 L flask contains 2.0 g of N_(2), 0.4 g H_(2) and 9.0 of O_(2) at 27^(@)C . What is the pressure in the flask?

A vessel of volume 4 litres contains a mixture of 8 grams of O_(2) , 14 grams of N_(2) and 32 grams of SO_(2) at 27^(@) C . Find the pressure exerted by the mixture. Given, R = 8.3 J mol_(-1) K_(-1) .

1g H_(2), 2g He and 3g NO are contained in 1.1 L flask at 300 K. Total pressure exerted by the mixture is :

A container of 1 L capacity contains a mixture of 4 g of O_(2) and 2 g H_(2) at 0 ^(@)C . What will be the total pressure of the mixture ?

In a flask of volume 8.2 litres there is a mixture of "1" mole of N_(2) and 1 mole of He at 27^(@)C .The pressure exerted by the mixture in atmospheres is (R=0.082L atm K^(-1)mol^(-1))

A 5.0 L flask contains 19.5 g of SO_(3) and 1.0 g of He gas at 20^(@)C . Calculate the partial pressures exerted by SO_(3) and He and the total pressure of the gaseous mixture.

2.802 g of N_(2) gas is kept in one litre flask at 0^(@)C . Calculate the pressure exerted by the gas.