`12gN_(2), 4gH_(2)` and `9gO_(2)` are put into a `1` L container at `27^(0)C` .What is the total pressure?

2.8 g of N_(2) 0.40 g of H_(2) and 6.4 g of O_(2) are placed in a container of 1.0 L capacity at 27^(@) C. The total pressure in the container is

Equal weight of N_(2) and O_(2) are put in a flask at 27^(@)C Calculate the partial pressure of N_(2) if partial pressure O_(2)=0.44 atm.

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?

2mol of N_(2) and 1mol of He are introduced into a 10L evacuated closed container at 27^(@)C .The pressure set up in the container will be

A mixture containing 1.6 g of O_(2) , 1.4 g of N_(2) and 0.4 g of He occupies a volume of 10 litres at 27^(@)C . Calculate the total pressure of the mixutre and partial pressure of each compound.

A sample of pure CuO was reduced with H_2 gas and H_(2)O formed was collected in a 44.8 L flask containing dry N_(2) . At 27^@C , the total pressure containing N_(2) and H_(2)O was 1.0 atm. The relative humidity in the flask was 80% The vapour pressure of water at 27^@C is 25 mm. How many grams of CuO was reduced?