A mixture of one mole of each of `O_2(g), H_2(g)`, He(g) exists in a container of volume V at temperatureT in which partial pressure of `H_2` (g) is 2atm. the total pressure in the container is:

3g of H_(2) and 24g of O_(2) are present in a gaseous mixture at constant temperature and pressure. The partial pressure of hydrogen is

3g of H_(2) and 24g of O_(2) are present in a gaseous mixture at constant temperature and pressure. The partial pressure of hydrogen is

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

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

For a gaseous mixtue of 2.41g of helium and 2.79g of neon in an evacuated 1.04 dm^(3) container at 298 K Calculate the partial pressure of each gas and hence find the total pressure of the mixture.

A mixture in which the mole ratio of H_(2) and O_(2) is 2:1 is used to prepare water by the reaction. 2H_(2(g))+O_(2(g))rarr2H_(2)O_((g)) The total pressure in the container is 0.8 atm at 20^(@)C before the reaction. Determine the final pressure at 120^(@)C after reaction assuming 80% yield of water.

A mixture in which the mole ratio of H_(2) and O_(2) is 2:1 is used to prepare water by the reaction. 2H_(2(g))+O_(2(g))rarr2H_(2)O_((g)) The total pressure in the container is 0.8 atm at 20^(@)C before the reaction. Determine the final pressure at 120^(@)C after reaction assuming 80% yield of water.