Equal moles of each `H_2`, `CH_4`, and `SO_3`, are kept in a vessel A hole is made in vessel. After an hour the partial pressures of gases will be in the order of

0.5 mol of H_(2) , SO_(2) , and CH_(4) is kept in a container. A hole was made in the container. After 3 hours , the order of partial pressure in the container will be

Equal masses of He, O_(2) and SO_(2) are taken in a closed container. The ratio of the partial pressures of gases He, O_(2) and SO_(2) would be

Equal moles of each of SO_(3), CO_(2)O_(2) and H_(2) are kept in a container. A hole is made in the container and gasses are allowed to effuse. After 5 minutes the order of partial pressure of each gas in the container would be :

Equal moles of N_2 , H_2 and NH_3 are present in a container which are effusing from an orifice at temperature 27°C. After passing some time the correct order of their partial pressure in the container is

1 gram H_(2) and 8g O_(2) were taken in a 10 liter vessel at 300 K. The partial pressure exerted by O_(2) will be

Equal masses of the two gases A and B are kept in two separate vessels at the same temperature and pressure. If the ratio of the molecular masses of A and B is 2 : 3 , find the ratio of the volumes of the two vessels.

If the ration of the masses of SO_(3) and O_(2) gases confined in a vessel is 1 : 1 , then the ratio of their partial pressure would be

If the ration of the masses of SO_(3) and O_(2) gases confined in a vessel is 1 : 1 , then the ratio of their partial pressure would be

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

Equal mass of H_(2) , He and CH_(4) are mixed in empty container at 300 K, when total pressure is 2.6 atm The partial pressure of H_(2) in the mixture is