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 masses of O_(2), H_(2) and CH_(4) are taken in a container. The respective mole ration of these gases in container is:

Is Dalton's law of partial pressures valid for a mixture of SO_(2) and O_(2) ?

Equal masses of SO_(2), CH_(4) and O_(2) are mixed in empty container at 298 K, when total pressure is 2atm . The partial pressure of CH_(4) in the mixture is

Equal mass of O_2 and O_3 gases contain the same number of :

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

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

Find the value of K_(p) for the reaction : 2SO_(2)(g)+O_(2)(g) hArr 2SO_(3)(g) , if the partial pressures of SO_(2), O_(2) , and SO_(3) are 0.559 atm, 0.101 atm and 0.331 atm respectively. What will be the partial pressure of O_(2) gas if at equilibrium, equal amounts (in moles) of SO_(2) and SO_(3) are observed?

Find the value of K_(p) for the reaction : 2SO_(2)(g)+O_(2)(g) hArr 2SO_(3)(g) , if the partial pressures of SO_(2), O_(2) , and SO_(3) are 0.559 atm, 0.101 atm and 0.331 atm respectively. What will be the partial pressure of O_(2) gas if at equilibrium, equal amounts (in moles) of SO_(2) and SO_(3) are observed?