The active mass of `64 g` of `HI` in a `2-L` flask would be

Active mass of 5.6 g CaO(s) is

The active mass of 7.0 g of nitrogen in a 2.0 L container would be

Active mass of 0.64g SO_(2) in 10 lit vessel is

Four flask of 1 litre capacity each are separately filled with gases H_2,He,O_2 and O_3 . At the same temperature and pressure, the ratio of the number of atoms of these gases present in different flask would be :

The value of K_(c) for the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) is 64 at 773K . If one "mole" of H_(2) , one mole of I_(2) , and three moles of HI are taken in a 1 L flask, find the concentrations of I_(2) and HI at equilibrium at 773 K .

Two flasks X and Y have capacity 1 L and 2 L respectively and each of them contains 1 mole of a gas. The temperature of the flasks are so adjusted that average speed of molecules in X is twice as those in Y. The pressure in flask X would be

Four one litre flaske are separately filled with the gases H_(2), He, O_(2) "and" O_(3) at the same temperature and pressure. The ratio of total number of atoms of these gases present in different flask would be:

For the reaction CO(g) +2H_2(g) hArr CH__3OH(g) . If active mass of CO is kept constant and active mass of H_2 is tripled, the rate of of forward reaction will become

The partial pressure of hydrogen in a flask containing 2 g of H_(2) and 32 g of SO_(2) is

The value of K_(c) for the reaction: H_(2)(g)+I_(2)(g) hArr 2HI (g) is 48 at 773 K. If one mole of H_(2) , one mole of I_(2) and three moles of HI are taken in a 1L falsk, find the concentrations of I_(2) and HI at equilibrium at 773 K.