At room temperature ratio of pressures of `CH_(4)` and `CO_(2)` kept in two separate containers of equal volume is `3:5`. Then two containers have equal number of-

At the same temperature and pressure , equal volumes of different gases contain the same number of

Assertion (A): At 273K and 0.5 atms pressure, 1L of H_2 and 1L of CO_2 contain same number of molecules. Reason (R): Equal volumes of all gases contain equal number of molecules under the same conditions of temperature and pressure.

At room temperature and pressure, two flasks of equal volumes are filled with H_2 and SO_2 separately. Particles which are equal in number in two flasks are

S_(1) : Even at different temperature and pressure, equal volume of all the gases contains equal number of moles. S_(2) : 11.2 L CO_(2)(g) at STP contains the same number of free entity as 22.4 L O_(2)(g) at STP . S_(3) : If reacting species in a reaction are not taken in their stoichiometric coefficient ratio then one of the reactant will be limiting reagent. S_(4) : If two different solutions having different solute are mixed in certain volume proportion then resulting concentration of the components will decrease.

Equal mass of two gases A and B are kept in two separate containers under the same conditions of temperature and pressure. If the ratio of molar masses of A and B be 2:3, then what will be the ratio of volumes of the two containers?

Equal molar amount of H _(2), He having molecular weight of 2 and 4 respectively are filled at same temperature in two containers of equal volumes. If H_(2) gas has a pressure of 4 atmospheres, then He gas will have pressure as :-

Three flasks of equal volumes contain CH_(4),CO_(2), and Cl_(2) gases respectively. They will contain equal number of molecules if :