At same temperature and pressure,the fraction of masses having equal volumes of `O_2` `SO_3`
2:1
2:5
1:2
1:1

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.

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 :

Samples of the gases O_(2), N_(2), CO_(2) and CO under the same conditions of temperature and pressure contain the same number of molecules represented by X. The molecules of oxygen (O_(2)) occupy V litres and have a mass of 8 g. Under the same conditions of temperature and pressure, answer the following questions: What is the volume occupied by 3X molecules of CO?

Samples of the gases O_(2) ,N_(2), CO_(2) and CO under the same conditions of temperature and pressure contain the same number of molecules represented by X. The molecules of oxygen (O_(2)) occupy V litres and have a mass of 8 g. Under the same conditions of temperature and pressure, answer the following questions: What is the volume occupied by X moelcules of N_(2)

A mixture of two gases A and B in the mole ratio 2:3 is kept in a 2 litre vessel. A second 3 litre vessel has the same two gases in the mole ratio 3:5 . Both gas mixtures have the same temperature and same pressure. They are allowed to intermix and the final temperature and pressure are the same as the initial values, the final volume beingh 5 litres. Given theat the molar masses are M_(A) and M_(B) . what is the mean molar mass of the final mixture :

Samples of the gases O_(2), N_(2), CO_(2) and CO under the same conditions of temperature and pressure contain the same number of molecules represented by X. The molecules of oxygen (O_(2)) occupy V litres and have a mass of 8 g. Under the same conditions of temperature and pressure, answer the following questions: What is the mass of CO_(2) in gram ?

60ml of mixture of equal volumes of Cl_(2) and an oxide of chlorine, i.e., Cl_(2)O_(n) was heated and then cooled back to the original temperature. The resulting gas mixture was found to have volume of 75ml . On treatment with KOH solution, the volume contracted to 15ml . Assume that all measurements are made at the same temperature and pressure. Deduce the value of n in Cl_(2)O_(n) . The oxide of Cl_(2) n heating decomposes quantiatively to O_(2) and Cl_(2) .

Assertion: Under similar conditions of temperature and pressure, O_(2) diffuses 1.4 times faster than SO_(2) . Reason: Density of SO_(2) is 1.4 times greater than that of O_(2) .

N_(2)O_(3) dissociates into NO and NO_(2) . At equilibrium pressure of 3 atm , all three gases were found to have equal number of moles in a vessel. In another vessel, equimolormixture of N_(2)O_(3), NO and NO_(2) are taken at the same temperature but at an initial pressure of 9 atm then find the partial pressure of NO_(2) (in atm ) at equilibrium in second vessel! N_(2)O_(3)(g) hArr NO(g) + NO_(2) (g)

Samples of the gases O_(2), N_(2), CO_(2) and CO under the same conditions of temperature and pressure contain the same number of molecules represented by X. The molecules of oxygen (O_(2)) occupy V litres and have a mass of 8 g. Under the same conditions of temperature and pressure, answer the following questions: In answering the above questions, name the law you have used?