A container of volume V, contains `0*28` g of `N_(2)` gas. If same volume of an unknown gas under similar conditions of temperature and pressure weighs `0*44` g, the molecular mass of the gas is

A bag contains 0.32 g of oxygen. The same valume of an unknown gas A under similar conditions of temperature and pressure weigh 0.26 g . The gas A is known to contain only C and H in 1:1 ratio. The molecular formula of the compound is

A bag contains 0.32 g of oxygen. The same valume of an unknown gas A under similar conditions of temperature and pressure weigh 0.26 g . The gas A is known to contain only C and H in 1:1 ratio. The molecular formula of the compound is

A gas cylinder full of hydrogen gas contains 6 g of this gas. The same cylinder can hold 102 g of a gas X under the same conditions of temperature and pressure. Calculate the vapour density of the gas X

Assertion : Equal volumes of all gases under similar conditions of temperature and pressure contain equal number of molecules Reason : Volume of a gas is inversely proportional to pressure

10L of a gas at 0^(@)C and 760 mm pressure weighs 13.39g. Under identical conditions of temperature and pressure, ass of 10 L of hydrogen is 0.8928g. What is the molecular mass of the gas?

A certain volume of argon gas (Mol. Wt.=40) requires 45s to effuse through a hole at a certain pressure and temperature. The same volume of another gas of unknown molecular weight requires 60s to pass through the same hole under the same conditions of temperature and pressure. The molecular weight of the gas is: