A gaseous compound is composed of `85.7%` by mass carbon and `14.3%` by mass hydrogen. Its density is `2.28` g/litre at `300 K and 1.0` atm pressure. Determine the molecular formula of the compound.

8.2 L of an ideal gas weights 9.0 g at 300 K and 1 atm pressure. The molecular mass of the gas is

7.00 g of a gas occupies a volume of 4.1 L at 300 K and 1 atm pressure. What is the molecular mass of the gas?

A pure gas that is 14.3% hydrogen and 85.7% carbon by mass has a density of 2.5g L^(-1) at 0^(@)C and 1 atm pressure. What is the molecular formula of the gas :

A gaseous organic compound has a density of 2.5 kg//m^3 at 2 atm and at 273^@C .The molecular formula of the compound can be :

A compound X consists of 4.8% carbon and 95.2% bromine by mass. If the vapour density of the compound is 252, what is the molecular formula of the compound?

A compound has the following percentage composition by mass : Carbon = 54.55%, Hydrogen = 9.09% and Oxygen = 36.26%. Its vapour density is 44. Find the Empirical and molecular formula of the compound. (H = 1, C = 12,0 = 16)

An oxygen containing organic compound was found to contain 53% carbon and 13% hydrogen. Its vapour density is 23. The compound reacts with sodium metal to liberate hydrogen. Identify the functional isomer of this compound.

A compound on analysis gave the follwing result C=54.54%, H=9.09% and vapour density of compound = 88.Determine the molecular formula of the compound.

A compound is composed of 2.2% hydrogen, 26.6% carbon and 71.2% oxygen. Calculate the empirical formula of the compound. If its molecular mass is 90, find its molecular formula.

A hydrocarbon contains 85.7% carbon. If 42 mg of the compound contain 3.01 xx 10^20 molecules, find the molecular formula of the compound.