A hydrocarbon contains 10.5 g of carbon and 1g of hydrogen. The weight of 1 litre of the hydrocarbon at `127^(@)C` and 1 atm pressure is 2.8g. Determine the molecular formula of the compound.

The weight of 1 litre of a gas at 27^(@) and 600 mm pressure is 0.8g. What is its vapour density and molecular weight?

A gaseous compound is composed of 85.7% by mass of carbon and 14.3% by mass hydrogen. Its density is 2.28 g/L at 300 K and 1 atm pressure. Determine molecular formula of the compound.

The weight of 350 mL of a diatomic gas at 0^(@)C temperature and 2 atm pressure is 1g. Calculate the weight of its one atom.

A compound of carbon, hydrogen and oxygen contains 40% of carbon and 6.67% of hydrogen. Vapour density of the compound is 2.813 times of the vapour density of oxygen. Determine the empirical formula and molecular formula of the compound.

The gaseous compound is composed of 85.7% C by w//W & 14.3% by mass hydrogen. It's density id 2.28 gm//litre at 300 K and and 1 atm pressure. Determine molecular formula of the compound.

Determine the value of 2.2 g of carbon dioxide at 27^(@)C and 570 mm Hg pressure.

The percentage of carbon and hydrogen in an organic compound are 92.5 and 7.5. Determine the'molecular formula of the compound if its vapour density is 39.

An organic compound contains C, H and oxygen. 0.30 g of this compound on combustion yielded 0.44 g of CO_2 and 0.18 g of H_2O .If the weight of 1 mole of the compounds is 60, what is the molecular formula of the organic compound.?

At a temperature of 273K and 1 atm pressure 1L of a gas weighs 2.054g. Calculate its molecular mass.

An organic compound, consisting of carbon, hydrogen, nitrogen and oxygen contains 40.67% of carbon and 8.47% of hydrogen 0.5g of that compound gives 94.91mL of nitrogen at STP. What is the empirical formula of that compound?