An organic compound contains `69%` carbon and `4.8%` hydrogen and the remaining is oxygen. Calculate the mass of `CO_2` and `H_2O` formed when 0.20 g of the compound is subjected to combustion?

An organic compound contains 49.3 % carbon 6.84 % hydrogen and its vapour density is 73. Molecular formula of the compound is

A compound contains 80% of carbon and 20% hydrogen. If the molecular mass is 30 calculate empirical formula and molecular formula.

An organic compound cọntains 69.77 %carbon, 11.63 % hydrogen and rest oxygen. The molecular mass of the compound is 86 . It does not reduce Tollens' reagent but forms an addition compound with sodiumhydrogensulphite and give positive iodoform test. On vigorous oxidation it gives ethanoic and propanoicacid. Write the possible structure of the compound.

An organic compoun0d contains 24.27% carbon, 4.07% hydrogen and 71.65% chlorine. Its molar mass is 98.96. Its empirical formula is

A compound contains 52.2% C and 13 % hydrogen and remaining percentage oxygen. If vapour density of the compound is 46, molecular formula is

An organic compound contains 40% carbon, 6.67% hydrogen and 53.33% oxygen by mass. What is the molecular formula of the compound if its molecular mass is 180?

An organic compound contains 20% carbon. It's vapour density is 120. The number of carbon atoms in one molecule of the compound is

Calculate the amount of CO_2 produced when 1 mole of carbon is burned in 16 g of O_2