A compound containing only carbon, hydrogen, and oxygen has a molar mass of approximately 90 g/mol. Combustion analysis of 0.405 g of the compound produces 0.54 g $CO_2$ and 0.27 g $H_2O$. If the compound's empirical formula is the same as its molecular formula, what is the number of oxygen atoms in one molecule of the compound?

If a compound consists of 92.3% carbon and 7.7% hydrogen by weight, what is its empirical formula? (Atomic weights: C = 12, H = 1)

An organic compound having molecular mass 60 is found to contain C=20%, H=6.67% and N=46.67% while rest is oxygen. On heating it gives ${\rm{N}}{{\rm{H}}_3}$ along with a solid residue. The solid residue gives violet colour with alkaline copper sulphate solution. The compound is

An organic compound is found to contain 40% carbon, 6.67% hydrogen, and 53.33% oxygen by weight. What is the empirical formula of this compound? (Atomic weights: C=12, H=1, O=16)

A hydrocarbon contains 85.7% carbon. Its molecular mass is 42. The molecular formula of the compound is:

Which of the following pairs has the same empirical formula?

A compound contains 40% carbon, 6.67% hydrogen, and 53.33% oxygen. Its empirical formula is:

A compound has the molecular formula C$_2$H$_4$O$_2$. What is its empirical formula?

A Carbon compound contains 12.8 % Carbon, 2.1 % Hydrogen and 85.1 % of Bromine. The molecular weight of the compound is 187.9. Its molecular formula is (at. Wt. of Br = 80)

What is the empirical formula of a compound having 40% carbon, 6.66% hydrogen and 53.34% oxygen?

Empirical formula of glucose is