n:A composition of an organic compound is found to CONTAIN 39.9 % of CARBON, 6.7% of hydrogen and remaining being oxygen. The molar mass of the compound is 180. Determine its empirical FORMULA and molecular formula.Answer: Empirical formula of the compound = CH₂O Molecular formula = C₆H₁₂O₆Explanation:Mass of carbon = 39.9 gMass of hydrogen = 6.7 gMass of oxygen = (100 - (39.9 + 6.7) ) = 53.4 gEmpirical formulaMolecular formula➟ First we have to find the number of moles of each element present in the compund.➟ The number of moles of a given compound is given by,     Number of moles = Given mass/Molar mass➟ Number of moles of carbon = 39.9/12     Number of moles of carbon = 3.325 moles➟ Number of moles of hydrogen = 6.7/1     Number of moles of hydrogen = 6.7 moles➟ Number of moles of oxygen = 53.4/16     Number of moles of oxygen = 3.34 moles➟ Now we have to find the simplest whole number ratio of all the ELEMENTS.     Simplest whole number ratio of carbon = 3.325/3.325 = 1     Simplest whole number ratio of hydrogen = 6.7/3.325 = 2     Simplest whole number ratio of oxygen = 3.34/3.325 = 1➟ Hence,     Empirical formula of the compound = CH₂O➟ Now we have to find the molecular mass of the compund.     Molecular mass = 12 + 2 + 16 = 30➟ Now we know that,     Molar mass/Molecular mass = n     n = 180/30     n = 6➟ We know that,     Molecular formula = n × Empirical formula     Molecular formula = 6 × CH₂O     Molecular formula = C₆H₁₂O₆