An organic compound contains 54.55 % of carbon, 9.09 % of hydrogen and the remaining percentage of oxygen. The vapour density of the compound is 44 . The molecular formula of the compound is : (Given atomic masses : C = 12 u , H = 1 u , O = 16 u )

Step-by-step solution

Percentage of Oxygen = 100 - (54.55 + 9.09) = 36.36 % Calculation of relative number of moles: For C : 54.55 12 = 4.54 For H : 9.09 1 = 9.09 For O : 36.36 16 = 2.27 Simplest molar ratio (dividing by the smallest value, 2.27 ): C : 4.54 2.27 = 2 H : 9.09 2.27 = 4 O : 2.27 2.27 = 1 The empirical formula is C ₂ H ₄ O . Empirical formula mass = (2 12) + (4 1) + (1 16) = 44 u . Molar mass = 2 Vapour density = 2 44 = 88 g mol ⁻¹ . Multiplying factor n = Molar mass Empirical formula mass = 88 44 = 2 . Molecular formula =