On complete combustion 1.0 g of an organic compound (X) gave 1.46 g of ( CO ₂ ) and 0.567 g of ( H ₂ O ). The empirical formula mass of compound (( X ) ) is ________ g. (Given molar mass in ( g mol ⁻¹ C : 12, H : 1, O : 16 ))

Step-by-step solution

Moles of ' C ' (= n _ CO ₂ = 1.46 44 =0.033 ) Moles of ' C ' (= W _ C =0.033 12 ) Moles of 'H' (=2 n _ H ₂ O =2 0.567 18 =0.063 ) Mass of ' H ' (=0.0063 ) Mass of Oxygen (( O )=1- ( W _ c + W _ H ) ) (=1-(0.033 12+0.063 1)=0.541 gm ) Moles of ' O ' (= 0.541 16 =0.033 ) Empirical formula (= CH ₂ O ) Empirical formula mass (=30 ).