A given mass of a hydrocarbon on complete combustion produced 176 ~g of CO ₂ and 90 ~g of H ₂ O . What is the Molecular formula of the compound?

Step-by-step solution

The combustion reaction of a hydrocarbon C_xH_y is given by: C_xH_y + (x + y 4 )O₂ xCO₂ + y 2 H₂O . Calculate the moles of CO₂ produced: n_ CO₂ = 176 g 44 g/mol = 4 mol . Calculate the moles of H₂O produced: n_ H₂O = 90 g 18 g/mol = 5 mol . From the stoichiometry of the reaction, the moles of carbon atoms in the hydrocarbon equals the moles of CO₂ , so x = 4 . The moles of hydrogen atoms in the hydrocarbon equals twice the moles of H₂O , so y = 2 5 = 10 . The molecular formula of the hydrocarbon is C₄H₁₀ . Answer: