![A hydrocarbon has an empirical formula of CH2. Its density at r.t.p. is 0.001167 g/cm3. [1] a) Determine the molecular formula of the hydrocarbon. [1] b) Draw the structural formula of the hydrocarbon](/_next/image?url=https%3A%2F%2Fohijasnjvprzodcmxltt.supabase.co%2Fstorage%2Fv1%2Fobject%2Fpublic%2Fwhatsapp-images%2F1776696258136-1306b983d15fb148.png&w=3840&q=75)
This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
a) Determine the molecular formula of the hydrocarbon. Step 1: Calculate the empirical formula mass (EFM) of CH_2. The atomic mass of Carbon (C) is 12.0 and Hydrogen (H) is 1.0. EFM = (1 × 12.0) + (2 × 1.0) = 12.0 + 2.0 = 14.0 g/mol Step 2: Calculate the molar mass of the hydrocarbon using its density and molar gas volume at r.t.p. First, convert the density from g/cm^3 to g/dm^3. 1 dm^3 = 1000 cm^3 Density = 0.001167 g/cm^3 × 1000 cm^3/dm^3 = 1.167 g/dm^3 Now, calculate the molar mass (M). Molar Mass = Density × Molar Gas Volume Molar Mass = 1.167 g/dm^3 × 24 dm^3/mol = 28.008 g/mol Step 3: Determine the integer 'n' relating the molecular formula to the empirical formula. n = Molar MassEmpirical Formula Mass n = 28.008 g/mol14.0 g/mol = 2.00057 ≈ 2 Step 4: Determine the molecular formula. Molecular Formula = (Empirical Formula)_n Molecular Formula = (CH_2)_2 = C_2H_4 The molecular formula of the hydrocarbon is C_2H_4. b) Draw the structural formula of the hydrocarbon. The hydrocarbon is C_2H_4, which is ethene. It contains a carbon-carbon double bond. H & & H \\ | & & | \\ C & = & C \\ | & & | \\ H & & H 3 done, 2 left today. You're making progress.