Practice question

Given: A compound burns in oxygen to produce 8.8 g of CO₂ and 3.6 g of H₂O. What is its empirical formula? (Atomic masses: C = 12, H = 1, O = 16) These values define the system as per NCERT data. Formula: Mass of C = (12 / 44) × 8.8 = 2.4 g. This is standard NCERT relation. Substitution & Calculation: Mass of H = (2 / 18) × 3.6 = 0.4 g. Moles: C = 2.4 / 12 = 0.2, H = 0.4 / 1 = 0.4. Ratio: 0.2 / 0.2 : 0.4 / 0.2 = 1 : 2. Empirical formula = CH₂. Result: The computed value matches expected outcome and confirms correct choice as per NCERT.