On complete combustion 1.0 g of an organic compound (X) gave 1.46 g of CO2 and 0.567 g of H2O. The empirical formula mass of compound (X) is

Empirical Formula Mass Numerical – JEE Main PYQs | Combustion Analysis

On complete combustion 1.0 g of an organic compound (X) gave 1.46 g of CO₂ and 0.567 g of H₂O. The empirical formula mass of compound (X) is ______ g.

Given: Molar mass (in g mol⁻¹) C = 12, H = 1, O = 16

A. 60
B. 45
C. 30
D. 15

Step 1: Calculate moles of CO₂ formed

Moles of CO₂ = 1.46 / 44 = 0.03318 moles

Step 2: Calculate moles of carbon

Moles of carbon = 0.03318 moles

Step 3: Calculate moles of H₂O formed

Moles of H₂O = 0.567 / 18 = 0.0315 moles

Step 4: Calculate moles of hydrogen

Moles of hydrogen = 2 × 0.0315 = 0.063 moles

Step 5: Calculate mass of carbon and hydrogen

Mass of C = 0.03318 × 12 = 0.398 g
Mass of H = 0.063 × 1 = 0.063 g

Step 6: Calculate mass and moles of oxygen

Mass of O = 1.0 − (0.398 + 0.063) = 0.539 g
Moles of O = 0.539 / 16 = 0.0337 moles

Step 7: Find simplest mole ratio

C : H : O = 0.033 : 0.063 : 0.0337
Divide by smallest value (≈ 0.033)
≈ 1 : 2 : 1

Step 8: Determine empirical formula and mass

Empirical formula = CH₂O
Empirical formula mass = 12 + 2 + 16 = 30 g

✅ Final Answer: 30 g

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