A pure aliphatic hydrocarbon undergoes complete combustion with excess to yield precisely of and of — Qualitative and Quantitative Analysis Chemistry Question

💡 Solution & Explanation

First, find the moles of C and H. Moles of $C = \frac{\text{Mass of } CO_2}{44} = \frac{3.08}{44} = 0.07 \text{ mol}$. Moles of $H = 2 \times \frac{\text{Mass of } H_2O}{18} = 2 \times \frac{1.44}{18} = 2 \times 0.08 = 0.16 \text{ mol}$. The molar ratio of $C:H$ is $0.07 : 0.16$, which simplifies to the integer ratio $7 : 16$. The empirical formula is $C_7H_{16}$. The empirical formula mass is $(12 \times 7) + (1 \times 16) = 84 + 16 = 100 \text{ g/mol}$.