Given : % of carbon = 69; % of hydrogen = 4.8 % of oxygen = 100 – (69 + 4.8) = 26.2 Mass of compound = 0.2 g 100 g of compound contains 69 g of C 0.2 g of compound contains $\frac{69 \times 0.2}{100}$ = 0.138 g of C Also, 12 g of C produces 44 g of $\mathrm{CO}_2$ ∴ 0.138 g of C will give = $\frac{44 \times 0.138}{12}$ = 0.506 g of $\mathrm{CO}_2$ 100 g of compound contains 4.8 g of H ∴ 0.2 g of compound contains $\frac{4.8 \times 0.2}{100}$ = 0.0096 g of H Also, 2 g of H produces 18 g of $\mathrm{H_2O}$ ∴ 0.0096 g of H produces $\frac{18 \times 0.0096}{2}$ g = 0.0864 g of $\mathrm{H_2O}$ Thus, mass of $\mathrm{CO}_2$ produced = 0.506 g and mass of $\mathrm{H_2O}$ produced = 0.0864 g