91- 6303239042
$$\% \text{ C} = \frac{12}{44} \times \frac{\text{Mass of } \text{CO}_2 \text{ formed}}{\text{Mass of Organic Compound}} \times 100$$
$$\% \text{ H} = \frac{2}{18} \times \frac{\text{Mass of } \text{H}_2\text{O} \text{ formed}}{\text{Mass of Organic Compound}} \times 100$$
A known mass of the organic compound is heated strongly with pure cupric oxide ($\text{CuO}$) in an atmosphere of dry oxygen. The carbon and hydrogen present in the compound are quantitatively oxidized to carbon dioxide ($\text{CO}_2$) and water ($\text{H}_2\text{O}$), respectively.
$$\text{C}_x\text{H}_y + \left( x + \frac{y}{4} \right) \text{O}_2 \xrightarrow{\text{CuO}, \, \Delta} x\text{CO}_2 + \frac{y}{2}\text{H}_2\text{O}$$
