A compound contains Carbon and Hydrogen which on burning in Oxygen gives 3.38g of CO2 and 0.690 g of H2O. Calculate the percentage composition of the compound. (H=1u , C=12u

Answer 1

A compound contains Carbon and Hydrogen which on burning in Oxygen gives 3.38g of CO2 and 0.690 g of H2O. Calculate the percentage composition of the compound. (H=1u , C=12u

Convert the 3.38g CO₂ into grams of Carbon using the ratio of 1 carbon per molecule of CO₂:

3.38g CO₂ * 1mol CO₂ / 44g * CO₂ * 1mol C / 1 mol CO₂ * 12g / 1 mol C = o.921 g C

Convert the 0.690g H₂O into grams of Hydrogen using the ratio of 2 hyrogen per molecule of H₂O:

0.690g H₂O * 1mol H₂O / 18g H₂O * 2mol H / 1 mol H₂O * 1g / mol H = 0.0767 g H

Percent Composition Carbon:

0.921g C / (0.921g C + 0.0767g H) = 0.923 or 92.3% C

Percent Composition Hydrogen:

0.0767g C / (0.921g C + 0.0767g H) = 0.0768 or 7.68% H