Question

a sample of organic compound containing carbon and hydrogen burns in excess oxygen to yield 8.8g of co2 and 5.4g of H2O.What is the empirical formula of the compound ​

Answer 1

To find the empirical formula of the organic compound, the moles of carbon and hydrogen are calculated from the masses of CO2 and H2O produced by combustion. These moles are then simplified to the smallest whole number ratio, resulting in an empirical formula of CH3.

Step-by-step explanation:

To determine the empirical formula of the organic compound based on the provided information, we must first convert the masses of CO2 and H2O to moles. Since CO2 contains one carbon atom, we can find the amount of carbon in the sample. Also, H2O contains two hydrogen atoms, which lets us find the amount of hydrogen.

We are given:

• Mass of CO2 = 8.8 g
• Mass of H2O = 5.4 g

Using the molar masses of CO2 (44.01 g/mol) and H2O (18.02 g/mol), we calculate the moles:

• For CO2: 8.8 g / 44.01 g/mol = 0.2 moles of CO2 (hence 0.2 moles of C)
• For H2O: 5.4 g / 18.02 g/mol = 0.3 moles of H2O (hence 0.6 moles of H)

Next, we find the simplest mole ratio of C to H by dividing by the smallest number of moles:

1. Carbon: 0.2 moles / 0.2 = 1
2. Hydrogen: 0.6 moles / 0.2 = 3

Therefore, the empirical formula of the compound is CH3.