Question

A compound containing only carbon, hydrogen, and oxygen is analyzed using combustion analysis. When 0.501 g of the compound is burned, 0.711 g of carbon dioxide and 0.436 g of water are collected.

Given that there are 0.0161 moles of carbon and 0.0484 moles of hydrogen produced in the reaction, calculate the mass of oxygen in the original compound. You will need to subtract the mass of the carbon that ended up in the carbon dioxide and the mass of the hydrogen that ended up in the water from the mass of the original compound.

Answer 1

To find the mass of oxygen in the original compound, the masses of carbon and hydrogen calculated from the moles given are subtracted from the total mass of the compound, resulting in 0.2588 g of oxygen.

Step-by-step explanation:

To calculate the mass of oxygen in the original compound, we start by subtracting the masses of carbon and hydrogen. From the combustion analysis, we know that the molar mass of carbon (C) is 12.01 g/mol and hydrogen (H) is 1.008 g/mol. With 0.0161 moles of carbon, the mass of carbon is 0.0161 moles × 12.01 g/mol = 0.1934 g.

For hydrogen, with 0.0484 moles, the mass is 0.0484 moles × 1.008 g/mol = 0.0488 g.

By subtracting the mass of carbon and hydrogen from the original mass of the sample, we can find the mass of oxygen: 0.501 g - (0.1934 g + 0.0488 g) = 0.2588 g of oxygen in the original compound.