Question

A compound containing only carbon, hydrogen, and oxygen is analyzed using combustion analysis. When 55.5 g of the compound is burned, 98.9 g of carbon dioxide and 40.5 g of water are collected.

Given that there are 2.25 moles of carbon and 4.50 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

Determining an Empirical Formula from Combustion Data

Step-by-step explanation:

Step 1: Identify the mass of carbon dioxide and water produced by the combustion.

Step 2: Find how many moles of carbon are in carbon dioxide.

Step 3: Find how many moles of hydrogen are in water.