Question

An unknown compound contains only carbon, hydrogen, and oxygen (CxHyOz). Combustion of 2.50 g of this compound produced 3.67 g of carbon dioxide and 1.50 g of water. How many moles of hydrogen, H, were in the original sample?

Answer 1

The original sample contains 0.1666 moles of hydrogen (H).

Step-by-step explanation:

Based on the given information, we can determine the number of moles of carbon and hydrogen in the original sample.

First, we need to calculate the number of moles of carbon dioxide (CO2) produced. We know that the molar mass of CO2 is 44.01 g/mol. So, 3.67 g of CO2 is equal to 3.67 g / 44.01 g/mol = 0.0834 mol.

Next, we need to calculate the number of moles of water (H2O) produced. We know that the molar mass of H2O is 18.02 g/mol. So, 1.50 g of H2O is equal to 1.50 g / 18.02 g/mol = 0.0833 mol. Since 1 mol of H2O contains 2 moles of hydrogen (H), the original sample contains 2 x 0.0833 mol = 0.1666 mol of hydrogen.

Therefore, there are 0.1666 moles of hydrogen (H) in the original sample.