Question

A compound containing Carbon, Nitrogen, and Oxygen gave the following data on analysis: 0.1g of the compound on combustion gave 0.228g of CO₂ and 0.124g of H₂O. On further analysis 0.1g of the compound gave NH₃ which required 17.2 cm of 0.1M HCl for neutralization.

How many moles of carbon, Hydrogen and Nitrogen are there in 0.1g of the compound?

Answer 1

To determine the moles of carbon, hydrogen, and nitrogen in the compound, calculate the moles of CO₂ and H₂O produced from the combustion analysis, and the moles of NH₃ produced from further analysis. Use stoichiometry to determine the moles of carbon and hydrogen, and subtract those from the total moles to find the moles of nitrogen.

Step-by-step explanation:

The compound consists of Carbon, Nitrogen, and Oxygen. To determine the moles of carbon, hydrogen, and nitrogen in the compound:

Step 1: Calculate the moles of CO₂ produced from the combustion. Convert the mass of CO₂ (0.228g) to moles using the molar mass of CO₂ (44.01 g/mol).

Step 2: Calculate the moles of H₂O produced from the combustion. Convert the mass of H₂O (0.124g) to moles using the molar mass of H₂O (18.02 g/mol).

Step 3: Calculate the moles of NH₃ produced from the further analysis. Convert the volume of HCl used for neutralization (17.2 cm³) to moles using the concentration of HCl (0.1M).

Step 4: Use the stoichiometry of the combustion reaction to determine the moles of Carbon and Hydrogen in the compound.

Step 5: Calculate the moles of Nitrogen in the compound by subtracting the moles of Carbon and Hydrogen from the total moles of the compound.