Please someone help

Question

Problem: 0.1156 g CxHyNz reacts with oxygen, O2, to give 0.1638 g CO2, 0.1676 g H2O, and N2. Find the empirical formula of the organic compound. CxHyNz + O2 → CO2 + H2O + N2 To determine the empirical formula you should know how much carbon, hydrogen, & nitrogen are each present in the sample. Follow the steps: Use dimensional analyses here. 1. Determine how much C is in CO2 then convert to mole. 2. Determine how much H is in H2O then convert to mole. 3. How do you think you can determine the amount of oxygen? 4. How do you think you can determine the amount of nitrogen?

Answer 1

Using dimensional analysis...

moles C = 0.1638 g CO2 x 1 mol CO2/44 g x 1 mol C/mol CO2 = 0.003723 moles C

moles H = 0.1676 g H2O x 1 mol H2O/18 g x 2 mol H/mol H2O = 0.01862 moles H

To find N, you can convert moles of C and moles of H to grams of C and grams of H, and subtract that from the initial mass of 0.1156 g to get grams of N. Convert g of N to moles of N. Since there is no oxygen in the original compound, you don't need to find the amount of oxygen.