Coniine, a toxic substance isolated from poison hemlock, contains only carbon, hydrogen, and nitrogen. Combus-tion analysis of a 5.024 mg sample yields 13.90 mg of CO2 and 6.048 mg of H2O. What is the empirical formula of coniine?

Verified step by step guidance

1. Determine the moles of carbon in the CO2 produced. Use the molar mass of CO2 (44.01 g/mol) and the fact that each mole of CO2 contains one mole of carbon.
2. Determine the moles of hydrogen in the H2O produced. Use the molar mass of H2O (18.02 g/mol) and the fact that each mole of H2O contains two moles of hydrogen.
3. Calculate the mass of carbon and hydrogen in the original sample using their respective moles and atomic masses (C: 12.01 g/mol, H: 1.008 g/mol).
4. Subtract the mass of carbon and hydrogen from the total mass of the sample to find the mass of nitrogen.
5. Convert the mass of nitrogen to moles using the atomic mass of nitrogen (N: 14.01 g/mol) and determine the simplest whole number ratio of moles of C, H, and N to find the empirical formula.

Key Concepts

Combustion Analysis

Combustion analysis is a technique used to determine the elemental composition of organic compounds. In this process, a sample is burned in excess oxygen, producing carbon dioxide and water. The masses of these products are measured, allowing for the calculation of the amounts of carbon and hydrogen in the original sample, which are essential for determining the empirical formula.

Empirical Formula

The empirical formula of a compound represents the simplest whole-number ratio of the elements present in that compound. It is derived from the moles of each element calculated from the combustion analysis data. This formula provides insight into the basic composition of the substance, although it may not reflect the actual molecular structure.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in chemical reactions. It involves using balanced chemical equations to calculate the amounts of substances consumed and produced. In the context of combustion analysis, stoichiometry helps convert the masses of CO2 and H2O produced into moles of carbon and hydrogen, which are crucial for determining the empirical formula.