Compound X contains only carbon, hydrogen, nitrogen, and chlorine. When 1.00 g of X is dissolved in water and allowed to react with excess silver nitrate, AgNO3, all the chlorine in X reacts and 1.95 g of solid AgCl is formed. When 1.00 g of X undergoes complete combustion, 0.900 g of CO2 and 0.735 g of H2O are formed. What is the empirical formula of X?

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows chemists to calculate the amounts of substances consumed and produced in a reaction, based on balanced chemical equations. In this question, stoichiometry is essential for determining the moles of chlorine that reacted with silver nitrate and the moles of carbon and hydrogen produced during combustion.

The empirical formula of a compound represents the simplest whole-number ratio of the elements present in that compound. It is derived from the mass of each element in a sample and is crucial for understanding the composition of the compound. In this question, calculating the empirical formula involves determining the moles of carbon, hydrogen, nitrogen, and chlorine from the experimental data provided.

Combustion analysis is a method used to determine the elemental composition of organic compounds by burning the sample and measuring the resulting products, typically carbon dioxide and water. The masses of these products are used to calculate the amounts of carbon and hydrogen in the original compound. In this question, the combustion of compound X provides critical data needed to find the empirical formula by allowing the calculation of the moles of carbon and hydrogen present.