True or False. It is possible to find the empirical formula for a compound with the elements carbon, hydrogen, oxygen, and chlorine via combustion analysis.

Sample X has a molecular weight of 378.29 g and only contains C, H, and Cl. If 1.12 g X produces 1.57 g CO₂ and 0.56 g H₂O after combustion analysis, what is the molecular formula?

Only carbon, hydrogen, nitrogen, and chlorine are present in compound X. When excess silver nitrate (AgNO₃) is added to 1.52 g of X after it has been dissolved in water, all of the chlorine in X reacts, forming 3.01 g of solid AgCl. Complete combustion of 1.52 g of X results in the formation of 1.39 g of CO2 and 0.95 g of H2O. Identify the empirical formula of X.

In an experiment, 2.35 g of sample was combusted and produced 1.10 g of NO₂. In another experiment, 2.67 g of the same sample was converted to 5.00 g of PbBr₂. What is the empirical formula of the sample if it is only composed of N, H, and Br?

Calculate the empirical formula of a compound that only contains C, H, O, and F. 

A 7.03 g sample has undergone combustion and produced 13.0 g CO₂ and 4.26 g H₂O. 

A second sample of the compound that weighs 6.13 g is found to contain 0.98 g F.