A compound containing the elements C, H, N, and O is analyzed. When a 1.2359g sample is burned in excess oxygen, 2.241g of CO2(g) is formed. The combustion analysis also showed that the sample contained 0.0648g of H. i) determine the mass, in grams, of C in the 1.2359g sample of the compound. ii) when the compound is analyzed for N content only, the mass percent of N is found to be 28.84 percent. Determine the mass, in grams, of N in the original 1.2359g sample of the compound. iii) Determine the mass, in grams, of O in the original 1.2359g sample of the compound. iv) Determine the empirical formula of the compound.

1.   If 23.0 g of nitrogen gas are available with 24.0 g of hydrogen gas, then how many grams of ammonia gas (NH3) can they produce in a synthesis (combination) reaction?   ______ g NH3 (just type the number with correct significant figures).   2.   Suppose you have 8.000 grams of solid magnesium and 621.000 grams of CuCl2 (molar mass 134.45 g/mol) dissolved in water. You get a chemical reaction in which solid copper forms.   Figure out which is the limiting reactant, and then use that to figure out:   how much solid copper can you form (theoretical yield)?   ______ g Cu   3. Suppose you have 990.0 grams of barium chloride dissolved in water and 204.0 grams of aluminum sulfate dissolved in water. How many grams of the aqueous product can you make (not including the mass of the water)?     Please provide only typed answer solution no handwritten solution needed allowed

SO2(g) + H2O(l) → H2SO3(g) Given an initial mass of 14.12 g SO2, an excess of H2O, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of H2SO3 produced by the reaction.

An organic compound X was found to contain only C, H, and Cl.  The following experiments were carried out with compound X: 1) When a 1.50-g sample of the compound was completely combusted in air, 3.52 g CO2 was formed. 2) When a 1.00-g sample of the compound was allowed to react with an excess of Ag, 1.27 g of AgCl was obtained.Determine the empirical formula of compound X. C9H4Cl C6H4Cl2 C9H6Cl C3H2Cl2 C6H5Cl