M.E A sample contains only CaCO3 and KCl. CaCO3 decomposes upon heating according to the equation below. Determine the mass of CaCO3 in a 4.126 g sample that when heated decomposed to leave a residue with a mass of 3.645 g. CACO3 (s) – CaO (s) + CO2 (g) M to rodzy O3. When sandsto 2.

You are given a solid that is a mixture of Na2SO4 and K2SO4. A0.205 g sample of the mixture is dissolved in water. An excess of anaqueous solution of BaCl2is added. The BaSO4 that is formed isfiltered, dried, and weighed. Its mass is 0.298 g. What mass ofsulfate ions is in the sample? What is the mass percent of sulfate ionin the sample? What are the percent compositions by mass of thesodium sulfate and the potassium sulfate in the sample?

10. When the equation below is balanced, the coefficient in front of carbon dioxide is C3H8 + O2 --> CO2 + H2O: A. 1 B. 3 C. 6 D. 12

6. Mg(OH)2+ H3N-> Mg3N2 + heat a. Balance the reaction b. What is the reaction type? C. If 0.540 g of hydronitric acid react in the presence of excess magnesium hydroxide, what is the theoretical yleld of water produced in grams? d. If 1.32 g of water is actually produced, what is the percent yield? e. What is the percent error?