<p>Worksheet Name Empirical Formulas of Date ______Compounds</p><p>1. Calculate the empirical formula of a compound containing 43.6 % phosphorus and 56.33 % oxygen.</p><p>2. A certain compound contains 26.6 % potassium, 35.4 % chromium, & 38.1 % oxygen. What is its empirical formula?</p><p>3. The analysis of a compound gives: hydrogen = 3.06 %; phosphorus = 31.63 %; and oxygen = 65.30 %. Calculate its empirical formula.</p><p>4. A compound is formed when 5.58 g of iron metal combines with 3.21 g of sulfur. What is the empirical formula of this compound? 5. When 1.01 g of zinc is burned in air 1.26 g of zinc oxide are produced. What is the empirical formula of zinc oxide?</p><p>6. A compound contains 63.1 % C, 11.9 % H, and 25.0 % F; what is its empirical formula?</p><p>7. An organic compound was found on analysis to consist of 47.4 % C and 10.6 % H. The balance was presumed to be oxygen. What is the empirical formula of the compound?</p><p>8. A 3.245 g sample of titanium chloride was reacted with Na metal, producing NaCl and metallic titanium. After the NaCl was washed out the remaining titanium metal weighed 0.819 g. What is the empirical formula of the titanium chloride? (HINT: Determine how much chlorine was in the titanium chloride first.)</p><p>9. Many crystalline compounds, called "hydrates", contain water that can be removed when the compound is heated. The loss of weight upon heating can be used to determine the number of "waters of hydration" in the compound. A 1.222 g sample of a hydrate of barium chloride was heated until all of the water was expelled. The dry powder remaining weighed1.042 g. Calculate the number of water molecules present per each BaCl2.</p>