Name: _______________________________ Date: _______________________________ Empirical and Limiting Reactant Dry Lab 1. Calculate the percent composition of each element in aspirin, C9H8O4 2. The drug,...

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Name: _______________________________ Date: _______________________________ Empirical and Limiting Reactant Dry Lab 1. Calculate the percent composition of each element in aspirin, C9H8O4 2. The drug, timolol, has a molecular mass of 432 g/mol. An elemental analysis shows that the drug is composed of 49.4% C, 7.64% H, 17.7% N, 15.2% O, and 10.1% S. What is the molecular formula for timolol? 3. Given that a compound contains 63.15% carbon, 31.55% oxygen and 5.3% hydrogen: What is its empirical formula? If its molecular weight is approx. 152.14 g/mol, what is its molecular formula? 4. Given that a compound contains 46.87 % iron, 17.33 % phosphorous and 35.81 % Oxygen and has a molecular mass of 357 g/mol. Calculate the empirical and molecular formulas. 5. What is the empirical formula of a compound that is 24.2 % Cu, 27.0 % Cl, and 48.8 % O? 6. If I have 5.3 mol of N2H4 how many moles of NH3 do I have, given the following balanced equation? 3N2H4 (l) → 4NH3 (g) + N2 (g) 7. Ammonia reacts with hydrogen chloride to produce ammonium chloride. Calculate the number of grams of ammonium chloride from a reaction of 3.0 g NH3 and 5.0 g HCl. ___NH3 (g) + ____HCl (g) → NH4Cl (g) 8. A chemist reacts 25.9 g of aqueous nickel (II) chloride with 10.0 g of aqueous sodium hydroxide to produce a solid in an aqueous solution. The reaction produced 9.5 g of the solid product. Write the chemical reaction and balance, calculate the theoretical yield, identify the limiting reactant, identify what type of reaction occurred and calculate the percent yield. 9. A reaction vessel contains 10.0 g of CO and 10.0 g of O2. How many grams of CO2 could be produced? 2CO (g) + O2 (g) → 2 CO2 (g) 10. Baking soda can be made in large quantities by the following reaction. If 10.0 g of sodium chloride reacts with excess of the other reactants and 4.2 g of baking soda (NaHCO3), is isolated, what is the percent yield of the reaction? NaCl (aq) + NH3 (aq) + CO2 (aq) + H2O (l) → NaHCO3 (s) + NH4Cl (aq) 11. If 0.154 g of Cu react with 0.483 g of AgNO3 to produce Ag. The actual amount of Ag produced was 0.299g. What is the percent yield of Ag according to the following equation? Cu (s) + 2AgNO3 (aq) → 2Ag (s) + Cu(NO3)2 (aq) 12. Silver nitrate solution reacts with calcium chloride solution to produce two products. One product forms a solid at the bottom of the beaker and the other is a solution. If 21.5 g of silver nitrate reacts with 8.40 g of calcium chloride. What is the theoretical yield of the solid product? Which of the two reactants is the limiting reagent? If the solid product has a mass of 8.69 g, what is the percent yield of the solid? 13. In a laboratory, a reaction of 0.598 g of lead (II) nitrate with 0.641 g of potassium iodide resulted in a precipitate. The amount of precipitate produced from the reaction was 0.748g. a. Complete and balance the chemical reaction. b. What type of reaction is in part (a) (2 answers) c. Calculate the theoretical yield and identify the limiting reactant? d. Calculate the percent yield?