Chapter 11 Review 1) What does stoichiometry mean? 2) Before performing a stoichiometry problem, you must first do what with the chemical equation? 3) The coefficients in a chemical equation represent what? 4) In a chemical equation, what relationships are shown? 5) Solve the following mole-mole conversions using this equation: 2NaHCO3 ď § Na2CO3 + CO2 +
a) If 3.5 moles of sodium bicarbonate (NaHCO3) are decomposed, how many moles of carbon dioxide are produced?
b) If 1.29 moles of water are produced by the decomposition of sodium bicarbonate, how many moles of sodium carbonate (Na2CO3) are produced?
c) How many moles of sodium bicarbonate are required to produce 19.5 moles of carbon dioxide?
6) Use the equation in # 5 to solve the following mass-mass conversions. a) If given 10.5 grams of sodium bicarbonate, how many grams of sodium carbonate can be produced?
b) How many grams of sodium bicarbonate would be required to produce 9.0 grams of water?
7) What conversion factor(mole ratio) would you use to solve for moles of sulfur formed from sulfur dioxide in the reaction SO2 â†’ S + O2
8) If 9.65 grams of sodium react with 2.5 grams of chlorine, how much sodium chloride will be produced? Equation: 2Na + Cl2 2NaCl (get the limiting reactant first)
9) Identify the limiting reactant when 5.1 g of lithium react with 1.5 mol of fluorine gas at STP to produce lithium fluoride. 2Li + F2 2LiF
10) If in a reaction involving the production of water, you are able to theoretically produce 25.0 grams of water but experimentally you were actually only able to produce 18.5 grams of water, what is the percent yield of water from your experiment?
11) Determine the percent yield for the reaction between 6.92 g of potassium and 4.28 g of oxygen gas if 7.36g of K2O is produced? 4K + O2 2K2O Step 1: Find limiting reactant
Step 2: Solve for theoretical amount of product using the limiting reactant.
Step 3: Solve for percent yield.
12) Define limiting reactant.
13) Define excess reactant.
Published on May 30, 2012