HN Study Guide Stoich

Calculations with stoichiometry. Remember that 1mol=22.4L at STP and 1mol=6.02x1023 particles Part 1: Back to the basics (in case you forgot) 2 DECIMAL PLACES AND A UNIT OF g/mol Give the molar masses for the following substances Aluminum hydroxide Calcium carbonate Sulfur pentafluoride Dihydrogen monoxide Iron (III) oxide Zinc acetate Ammonium sulfate Part 2: Stoichiometry Calculations (on the test, they will not be separated by one calculation stoich and LR) 1. Given the following equation: K + Cl2 ---> KCl How many moles of KCl are produced from 1.5 moles of K. From 1.00 moles of Cl2 how many moles of KCl can you form? 2. Given the following equation: Na2O + H2O ---> NaOH How many moles of NaOH are produced from 3.0 moles of Na2O? How many moles of Na2O are required to produce 1.60 x 102 grams of NaOH? 3. Given the following equation: Fe + S8 ---> FeS What mass of iron is needed to react with 16.0 grams of sulfur? 4. Given the following equation: NaClO3 ---> NaCl + O2 12.00 moles of NaClO3 will produce how many grams of O2? How many grams of NaCl are produced when 80.0 grams of O2 are produced? 5. Given the following equation: Cu + AgNO3 ---> Cu(NO3)2 + Ag How many moles of Cu are needed to react with 3.50 moles of AgNO3? If 89.5 grams of Ag were produced, how many grams of Cu reacted? 6. Given the reaction: NH3 (g) + O2 (g) ---> NO (g) + H2O (l) How many liters of NO will you produce if you start with 35.0g of oxygen at STP? If you start with 540mL at STP, how many grams of NH3 will you produce? How many molecules of water will you produce if you start with 56.1 grams of NH3 and an excess of oxygen? Part 3: Limiting reactant and Percent Yield Sodium chloride can be prepared by the reaction of sodium metal and chlorine gas. What is the limiting reactant ? How many moles of NaCl are produced? How much of the excess reactant remains unreacted? Hydrogen gas can be produced in the laboratory by the reaction of magnesium metal with hydrochloric acid. Calcium carbonate is decomposed by heating to form calcium oxide and carbon dioxide gas. If 19 g of zinc are reacted with 19 g magnesium chloride, zinc chloride and magnesium are formed. Which reactant will be in excess ? Calculate the mass of the zinc chloride produced. Calculate the mass of the excess reactant that remains unreacted. Nitrogen gas can be prepared by passing gaseous ammonia over solid copper (II) oxide at high temperatures. The other products of the reaction are solid copper and water vapor. Which is the limiting reactant? How many grams of N 2 will be formed? If only 8.2 grams N 2 are actually formed during the experiment, what is the percent yield? 6. A reaction container holds 5.77 g of P4 and 5.77 g of O2. The following reaction occurs: P4 + O2 ? P4O6. a. What is the limiting reagent for the formation of P4O6? b. What mass of P4O6 is produced? c. What mass of excess reactant is left in the reaction container? 7. Aluminum has a density of 2.7g/mL. In the reaction ____ Al + ____ Cl2? ____ AlCl3 a. What’s the limiting reactant when 20.5g of Al reacts with 20.5g Cl2 ? b. How many grams of aluminum chloride will be made? c. If you start with 0.0250 L Al, how many grams is that? d. To produce 2.50 grams of product, you would need how many milliliters of aluminum?