CH. 12 STOICHIOMETRY
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1 CH. 12 STOICHIOMETRY
2 Balanced Chemical Equations Used to calculate: How much of each reactant is needed How much product will form If you know one quantity you can calculate the rest. Quantity may be in atoms, molecules, moles; mass (g) and/or volume (L)
3 Conversion Factors Mass: molar mass is in g/mol Find by adding the atomic masses of each atom Volume: gases at STP have a volume of 22.4 L/mol Mol to molecules: 6.02 x 1023 molecules/mol
4 Practice 1 A. B. C. D. NH3(g) + O2(g) NO(g) + H2O (g) CuO(s) + NH3(aq) Cu(s) + H2O(l) + N2(g) K(s) + H2O(l) KOH(l) + H2(g) C2H5OH(l) + O2(g) CO2 (g) + H2O(g) 1. Balance the equations above. 2. Determine the number of moles of each compound. 3. Calculate the mass of each compound. 4. For gases, also determine the volume at STP.
5 Practice 1 A. B. C. D. 4NH3(g) + 5O2(g) 4NO(g) + 6H2O (g) 3CuO(s) + 2NH3(aq) 3Cu(s) + 3H2O(l) + N2(g) 2K(s) + 2H2O(l) 2KOH(l) + H2(g) C2H5OH(l) + 3O2(g) 2CO2 (g) + 3H2O(g) 1. Balance the equations above. 2. Determine the number of moles of each compound. 3. Calculate the mass of each compound. 4. For gases, also determine the volume at STP.
6 12.2 Chemical Calculations Mole ratios: determined from the balanced chemical equation (interpreted in mol) Example: in the balanced chemical equation N2(g) + 3 H2(g) 2 NH3(g) there is 1 mol N2, 3 mol H2, and 2 mol NH3. The mole ratios you can use as conversion factors are 1 mol N2/ 3 mol H2 2 mol NH3/ 1 mol N2 3 mol H2/ 2 mol NH3
7 Sample N2(g) + 3 H2(g) 2 NH3(g) mol mol Conversion factors: mol How many mol of NH3 are produced when 0.60 mol nitrogen reacts with hydrogen?
8 Practice 2 4 Al(s) + 3 O2(g) 2 Al2O3(s) 1. a. b. c. d. Write the six mol ratios that can be derived from this equation. How many mol of aluminum are needed to form 3.7 mol Al2O3? How many mol of oxygen are required to react completely with 14.8 mol Al? How many mol of Al2O3 are formed when 0.78 mol O2 reacts with aluminum?
9 Mass to Mass conversions Mass of one substance cannot be directly converted to mass of another substance because different substances have different molar masses and a mole ratio is used to convert between substances in a balanced chemical equation.
10 Sample N2(g) + 3 H2(g) 2 NH3(g) Calculate the number of grams of NH3 produced when 5.40 g of hydrogen reacts with an excess of nitrogen. Mass of hydrogen: Mole ratio: Molar mass of H2: Molar mass of NH3:
11 Practice 3 Acetylene gas (C2H2) is produced by adding water to calcium carbide (CaC2). CaC2(s) + 2 H2O(l) C2H2(g) + Ca(OH)2(aq) a. How many grams of acetylene are produced by adding water to 5.00 g CaC2? b. How many moles of CaC2 are needed to react completely with 49.0 g H2O?
12 Other Stoichiometric Calculations If the quantity given is not in moles, convert to moles! To convert from one substance to another, use the mole ratio. Convert moles of new substance to any other unit as the problem requires.
13 Examples How many molecules of oxygen are produced when 29.2 g of water is decomposed by electrolysis according to this balanced equation? 2H2O(l) 2H2(g) + O2(g) How many liters of nitrogen dioxide are produced when 34 L of oxygen react with an excess of nitrogen monoxide? Assume conditions are at STP. 2NO(g) + O2(g) 2NO2(g)
14
15 Practice Phosphorus and hydrogen can be combined to form phosphine (PH3). P4(s) + 6H2(g) 4PH3(g) How many liters of phosphine are formed when 0.42 L of hydrogen reacts with phosphorus? Ammonia reacts with oxygen to produce nitrogen monoxide and water. NH3(g) + O2(g) NO(g) + H2O(l) How many liters of NO are produced when 1.40 L of oxygen reacts with ammonia?
16 Practice CS2(l) + 3O2(g) CO2(g) + 2SO2(g) Calculate the volume of sulfur dioxide, in milliliters, produced when 27.9 ml O2 reacts with carbon dioxide. How many deciliters of carbon dioxide are produced when 0.38 L of sulfur dioxide is formed?
17 12.3 Limiting Reagent and Percent Yield An insufficient quantity of any of the reactants will limit the amount of product that forms. Limiting reagent: reactant that determines the amount of product that can form Excess reagent: reactant that is not completely used up in a reaction
18 Limiting Reagent: S mores 2Gc + 1 Ma + 3Ch 1 Gc2MaCh3 (S m)
19 Practice 2Cu(s) + S(s) Cu2S(s) What is the limiting reagent when 3 moles of Cu reacts with 2 moles of S? What is the limiting reagent when 90.0 g Cu reacts with 1 mole of S? What is the limiting reagent when 84.5 g of Cu reacts with 84.5 g of S? What is the limiting reagent when 5.00 x 1024 atoms of Cu react with 2.9 x 1023 atoms of S?
20 Percent Yield
21 Reasons for less than 100% Yield Incomplete reactions Impure reactants Competing side-reactions Loss of product during filtration or transferring between containers Imprecise measurement
22 Practice CaCO3(s) Δ CaO(s) + CO2(g) What is the theoretical yield of CaO in grams if 24.8 g of CaCO3 is heated? What is the percent yield if 13.5g CaO are produced? What is the theoretical yield of CO2(g) in liters if 59.1 g of CaCO3 decomposes? What is the percent yield if the actual yield from this reaction is 13.0 L of CO2? If the actual yield is 11.7 L of CO2?
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What does this equation tell you? 1. 1 molecule of nitrogen gas reacts with 3 molecules of hydrogen gas to produce 2 molecules of ammonia gas.
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Exe r c i s es Answers to odd-numbered Exercises are in Appendix I. Key Te rm s Answers to Key Terms are in Appendix H.
284 CHAPTER 10 CHEMICAL EQUATION CALCULATIONS Moles reactant (b) 'llljll!llim'.lllill!w 11r1 nrr1111 Moles product.,.. Concept Map-Summary Stoichiometry We use a strategy map to show the application unit