Modern Chemistry Chapter 9 Stoichiometry Sections 1-3 Introduction to Stoichiometry Ideal Stoichiometric Calculations Limiting Reactant and Percent Yield

Chapter 9 Vocabulary Composition Stoichiometry Reaction Stoichiometry Mole Ratio Limiting Reactant Excess Reactant Actual Yield Theoretical Yield Percent Yield

Chapter 9 Section 1 Introduction to Stoichiometry Chapter 9 Section 1 Intro. Stoichiometry pages 299-303

Chapter 9 Section 1 Intro. Stoichiometry pages 299-303 Definitions Composition stoichiometry deals with the mass relationships of elements in compounds. Reaction stoichiometry involves the mass relationships between reactants and products in a chemical reaction. Chapter 9 Section 1 Intro. Stoichiometry pages 299-303

Stoichiometry Animation Chapter 9 Section 1 Intro. Stoichiometry pages 299-303 p. xx

Chapter 9 Section 1 Intro. Stoichiometry pages 299-303 Definitions A mole ratio is a conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction Example: 2Al2O3(l)  4Al(s) + 3O2(g) Mole Ratios: 2 mol Al2O3 2 mol Al2O3 4 mol Al 4 mol Al 3 mol O2 3 mol O2 Chapter 9 Section 1 Intro. Stoichiometry pages 299-303

Chapter 9 Section 1 Intro. Stoichiometry pages 299-303 Using the Mole Ratio Chapter 9 Section 1 Intro. Stoichiometry pages 299-303 p. xx

Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g) Mole – Mole Examples Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g) If 2 mol of HCl react, how many moles of H2 are obtained? How many moles of Mg will react with 2 mol of HCl? If 4 mol of HCl react, how many mol of each product are produced? How would you convert from moles of substances to masses? Chapter 9 Section 1 Intro. Stoichiometry pages 299-303

Chapter 9 Section 1 Intro. Stoichiometry pages 299-303 Converting from gmol Chapter 9 Section 1 Intro. Stoichiometry pages 299-303 p. xx

Chapter 9 Section 1 Intro. Stoichiometry pages 299-303 Section 1 Homework Page 301 #1-4 Chapter 9 Section 1 Intro. Stoichiometry pages 299-303

Chapter 9 Section 2 Ideal Stoichiometric Calculations Chapter 9 Section 2 Ideal Stoichiometry pages 304-311

Reactants  Products MASS OF SUBSTANCE GIVEN MASS OF SUBSTANCE WANTED MOLAR MASS MOLAR MASS MOLES OF SUBSTANCE GIVEN MOLES OF SUBSTANCE WANTED MOLE RATIO Chapter 9 Section 2 Ideal Stoichiometry pages 304-311

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Tool Box GRAMSmL DENSITY GRAMSMOLES MOLAR MASS MOLES MOLES MOLE RATIO MOLES PARTICLES 6.02x1023 1000 g = 1kg 1000 mL = 1L 1000 mg = 1g Chapter 9 Section 2 Ideal Stoichiometry pages 304-311

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Kg L mg mL g MOLES MOLES g mg mL L Kg Chapter 9 Section 2 Ideal Stoichiometry pages 304-311

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Sample Problem How many kilograms of ethane are required to react with excess oxygen to produce 8.70 L of carbon dioxide? The density of carbon dioxide gas at standard temperature is 1.799 g/L. 0.00535 kg Chapter 9 Section 2 Ideal Stoichiometry pages 304-311

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Kg L mg mL g MOLES MOLES g mg mL L Kg Chapter 9 Section 2 Ideal Stoichiometry pages 304-311

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 L CO2 g CO2 mol CO2 mol C2H6 g C2H6 kg C2H6 x x x x x L CO2 g CO2 mol CO2 mol C2H6 g C2H6 Kg g MOLES MOLES g L Chapter 9 Section 2 Ideal Stoichiometry pages 304-311

C2H6 (g) + O2 (g)  CO2 (g) + H2O (g) + E 8.70L ? Kg g g MOLES MOLES L CO2 g CO2 mol CO2 mol C2H6 g C2H6 kg C2H6 x x x x x L CO2 g CO2 mol CO2 mol C2H6 g C2H6 Chapter 9 Section 2 Ideal Stoichiometry pages 304-311

C2H6 (g) + O2 (g)  CO2 (g) + H2O (g) + E 8.70L ? Kg g g 1000g=1Kg MOLAR MASS MOLAR MASS MOLAR RATIO MOLES MOLES DENSITY L CO2 g CO2 mol CO2 mol C2H6 g C2H6 kg C2H6 x x x x x L CO2 g CO2 mol CO2 mol C2H6 g C2H6 Chapter 9 Section 2 Ideal Stoichiometry pages 304-311

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Sample Problem p. 306 In photosynthesis, plants use energy from the sun to produce glucose, C6H12O6, and oxygen from the reaction of carbon dioxide and water. What mass, in grams, of glucose is produced when 3.00 mol of water react with carbon dioxide? 90.1 g C6H12O6 Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 mol-mass

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Sample Problem p. 310 Tin (II) fluoride, SnF2, is used in some toothpastes. It is made by the reaction of tin with hydrogen fluoride according to the following equation. Sn(s) + 2HF(g)  SnF2(s) + H2(g) How many grams of SnF2 are produced from the reaction of 30.00 g HF with Sn? 117.5 g SnF2 Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 mass-mass.

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Sample Problem p. 305 In a spacecraft, the carbon dioxide exhaled by astronauts can be removed by its reaction with lithium hydroxide, LiOH, according to the following chemical equation. CO2(g) + 2LiOH(s)  Li2CO3(s) + H2O(l) How many moles of lithium hydroxide are required to react with 20 mol CO2, the average amount exhaled by a person each day? 40 mol LiOH Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 mol-mol

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Sample Problem p. 309 The first step in the industrial manufacture of nitric acid is the catalytic oxidation of ammonia. NH3(g) + O2(g)  NO(g) + H2O(g) (unbalanced) The reaction is run using 824 g NH3 and excess oxygen. a. How many moles of NO are formed? b. How many moles of H2O are formed? 48.4mol NO; 72.5 mol H2O Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 mass-mol

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Problem Magnesium burns in oxygen to produce magnesium oxide. How many grams magnesium will burn in the presence of 189 mL of oxygen? The density of oxygen is 1.429g/L. 0.410 g Mg Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 mL-g

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Problem Limestone, CaCO3, can be decomposed with heat to form lime, CaO, and carbon dioxide. How many moles of lime would be formed from the decomposition of 20.1 kilograms of limestone? 201 moles CaO Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Kg-mol.

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Section 2 Homework Page 311 #1-5 Chapter 9 Section 2 Ideal Stoichiometry pages 304-311

Section 2 Homework Problem Bank Page 890-892 #176, 177, 179, 180, 184, 187, 190, 191, 192, 194, 196 Chapter 9 Section 2 Ideal Stoichiometry pages 304-311

Chapter 9 Section 3 Limiting Reactant and Percent Yield Chapter 9 Section 3 Limiting Reactant pages 312-318

Chapter 9 Section 3 Limiting Reactant pages 312-318 Definitions The limiting reactant is the reactant that limits the amount of the other reactant that can combine and the amount of product that can form in a chemical reaction. The excess reactant is the substance that is not used up completely in a reaction. Chapter 9 Section 3 Limiting Reactant pages 312-318

Chapter 9 Section 3 Limiting Reactant pages 312-318 S’mores Given the bag o’ reactants find the number of s’mores you could produce if the balanced equation is 2 Tg + 1 Mm  1 Sm Tg = Teddy Graham Mm = Minimarshmallow Sm = S’more Chapter 9 Section 3 Limiting Reactant pages 312-318

Chapter 9 Section 3 Limiting Reactant pages 312-318 S’mores What is the limiting reactant? What is the reactant in excess? What is the amount in excess ? What is the theoretical yield? What is the actual yield? What is the percent yield? Chapter 9 Section 3 Limiting Reactant pages 312-318

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Sample Problem p. 313 Silicon dioxide (quartz) is usually quite unreactive but reacts readily with hydrogen fluoride according to the following equation. SiO2(s) + 4HF(g)  SiF4(g) + 2H2O(l) If 6.0 mol HF is added to 4.5 mol SiO2, which is the limiting reactant? HF Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 mol & mol limiting

Chapter 9 Section 3 Limiting Reactant pages 312-318 Problem I need a problem that requires them to answer these questions a. Which compound is the limiting reactant? b. What is the theoretical yield of product? c. What is the reactant in excess, and how much remains after the reaction is completed? 8.940 x 1023 molecules Chapter 9 Section 3 Limiting Reactant pages 312-318 mass & mass, limiting, actual

Chapter 9 Section 3 Limiting Reactant pages 312-318 Problem I need another problem that requires them to answer these questions a. Which compound is the limiting reactant? b. What is the theoretical yield of product? c. What is the reactant in excess, and how much remains after the reaction is completed? 8.940 x 1023 molecules Chapter 9 Section 3 Limiting Reactant pages 312-318 mass & mass, limiting, actual

Chapter 9 Section 3 Limiting Reactant pages 312-318 p. xx

Chapter 9 Section 3 Limiting Reactant pages 312-318 Section 3 Homework Page 318 #1 & 2 Chapter 9 Section 3 Limiting Reactant pages 312-318

Chapter 9 Section 3 Limiting Reactant pages 312-318 Definitions The theoretical yield is the maximum amount of product that can be produced from a give amount of reactant. The actual yield is the measured amount of product obtained from a reaction. The percentage yield is the ratio of the actual yield to the theoretical yield, multiplied by 100. Chapter 9 Section 3 Limiting Reactant pages 312-318

Chapter 9 Section 3 Limiting Reactant pages 312-318 Percent Yield Chapter 9 Section 3 Limiting Reactant pages 312-318 p. xx

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Sample Problem p. 317 Chlorobenzene, C6H5Cl, is used in the production of many important chemicals, such as aspirin, dyes, and disinfectants. One industrial method of preparing chlorobenzene is to react benzene, C6H6, with chlorine, as represented by the following equation. C6H6 (l) + Cl2 (g)  C6H5Cl (l) + HCl (g) When 36.8 g C6H6 react with an excess of Cl2, the actual yield of C6H5Cl is 38.8 g. What is the percentage yield of C6H5Cl? 73.2% Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 mass-mass percent

Chapter 9 Section 3 Limiting Reactant pages 312-318 Problem Hydrogen sulfide gas can be formed by the action of HCl and FeS, forming FeCl2 as product. What is the theoretical yield in molecules of hydrogen sulfide if 130.5 g of FeS are mixed with 150.0 g of HCl? If the percent yield in the lab is 93.6% what is the actual yield? 8.940 x 1023 molecules Chapter 9 Section 3 Limiting Reactant pages 312-318 mass & mass, limiting, actual

Chapter 9 Section 2 Ideal Stoichiometry pages 304-311 Problem Benzene, C6H6, is reacted with bromine, Br2, to produce bromobenzene, C6H5Br, and hydrogen bromide, HBr, as shown below. When 40.0 g of benzene are reacted with 95.0 g of bromine, 65.0 g of bromobenzene is produced. C6H6 + Br2  C6H5Br + HBr a. Which compound is the limiting reactant? b. What is the theoretical yield of bromobenzene? c. What is the reactant in excess, and how much remains after the reaction is completed? d. What is the percentage yield? Benzene, 80.4g, Br2 13.2g, 80.8% Chapter 9 Section 2 Ideal Stoichiometry pages 304-311

Chapter 9 Section 3 Limiting Reactant pages 312-318 Molarity Molarity measures the concentration of solutions. (aq) Molarity = moles / liter 3 mol 3M = 1 L Chapter 9 Section 3 Limiting Reactant pages 312-318

Chapter 9 Section 3 Limiting Reactant pages 312-318 Problem When 20.0 mL of 0.90M solution of lithium nitrate and 15.0 mL of 0.40M solution of calcium phosphate react, a precipitate is formed. The mass of the precipitate produced in the lab is 0.66 grams. What is the reactant in excess, the limiting reactant, the amount in excess, the theoretical yield and the percent yield. 0.69 grams theo. Chapter 9 Section 3 Limiting Reactant pages 312-318

Section 3 Homework Problem Bank Page 892-894 #201, 208, 214, 217, 219, 223, 226, 229, 232 Chapter 9 Section 3 Limiting Reactant pages 312-318