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UGA CHEM 1211 - Chapter 4

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Slide 1Slide 2Slide 3Slide 4Slide 5Slide 6Slide 7Slide 8Slide 9Slide 10Slide 11Slide 12Slide 13Slide 14Slide 15Slide 16Slide 17Slide 18Slide 19Slide 20Slide 21Slide 22Slide 23Slide 24Slide 25Chemical AnalysisSlide 27Slide 28Slide 29Slide 30Slide 31Slide 32Slide 33Slide 34Slide 35Slide 36Slide 37Slide 38Slide 39Dilution of SolutionsSlide 41Slide 42Slide 43Slide 44Slide 45Titration: A Method of Chemical AnalysisSlide 47Slide 48Slide 49Slide 50Slide 51Slide 52Slide 53Slide 54Slide 55An Absorption SpectrophotometerSlide 57Slide 58Slide 59Ch. 4 Stoichiometry: Quantitative Information about Chemical Reactions4.1 Mass Relationships in Chemical Reactions: StoichiometryA balanced chemical equation shows the quantitative relationship between reactants and products in a chemical reaction.Mass of reactant = mass of products (because of the Law of Conservation of Mass)#of atoms of reactant = #of atoms of products1H2 + O2 → H2O balance22H2 + O2 → 2H2O 2.3 moles of H2, produce how many moles of water (O2 is in excess).I want to produce 5.0 moles of H2O, how many moles of O2 do I have to start with?3Clicker Q: Given this balanced chemical reaction. 3 PbF2 + 2 PCl3 → 2 PF3 + 3 PbCl2 How many moles of PF3 can be made from the reaction of 4.5 moles of PbF2 with excess PCl3? 4grams  moles  moles  grams Using molar massUsing mole ratiosUsing molar mass•In order to solve stoichiometry problems, one must go through moles using molar masses and mole ratios as conversion factors.•One cannot do this without writing a balanced chemical equation first.5Given this balanced chemical reaction. Ca(OH)2 + 2 HCl → CaCl2 + 2 H2O If 37.0 g of Ca(OH)2 (74.0 g/mol) are reacted with excess HCl, how many grams of H2O can be formed? 67What mass of carbon dioxide can be produced by the reaction of 0.540 mole of iron (III) oxide with excess carbon monoxide?Fe O + 3 CO 2 Fe + 3 CO2 3 2 Clicker Q: What is the formula weight for CO2?Clicker Q: Mass of CO2 produced?8What mass of CO is required to react with 146 g of iron (III) oxide (159.7 g/mol)? Fe O + 3 CO 2 Fe + 3 CO2 3 2 9What mass of iron(III) oxide (159.7 g/mol) reacted with excess carbon monoxide if the carbon dioxide produced by the reaction had a mass of 8.65 grams? Fe O + 3 CO 2 Fe + 3 CO2 3 2 4.2 Reactions in Which one Reactant is present in Limited SupplyLimiting reactant: Substance that is used up first is the limiting reactant. It limits the amount of product that can be formed.Suppose a box contains 87 bolts, 110 washers, and 99 nuts. How many sets, each consisting of one bolt, two washers, and one nut, can you construct from the contents of one box?10Kokosberger4 eggs240 g of sugar320 g of coconut flakesMakes 48 “cookies”What if I had 6 eggs, 120 g of sugar, and 350 g of coconut flakes, how many cookies would I make?Clicker Q: What if I had 4 eggs, 250 g of sugar, and 340 g of coconut flakes, how many cookies would I make?11A Stoichiometry Calculation with a Limiting ReactantAt high temperatures, ammonia can react with oxygen according to the following unbalanced reaction: NH3 + O2 ---> NO + H2O If 6.55 moles of NH3 react with 15.4 moles of oxygen, how many moles of water can theoretically be produced? 12Clicker Q: How many moles of HCl can be produced by reacting 4.0 mol of H2 and 3.5 mol of Cl2? Which cpd is the limiting reactant? Enter moles of product produced.13How many g of silver bromide (187.8 g/mol) can be formed when solutions containing 50.0 g of magnesium bromide (184.1 g/mol) and 100.0 g of silver nitrate (169.9 g/mol) are mixed together (magnesium nitrate is also produced)? How many g of the excess reactant remain unreacted?1415Clicker Q: What is the maximum mass of sulfur dioxide (64.1 g/mol) that can be produced by the reaction of 95.6 g of carbon disulfide (76.12 g/mol) with 110. g of oxygen? Carbon disulfide reacts with oxygen to form carbon dioxide and sulfur dioxide.Which is the limiting reactant if we start with 50.0 g Al and 50.0 g O2? How much product can you make? How much (in moles) of the excess reagent remains?16174.3 Percent YieldThe theoretical yield is the maximum product yield that can be expected based on the masses of the reactants and the reaction stoichiometry.The actual yield is the experimentally measured amount of products that results upon completion of the reaction.The percent yield is a measure of the extent of the reaction in terms of the actual vs. the theoretical yield.=% Yield Actual Yield (in grams or moles)Theoretical Yield (in grams or moles)�100 18Fig. 4-3, p. 16619Clicker Q: If a chemical reaction has a % yield of 56.3% and the theoretical yield is 80.0 g, what is the actual yield in g? 2021A 10.0 g sample of ethanol, C2H5OH (46 g/mol), was boiled with excess acetic acid, CH3COOH, to produce 14.8 g of ethyl acetate, CH3COOC2H5 (88 g/mol). What is the percent yield?3 2 5 3 2 5 2CH COOH + C H OH CH COOC H H O� +Clicker Q: What is theoretical yield in g?Given this balanced chemical reaction: BaCl2(s) + H2SO4(aq) → BaSO 4(s) + 2 HCl(aq) If 97.2 g of BaCl2 (208.2 g/mol) are reacted with 11.4 g of H2SO4 (98.0 g/mol) and 21.9 g of BaSO4 (233.4 g/mol) are made, what is the percent yield for this reaction? Clicker Q: What is the theoretical yield (in g)?22How many grams of commercial acetic acid (97.0% C2H4O2 by mass) must be allowed to react with an excess of PCl3 to produce 77.7 g of C2H3OCl, if the reaction has a 67.8% yield? Balanced reaction: 3 C2H4O2 + PCl3 → 3C2H3OCl + H3PO423Hydrogen peroxide decomposes into H2O and oxygen gas. In a certain experiment, 71.13 g of hydrogen peroxide decomposed to yield 15.33 g of oxygen gas. Calculate the theoretical and percent yields for this experiment. Clicker Q: What is the % yield?244.4 Chemical Equations and Chemical AnalysisQuantitative Analysis of a MixtureDepends on 2 basic ideas:1. A substance, present in unknown amount, reacts with a known amount of another substance. Stoichiometric ratio known for their reaction then unknown amount can be calculated (like a titration)2. Material of unknown composition can be converted to one or more substances of known composition25•A 0.123 g sample of the mineral thenardite contains sodium sulfate along with several inert compounds.•The sodium sulfate in the sample is converted to insoluble barium sulfate by adding aqueous barium chloride in excess to the


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UGA CHEM 1211 - Chapter 4

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