Slide 1Slide 2Slide 3Limiting Reactant ConceptSlide 5Slide 6Slide 7Slide 8Slide 9Percent Yields from ReactionsSlide 11Slide 12Slide 13Slide 14Concentration of SolutionsSlide 16Slide 17Slide 18Slide 19Slide 201What mass of CO is required to react with 146 g of iron (III) oxide?146 g Fe2O3 / 159.69 g/mol = 0.914 moles Fe2O30.914 moles Fe2O3 (3 moles of CO / 1 mole of Fe2O3)= 2.74 moles CO2.74 moles CO x 28.0 g/mol = 76.7 g CO146 g Fe2O3 (1 mole Fe2O3/159.69 g Fe2O3)(3 moles CO/1 mole Fe2O3)(28.0 g CO/1 mole CO) = 76.7 g COFe O + 3 CO 2 Fe + 3 CO2 3 2 2Clicker question:What mass of iron (III) oxide reacted with excess carbon monoxide if the carbon dioxide produced by the reaction had a mass of 8.65 grams? 8.65 g CO2 / 44.0 g/mol = 0.1965 moles CO2 (1 Fe2O3/3CO2) = .0655 moles Fe2O3 x 159.69 g/mol = 10.46 = 10.5 g Fe2O3Fe2O3 + 3 COD¾ ®¾ 2 Fe + 3 CO2The limiting reactant (reagent) conceptSubstance that is used up first is the limiting reactant. It limits the amount of product that can be formed.4Limiting Reactant ConceptSuppose 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?110 / 55 = 2 washers, washers = limiting reactant!How many moles of HCl can be produced by reacting 4.0 mol of H2 and 3.5 mol of Cl2? Which compoundd is the limiting reactant?1. Write formula: H2 + Cl2 = 2HCl2. 4.0 moles of H2 (2 HCl / 1 H2) = 8.0 moles HCl3. 3.5 moles of Cl2 (2 HCl / 1 Cl2) = 7.0 moles HCl4. Chlorine (Cl2) is limiting reactant because it only make 7.0 moles of HCl5. 4 moles of H2 (1 Cl2 / 1 H2) = 4.0 mole Cl21. 3.5 moles of Cl2 (1 mole H2 / 1 mole Cl2) = 3.o mole H21. Cl2 = limiting reactant6What is the maximum mass of sulfur dioxide that can be produced by the reaction of 95.6 g of carbon disulfide with 110. g of oxygen? Carbon disulfide reacts with oxygen to form carbon dioxide and sulfur dioxide.CS2 + 3O2 = CO2 + 2SO2How many g of silver bromide can be formed when solutions containing 50.0 g of magnesium bromide and 100.0 g of silver nitrate are mixed together (magnesium nitrate is also produced)? How many g of the excess reactant remain unreacted?10Percent Yields from Reactions•Theoretical yield is calculated by assuming that the reaction goes to completion.–Determined from the limiting reactant calc.•Actual yield is the amount of a specified pure product made in a given reaction.–In the laboratory, this is the amount of product that is formed in your beaker, after it is purified and dried.•Percent yield indicates how much of the product is obtained from a reaction.% yield = actual yieldtheoretical yield100%11A 10.0 g sample of ethanol, C2H5OH, was boiled with excess acetic acid, CH3COOH, to produce 14.8 g of ethyl acetate, CH3COOC2H5. What is the percent yield?3 2 5 3 2 5 2CH COOH + C H OH CH COOC H H O� +Sequential ReactionsMore than one reaction is required to convert starting materials into the desired products. The amount of desired product from each reaction is taken as the starting material for the next reaction.13Starting with 10.0 g of benzene (C6H6), calculate the theoretical yield of nitrobenzene (C6H5NO2) and of aniline (C6H5NH2).Clicker questionIf 6.7 g of aniline is prepared from 10.0 g of benzene, what is the percentage yield?15Concentration of Solutions•Solution is a mixture of two or more substances dissolved in another.–Solute is the substance present in the smaller amount.–Solvent is the substance present in the larger amount.–In aqueous solutions, the solvent is water.•The concentration of a solution defines the amount of solute dissolved in the solvent.–The amount of sugar in sweet tea can be defined by its concentration.16One common unit of concentration is:% by mass of solute has the symbol %w/wmass of solute% by mass of solute = 100%mass of solutionmass of solution = mass of solute + mass of solvent�17What mass of NaOH is required to prepare 250.0 g of solution that is 8.00% w/w NaOH?18Calculate the mass of 8.00% w/w NaOH solution that contains 32.0 g of NaOH.19Calculate the mass of NaOH in 300.0 mL of an 8.00% w/w NaOH solution. Density is 1.09 g/mL.20What volume of 12.0% w/w KOH contains 40.0 g of KOH? The density of the solution is 1.11