35 Example 2What mass of carbon dioxide was used to form 5.0 moles of water?
36 Example 2 220 g CO2 C6H12O6 +6O2 --> 6CO2 + 6H2O 6 moles CO2 5.0 moles H2OX44g CO2=X1 mole CO26 moles H2O220 g CO2
37 Try it Out! N2O5 + H2O --> 2HNO3 What mass of water was used to form 2.5 moles of HNO3? (23 g H2O)What mass of HNO3 will form from moles of N2O5? (1512 g HNO3)
38 Answer to #1 23 g. H2O 18g. H2O 1 mole H2O 2.5 moles HNO3 X X =
39 Answer to #2 = 1512 g. HNO3 2 moles HNO3 63g. HNO3 12.00 moles N2O5 X 1 mole N2O51 mole HNO3=1512 g. HNO3
40 Mass-->Mole Conversions Given mass of one substance and asked to find moles of another substance.
41 To Solve molar molar mass ratio PT Moles Mass equation Moles Given Unknown
42 How many moles of NO were used to form 824g. NH3? Example2NO + 3H2 --> 2NH3 + O2How many moles of NO were used to form 824g. NH3?
43 Example = 48.5 moles NO 1 mole NH3 2 moles NO 824g. NH3 X X 17g. NH3 2NO + 3H2 --> 2NH3 + O21 mole NH32 moles NO824g. NH3XX17g. NH32 moles NH3=48.5 moles NO
44 How many moles of H2 were used to form 312 g of O2? Example2NO + 3H2 --> 2NH3 + O2How many moles of H2 were used to form 312 g of O2?1 mole O23 moles H2312g. O2XX32g. O21 mole O2=29.3 moles H2
45 Isosceles $300 $200 Right Scalene $250 Acute $50 $100 Equilateral $150 $100,000 PyramidIsosceles$300Pencil$200RightCougarsChemistryScalene$250Have the pairs hold up their hand when they finish.PurpleAcute$50$100Safety ShowerEquilateral$150MoleObtuse
46 Isosceles $300 $200 Right Scalene $250 Acute $50 $100 Equilateral $150 $100,000 PyramidIsosceles$300Stoichiometry$200RightCoefficientMolar MassScalene$250Have the pairs hold up their hand when they finish.Periodic TableAcute$50$100BalanceEquilateral$150RatioObtuse
47 Today… Turn in: Worksheet #1 & Worksheet #2 Our Plan: Conversions Table ReviewNotes – Mass to Mass ConversionsWorksheet #3Homework (Write in Planner):Worksheet #3 due next class
48 The Stoichiometry Map Mass Moles Given Volume Moles Unknown Molecules Molar RatioEquation6.022 x 1023Molar MassPT22.4 L/mole
49 Team Conversion review As a group of 3 or 4, complete the problems on the team conversion review. Each student should have a different colored writing utensil and you should take turns doing the work.
50 The Stoichiometry Map Mass Moles Given Volume Moles Unknown Molecules Molar RatioEquation6.022 x 1023Molar MassPT22.4 L/mole
51 Mass-->Mass Conversions Given the mass of one substance and asked to determine the mass of another substance.
52 To Solve: molar molar molar mass ratio mass Mass PT Moles Moles Mass equationmolarmassPTMassGivenMolesGivenMolesUnknownMassUnkn
53 Example Find the mass of table salt produced from 18.6g Na. 2Na + Cl2 -->2NaClFind the mass of table salt produced from 18.6g Na.
54 Example = 47.3g NaCl 2Na + Cl2 --> 2NaCl 1 mole Na 2 moles NaCl 1 mole NaCl=47.3g NaCl
55 Example2Al + Fe2O3 --> Al2O3 + 2FeFind the mass of aluminum oxide produced from 2.3g of aluminum.
56 Example = 4.3 g Al2O3 2Al + Fe2O3 --> Al2O3 + 2Fe 1 mole Al 1 mole Al2O3102g Al2O3X2.3g. AlXX27g. Al2 mole Al1 mole Al2O3=4.3 g Al2O32Al + Fe2O3 --> Al2O3 + 2Fe
57 Try it Out!Methane burns in air by the following reaction: CH4 + 2O2 --> CO2 + 2H2OWhat mass of water is produced by burning g of methane?
58 Example = 1,130 g H2O 1 mole CH4 2 mole H2O 18g H2O X 500.g CH4 X X
64 Today… Turn in: Any Missing Worksheets Our Plan: Lab Day 3 Turn in Lab TodayHomework (Write in Planner):Lab, if not done
65 Lab Helpful Hints #1 – 1000 mg = 1 g, 1000 mL = 1 L #3 – Convert both the 1g AgNO3 and your g of Cu to g of Ag. The limiting reactant is the reactant that produces the least product. You will do 2 three step conversions to find the answer.# 5 & #6 – Percent yield = (actual/theoretical) x 100WASH ALL SUPPLIES, RETURN TO SIDE TABLE, WIPE DOWN COUNTER, WASH HANDS!
67 Today… Our Plan: Turn in: Metal in Water Lab Relay Race Review Daily ChallengeNotes – Stoichiometry of Gases and MoleculesWorksheet #4Homework (Write in Planner):WS#4 due next class
68 Daily Challenge How many liters are in 1 mole of a gas? How many molecules are in 1 mole of any compound?For the reaction below, what mass of water can be produced from 1.5 moles of hydrogen? (27g)2H2 + O2 --> 2H2O
69 The Stoichiometry Map Mass Moles Given Volume Moles Unknown Molecules Molar RatioEquation6.022 x 1023Molar MassPT22.4 L/mole
70 Volume --> Volume Conversions Given the volume of one substance and asked to determine the volume of another substance.
71 To Solve: molar 22.4 L ratio Vol Vol Moles Moles equation 22.4 L Given UnknownVolUnkn22.4 L
73 STP is 0 degrees Celsius and 1 atm Molar VolumeYou can only use the conversion factor 22.4 under very specific conditions.It must be a gas and it must be at STP (Standard Temperature and Pressure)STP is 0 degrees Celsius and 1 atm
74 How many moles of Helium are in a 3.7 L balloon at STP? Sample ProblemHow many moles of Helium are in a 3.7 L balloon at STP?
76 Practice Problem 2 CO + O2 --> 2 CO2 What volume of carbon dioxide will be produced from 2.6 L of oxygen at STP?
77 The Stoichiometry Map Mass Moles Given Volume Moles Unknown Molecules Molar RatioEquation6.022 x 1023Molar MassPT22.4 L/mole
78 Practice Problem 5.2 L CO2 2 CO + O2 --> 2 CO2 2.6 L O2 X 1 mole O2 X22.4 L O22 mole CO2 X1 mole O222.4 L CO2 =1 mole CO25.2 L CO2
79 Practice ProblemUsing the same equation, what volume of carbon dioxide will be produced at STP from grams of carbon monoxide?
80 The Stoichiometry Map Mass Moles Given Volume Moles Unknown Molecules Molar RatioEquation6.022 x 1023Molar MassPT22.4 L/mole
81 Practice Problem 36.2 L CO2 2 CO + O2 --> 2 CO2 45.3 g CO X 1 mole CO X28 g CO2 mole CO2 X2 mole CO22.4 L CO2 =1 mole CO236.2 L CO2
82 Try It Out!Using the same equation, what volume of oxygen is used to produce 19.3 grams of carbon dioxide at STP? (4.91 L)
83 Try it Out! 4.91 L O2 2 CO + O2 --> 2 CO2 19.3 g CO2 X 1 mole CO2 X 1 mole O2 X2 mole CO222.4 L O2 =1 mole O24.91 L O2
84 Molecule Stoichiometry Problems You can do the same type of problems using molecules. Just use Avogadro’s Number!
85 ExampleIn the reaction: H2 + O2 --> 2H2O if you have grams of hydrogen, how many molecules of water will form?
86 The Stoichiometry Map Mass Moles Given Volume Moles Unknown Molecules Molar RatioEquation6.022 x 1023Molar MassPT22.4 L/mole
87 Example = 1.5 x 1023 molecules H2O 2H2 + O2 --> 2H2O 1 mole H22 mole H2OX0.50 g H2XX2 mole H22 g H21 mole H2O=1.5 x 1023 molecules H2O2H2 + O2 --> 2H2O
88 Real Life Applications CookingPlanning outcomes of reactionsRace cars/ mechanics
89 Real Life Applications Treating an upset stomachAirbagsArtists
90 Real Life Applications Launching space shuttleBaking breadEngineering
91 STOP!Complete Worksheet #4 by next class period!
92 Today… Turn in: Get Worksheet #4 Out to Check Our Plan: Balloon Races Limiting Reactant NotesFinish Balloon Races HandoutWorksheet #5Chemistry CartoonHomework (Write in Planner):Worksheet 5 & Cartoon Due Next Class
93 HC2H3O2 + NaHCO3 --> NaC2H3O2 + CO2 + H2O. MoleculesMassVolumeMoles GivenMoles UnknownMolar RatioEquation6.022 x 1023Molar MassPT22.4 L/molePre Lab Review – The balanced equation for the reaction of baking soda and vinegar is:HC2H3O2 + NaHCO3 --> NaC2H3O2 + CO2 + H2O.How many liters of carbon dioxide can form from 3.00 g of baking soda (NaHCO3)? Show your work at the top of your lab.
116 Today… Turn in: Get Worksheet #5 Out to Check Turn in Chemistry Cartoon - BasketOur Plan:L.R. Review ProblemPercent Yield NotesWorksheet #6Homework (Write in Planner):Worksheet #6 Due Tuesday/Wednesday
117 WS 6 #4Acrylonitrile, C3H3N, is an important ingredient in the production of various fibers and plastics. Acrylonitrile is produced from the following reaction:C3H6 + NH3 + O2 --> C3H3N + H2OIf 850 g of C3H6 is mixed with 300. g of NH3 and unlimited O2, to produce 850. g of acrylonitrile, what is the percent yield? You must first balance the equation. 91 %
118 Baseball’s Best!Babe Ruth played in baseball games in his career. He had hits in 8399 at bats what was his batting average?
119 Baseball’s Best!Hank Aaron played in baseball games in his career. He had hits in 12,364 at bats. What was his batting average?
120 Theoretical Yield is based on calculations Percent YieldTheoretical Yield is based on calculations
121 Actual Yield is based on the actual chemical reaction (the lab) Percent YieldActual Yield is based on the actual chemical reaction (the lab)
122 The Formula% yield = Actual yield X 100Theoretical yield
123 To Calculate Write equation Calculate the mass of the product that should have been formed. (theoretical yield)
124 Plug numbers into the equation To CalculatePlug numbers into the equation
125 ExampleDetermine the % yield for the reaction between 2.80 g Al(NO3)3 & excess NaOH if 0.966g Al(OH)3 is recovered.
126 ExampleWrite the equation:Al(NO3)3 + 3NaOH --> Al(OH)3 + 3NaNO3
133 Today… Turn in: Worksheet #6 Our Plan: Stoichiometry Lab Test Test ReviewHomework (Write in Planner):Test Review due next classUNIT 8 TEST NEXT CLASS!
134 Today… Turn in: Get out Test Review Our Plan: Questions on Test Review?TestLarry the Lawnchair Guy ReadingHomework (Write in Planner):Larry Reading due next class
135 Some sample problems… Given the following reaction: C3H8 + 5O2 > 3CO2 + 4H2OIf you start with 14.8 g of C3H8 and 3.44 g of O2, determine the limiting reagentGiven the following equation:H3PO4 + 3 KOH > K3PO4 + 3 H2OIf 49.0 g of H3PO4 is reacted with excess KOH, determine the percent yield of K3PO4 if you isolate 49.0 g of K3PO4.
136 Another Percent Yield Example Given the following equation:Al(OH)3 +3 HCl --> AlCl3 + 3 H2OIf you start with 50.3 g of Al(OH)3 and you isolate 39.5 g of AlCl3, what is the percent yield?H2SO4 + Ba(OH)2 ----> BaSO4 + H2OIf 98.0 g of H2SO4 is reacted with excess Ba(OH)2, determine the percent yield of if g of BaSO4 is formed.