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Stoichiometry Chapter 12 Turn in: Forensic Farming Reading Fill Out Goal Sheet Our Plan: Begin Lab Daily Challenge – Smore’s Stoichiometry Notes – Stoichiometry Conversions Worksheet #1 & Worksheet #2 Wrap Up - Pyramid Homework (Write in Planner): WS#1 & WS#2 Due Monday www.doh.state.fl.us Follow the procedure for Day 1 and begin recording observations Use the internet to answer the Pre-Lab Questions Stoy-key-ahm-a-tree Comes from the combination of the Greek words stoikheioin, meaning “element”, and metron, meaning “to measure” The study of the quantitative, or measurable, relationships in a chemical reaction. Using stoichiometry, you can determine the quantities of reactants & products in a reaction from the BALANCED equation. Like the Recipe! Do show the number of moles of each substance involved in the rxn. Do Not indicate the actual number of grams of the substance. N2 + 3H2 --> 2NH3 2 Atoms N 6 Atoms H On both the reactant and product side! N2 + 3H2 --> 2NH3 1 Molecule N2 3 Molecules H2 2 Molecules NH 3 N2 + 3H2 --> 2NH3 1 Mole N2 3 Moles H2 2 Moles NH 3 N2 + 3H2 --> 2NH3 28 Grams N2 6 Grams H2 34 Grams NH 3 Which were conserved? Atoms and Mass, but NOT Moles and Molecules! A conversion factor that relates the amounts in moles of any 2 substances involved in a chemical reaction. N2 + 3H2 --> 2NH3 1 mole N2 3 moles H2 3 moles H2 2 moles NH3 1 mole N2 2 moles NH3 Molecules Molecules 6.022 x 1023 Mass Volume Molar Mass PT 22.4 L/mole 6.022 x 1023 Moles Given Molar Ratio Equation Moles Unknown Molar Mass PT Mass 22.4 L/mole Volume The conversion of moles of one type of substance to moles of another type of substance. Moles Given Molar Ratio Equation Moles Unknown H2 + I2 --> 2HI If 4 moles of H2 react, how many moles of HI will form? H2 + I2 --> 2HI 2 moles HI 4 moles H2 X 1 mole H2 = 8 moles HI If 0.8 moles of HI form, how many moles of I2 were used in the rxn? H2 + I2 --> 2HI 0.8 moles HI X 1 mole I2 2 moles HI =0.4 moles I2 2H2 + O2 --> 2H2O 1.If 1.3 moles of H2O form, how many moles of O2 were used in the rxn? (0.65 moles) 2.If 0.21 moles of H2 react, how many moles of H2O will form? (0.21 moles) Given the moles of one substance & asked to determine the mass of another substance. molar Moles Given ratio molar mass Moles equation Unknown PT Mass Unknown C6H12O6 +6O2 --> 6CO2 + 6H2O What mass of sucrose was used if 3 moles of water formed? C6H12O6 +6O2 --> 6CO2 + 6H2O 3 moles H2O X 1 mole C6H12O6 X 6 moles H2O 90g C6H12O6 180g C6H12O6 1 mole C6H12O6 = What mass of carbon dioxide was used to form 5.0 moles of water? C6H12O6 +6O2 --> 6CO2 + 6H2O 5.0 moles H2O X 6 moles CO2 X 6 moles H2O 44g CO2 1 mole CO2 220 g CO2 = N2O5 + H2O --> 2HNO3 1.What mass of water was used to form 2.5 moles of HNO3? (23 g H2O) 2.What mass of HNO3 will form from 12.00 moles of N2O5? (1512 g HNO3) 63g. HNO3 12.00 moles N2O5 X 2 moles HNO3 X 1 mole N2O5 1 mole HNO3 = 1512 g. HNO3 Given mass of one substance and asked to find moles of another substance. molar Mass Given mass PT molar Moles Given ratio equation Moles Unknown 2NO + 3H2 --> 2NH3 + O2 How many moles of NO were used to form 824g. NH3? 2NO + 3H2 --> 2NH3 + O2 824g. NH3 X 1 mole NH3 17g. NH3 2 moles NO X 2 moles NH3 = 48.5 moles NO 2NO + 3H2 --> 2NH3 + O2 1 mole O2 3 moles H2 312g. O2 X X 32g. O2 1 mole O2 = 29.3 moles H2 $100,000 Pyramid Pencil Cougars Purple Chemistry Safety Shower Mole $100,000 Pyramid Stoichiometry Coefficient Periodic Table Molar Mass Balance Ratio Turn in: Worksheet #1 & Worksheet #2 Our Plan: Conversions Table Review Notes – Mass to Mass Conversions Worksheet #3 Homework (Write in Planner): Worksheet #3 due next class Molecules Molecules 6.022 x 1023 Mass Volume Molar Mass PT 22.4 L/mole 6.022 x 1023 Moles Given Molar Ratio Equation Moles Unknown Molar Mass PT Mass 22.4 L/mole Volume 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. Molecules Molecules 6.022 x 1023 Mass Volume Molar Mass PT 22.4 L/mole 6.022 x 1023 Moles Given Molar Ratio Equation Moles Unknown Molar Mass PT Mass 22.4 L/mole Volume Given the mass of one substance and asked to determine the mass of another substance. molar Mass mass Given PT molar molar Moles mass Moles ratio Given equation Unknown PT Mass Unkn 2Na + Cl2 -->2NaCl Find the mass of table salt produced from 18.6g Na. 2Na + Cl2 --> 2NaCl 18.6g. Na X 1 mole Na X 2 moles NaCl X 58.5g NaCl 23g. Na 2 mole Na 1 mole NaCl =47.3g NaCl 2Al + Fe2O3 --> Al2O3 + 2Fe Find the mass of aluminum oxide produced from 2.3g of aluminum. 2.3g. Al X 1 mole Al 27g. Al X 1 mole Al2O3 X 102g Al2O3 2 mole Al 1 mole Al2O3 = 4.3 g Al2O3 2Al + Fe2O3 --> Al2O3 + 2Fe Methane burns in air by the following reaction: CH4 + 2O2 --> CO2 + 2H2O What mass of water is produced by burning 500. g of methane? 1 mole CH4 X 2 mole H2O 18g H2O 500.g CH4 X X 16g CH4 1 mole CH4 1 mole H2O = 1,130 g H2O Complete Worksheet #3 by next class! Turn in: Worksheet #3 Our Plan: Questions on WS 1-3 Stoichiometry Team Review Quiz WS 1 – 3 Lab Day 2 Homework (Write in Planner): Finish missing worksheets Molecules Molecules 6.022 x 1023 Mass Volume Molar Mass PT 22.4 L/mole 6.022 x 1023 Moles Given Molar Ratio Equation Moles Unknown Molar Mass PT Mass 22.4 L/mole Volume 1.14.78 2.2,822 3.8.4528 Turn in: Any Missing Worksheets Our Plan: Lab Day 3 Turn in Lab Today Homework (Write in Planner): Lab, if not done #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 100 WASH ALL SUPPLIES, RETURN TO SIDE TABLE, WIPE DOWN COUNTER, WASH HANDS! Clicker Review Turn in: Metal in Water Lab Our Plan: Relay Race Review Daily Challenge Notes – Stoichiometry of Gases and Molecules Worksheet #4 Homework (Write in Planner): WS#4 due next class 1. 2. 3. 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 Molecules Molecules 6.022 x 1023 Mass Volume Molar Mass PT 22.4 L/mole 6.022 x 1023 Moles Given Molar Ratio Equation Moles Unknown Molar Mass PT Mass 22.4 L/mole Volume Given the volume of one substance and asked to determine the volume of another substance. molar Vol 22.4 L Given Moles 22.4 L Moles ratio Given equation Unknown Vol Unkn Conversion factor: 22.4 L/mole You 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 How many moles of Helium are in a 3.7 L balloon at STP? 3.7 L x 1 mole = 0.17 mole 22.4 L 2 CO + O2 --> 2 CO2 What volume of carbon dioxide will be produced from 2.6 L of oxygen at STP? Molecules Molecules 6.022 x 1023 Mass Volume Molar Mass PT 22.4 L/mole 6.022 x 1023 Moles Given Molar Ratio Equation Moles Unknown Molar Mass PT Mass 22.4 L/mole Volume 2 CO + O2 --> 2 CO2 2.6 L O2 X 1 mole O2 X 2 mole CO2 X 22.4 L CO2 = 22.4 L O2 1 mole O2 5.2 L CO2 1 mole CO2 Using the same equation, what volume of carbon dioxide will be produced at STP from 45.3 grams of carbon monoxide? Molecules Molecules 6.022 x 1023 Mass Volume Molar Mass PT 22.4 L/mole 6.022 x 1023 Moles Given Molar Ratio Equation Moles Unknown Molar Mass PT Mass 22.4 L/mole Volume 2 CO + O2 --> 2 CO2 45.3 g CO X 1 mole CO X 2 mole CO2 X 22.4 L CO2 = 28 g CO 2 mole CO 36.2 L CO2 1 mole CO2 Using the same equation, what volume of oxygen is used to produce 19.3 grams of carbon dioxide at STP? (4.91 L) 2 CO + O2 --> 2 CO2 19.3 g CO2 X 1 mole CO2 X 1 mole O2 X 22.4 L O2 = 44 g CO2 2 mole CO2 4.91 L O2 1 mole O2 You can do the same type of problems using molecules. Just use Avogadro’s Number! In the reaction: 2H2 + O2 --> 2H2O if you have 0.50 grams of hydrogen, how many molecules of water will form? Molecules Molecules 6.022 x 1023 Mass Volume Molar Mass PT 22.4 L/mole 6.022 x 1023 Moles Given Molar Ratio Equation Moles Unknown Molar Mass PT Mass 22.4 L/mole Volume 0.50 g H2 X 1 mole H2 2 g H2 = X 2 mole H2O 2 mole H2 X 6.022 x 1023 molecules 1 mole H2O 1.5 x 1023 molecules H2O 2H2 + O2 --> 2H2O Cooking Planning outcomes of reactions Race cars/ mechanics Treating an upset stomach Airbags Artists Launching space shuttle Baking bread Engineering Complete Worksheet #4 by next class period! Turn in: Get Worksheet #4 Out to Check Our Plan: Balloon Races Limiting Reactant Notes Finish Balloon Races Handout Worksheet #5 Chemistry Cartoon Homework (Write in Planner): Worksheet 5 & Cartoon Due Next Class Molecules Molecules 6.022 x 1023 Mass Volume Molar Mass PT 22.4 L/mole 6.022 x 1023 Moles Given Molar Ratio Equation Moles Unknown Molar Mass PT Mass 22.4 L/mole Volume Pre 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. What did you predict would happen? What did happen? Why? Smore’s Recipe 2 Graham Crackers 3 Pieces of Chocolate 1 Marshmallow 1.If you have 4 graham crackers, 9 pieces of chocolate, and 7 marshmallows, how many smores can you make? 2.Which ingredient determined this? 3.If you have 22 graham crackers, 27 pieces of chocolate, & 13 marshmallows, how many smores can you make? 4.Which ingredient determined this? Even in abundance, the reactants must still combine in proportion They follow stoichiometry. Is the reactant that limits the amount of product formed in a chemical equation. Is the substance that is not used up completely in a reaction. The quantities of products formed in a reaction are always determined by the quantity of the limiting reactant. 1.Write a balanced equation 2.Convert the mass of reactants to the mass of the product. 3.Whichever produces less product is the limiting reactant. Identify the L.R when 10.0 g of water react with 4.50 g of sodium to produce sodium hydroxide & hydrogen gas. 2H2O + 2Na --> 2NaOH + H2 1 mol H2O 2 mol NaOH 40g NaOH 10.0 g X X X H2O 18g H2O 2 mol H2O 1 mol NaOH = 22.2 g NaOH 1 mol Na 2 mol NaOH 40g NaOH 4.50 g X X X Na 23g Na 2 mol Na 1 mol NaOH = 7.83 g NaOH Na= L.R. Identify the L.R when 8.90 g HF are combined with 14.56g SiO2 in the following reaction: SiO2 + 4HF --> SiF4 + 2H2O SiO2 + 4HF -->SiF4 + 2H2O 2 mol H O 1 mol HF 18g H2O 2 8.9 g HF X X X 20g HF 4 mol HF 1 mol H2O = 4.0 g H2O 1 mol SiO2 2 mol H2O 14.50g SiO2 X X 60g SiO2 1 mol SiO2 = 8.700 g H2O X 18g H2O 1 mol H2O HF= L.R. Finish Balloon Races Questions Worksheet #5 Chemistry Cartoon Turn in: Get Worksheet #5 Out to Check Turn in Chemistry Cartoon - Basket Our Plan: L.R. Review Problem Percent Yield Notes Worksheet #6 Homework (Write in Planner): Worksheet #6 Due Tuesday/Wednesday Acrylonitrile, C3H3N, is an important ingredient in the production of various fibers and plastics. Acrylonitrile is produced from the following reaction: C3H6 + NH3 + O2 --> C3H3N + H2O If 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 % 1.Babe Ruth played in 2503 baseball games in his career. He had 2873 hits in 8399 at bats what was his batting average? www.pbs.org 2.Hank Aaron played in 3298 baseball games in his career. He had 3771 hits in 12,364 at bats. What was his batting average? www.pbs.org Theoretical Yield is based on calculations Actual Yield is based on the actual chemical reaction (the lab) % yield = Actual yield X 100 Theoretical yield 1.Write equation 2.Calculate the mass of the product that should have been formed. (theoretical yield) 3.Plug numbers into the equation Determine the % yield for the reaction between 2.80 g Al(NO3)3 & excess NaOH if 0.966g Al(OH)3 is recovered. Write the equation: Al(NO3)3 + 3NaOH --> Al(OH)3 + 3NaNO3 Calculate theoretical yield 78g Al(OH)3 2.80 g 1 mol Al(NO3)3 1 mol Al(OH)3 X X Al(NO3)3 X 213g Al(NO3)3 1 mol Al(NO3)3 1 mol Al(OH)3 = 1.03 g Al(OH)3 Al(NO3)3 + 3NaOH --> Al(OH)3 + 3NaNO3 Plug numbers into equation 0.966g % yield = X 100 1.03g = 93.8% Determine the percent yield for the reaction between 15.0 g N2 & excess H2 if 10.5g NH3 is produced. 2 mol NH3 1 mol N2 17g NH3 15.0g N2 X X X 28g N2 1 mol NH3 1 mol N2 = 18.2 g NH3 %yield = 10.5g NH3 18.2 g NH3 X 100 = 57.7% You have to find the limiting reactant first. Calculate amount of product for both reactants & whichever is less, use as theoretical yield. Complete Worksheet #6 by next class! Turn in: Worksheet #6 Our Plan: Stoichiometry Lab Test Test Review Homework (Write in Planner): Test Review due next class UNIT 8 TEST NEXT CLASS! Turn in: Get out Test Review Our Plan: Questions on Test Review? Test Larry the Lawnchair Guy Reading Homework (Write in Planner): Larry Reading due next class Given the following reaction: C3H8 + 5O2 -------> 3CO2 + 4H2O If you start with 14.8 g of C3H8 and 3.44 g of O2, determine the limiting reagent Given the following equation: H3PO4 + 3 KOH ------> K3PO4 + 3 H2O If 49.0 g of H3PO4 is reacted with excess KOH, determine the percent yield of K3PO4 if you isolate 49.0 g of K3PO4. Given the following equation: Al(OH)3 +3 HCl --> AlCl3 + 3 H2O If you start with 50.3 g of Al(OH)3 and you isolate 39.5 g of AlCl3, what is the percent yield? Given the following equation: H2SO4 + Ba(OH)2 ----> BaSO4 + H2O If 98.0 g of H2SO4 is reacted with excess Ba(OH)2, determine the percent yield of if 213.7 g of BaSO4 is formed. http://www.youtube.com/watch?v=NC- Km7aUjgc