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6/12/2018 Stoichiometry Milwaukie High School.

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1 6/12/2018 Stoichiometry Milwaukie High School

2 Notes One Unit 4 Making Cookies Making Chemicals Stoichiometry
6/12/2018 Notes One Unit 4 Making Cookies Making Chemicals Stoichiometry Moles-Moles Calculation A 401, A 402A Read pgs

3 Making Cookies

4 Making Cookies 64 cookies 160 cookies 128 cookies 16 cookies
What does the following recipe tell us? 1 C butter +1 C sugar +2 egg yolks +1/4 C vegetable oil +1/2 C cocoa + 2 tsp vanilla + 2-1/4 C flour + 1/4 tsp salt +1 C Chocolate Powder + 4 Oz semisweet chocolate, 2 TBS cream 32 Mud Puddle Cookies How many cookies can be made with… 2 cups of butter and 10 eggs? 64 cookies 160 cookies 4 cups of sugar and 1 Egg? 128 cookies 16 cookies 1-1/8 of C flour and 8 cups of oil? 16 cookies 1024 cookies 0.25 8 Cookies_____ cups butter? 1.5 24 Cookies_____ tsp vanilla? 4 64 Cookies_____ egg yolks?

5 Making Chemicals

6 Stoichiometry Consider the chemical equation: 4NH3 + 5O2  6H2O + 4NO
6/12/2018 “stoichio” = Greek for element “metry” = measurement Stoichiometry is about measuring the amounts of elements and compounds involved in a reaction. Quantitative study of reactants and products in chemical reactions. Consider the chemical equation: 4NH3 + 5O2  6H2O + 4NO There are several numbers involved. What do they all mean? What are reactants? The starting substance in a chemical reaction The arrow means “react to form” or “yield” What are products? A substance that results from a reaction Stoichiometry answers the question… How much product will we get from a given amount of reactant? Stoichiometry (stoich) uses the ratios in a balanced chemical equation Stoichiometry is used in chemistry labs with large amounts of substances, therefore Stoich uses the ratios in MOLES instead of molecules

7 Stoichiometry 4NH3 + 5O2  6H2O + 4NO NH3 O2 H2O NO
6/12/2018 4NH3 + 5O2  6H2O + 4NO Recall that Chemical formulas represent numbers of atoms NH3 1 nitrogen and 3 hydrogen atoms O2 2 oxygen atoms H2O 2 hydrogen atoms and 1 oxygen atom NO 1 nitrogen atom and 1 oxygen atom The chemical formula of a substance is a notation that uses atomic symbols with numerical subscripts to convey the relative proportions of atoms of the different elements in the substance

8 Recall that Chemical formulas have molar masses:
Stoichiometry 4NH3 + 5O2  6H2O + 4NO Recall that Chemical formulas have molar masses: NH3 17.0 g/mol O2 32.0 g/mol H2O 18.0 g/mol NO 30.0 g/mol ***To find the molar mass of a chemical formula – add the atomic masses of the elements forming the compound. Use the periodic table to determine the atomic mass of individual elements.***

9 Recall that Chemical formulas are balanced with coefficients
Stoichiometry 6/12/2018 4NH3 + 5O2  6H2O + 4NO Recall that Chemical formulas are balanced with coefficients 4 X NH3 = 4 nitrogen + 12 hydrogen 5 X O2 = 10 oxygen 6 X H2O = 12 hydrogen + 6 oxygen 4 X NO = 4 nitrogen + 4 oxygen The coefficients in a chemical equation can be interpreted as the ratio of molecules of each substance. When no coefficient is written, it is understood to be 1.

10 Stoichiometry 4NH3 + 5O2  6H2O + 4NO
With Stoichiometry we find out that 4 : 5 : 6 : 4 do more than just multiply atoms. 4 : 5 : 6 : 4 Are what we call a mole ratio.

11 4 : 5 : 6 : 4 Stoichiometry 4NH3 + 5O2  6H2O + 4NO OR
6/12/2018 4NH3 + 5O2  6H2O + 4NO 4 : 5 : 6 : 4 Can mean either: 4 molecules of NH3 react with 5 molecules of O2 to produce 6 molecules of H2O and 4 molecules of NO OR 4 moles of NH3 react with 5 moles of O2 to produce 6 moles of H2O and 4 moles of NO

12 Stoichiometry Example (1) moles of reactants  moles of products
6/12/2018 Stoichiometry Example (1) moles of reactants  moles of products  A reaction takes place between Lithium and water: Li(s) + H2O (l)  LiOH(aq) + H2 (g) Question: How many moles of H2 will be formed if 6.23 moles of Li combine with water?

13 6/12/2018 Stoichiometry Example (1) Continued Question: How many moles of H2 will be formed if 6.23 moles of Li combine with water? 1. Balance the equation using coefficients 2Li(s) + 2 H2O (l)  2 LiOH(aq) + 1H2 (g) 2. Convert the required amount to moles *do not need this step for this question* 6.23 moles of Li (from question)

14 6/12/2018 Stoichiometry Example (1) Continued Question: How many moles of H2 will be formed if 6.23 moles of Li combine with water? 3. Find the mole ratio using the coefficients. 2Li(s) + 2 H2O (l)  2 LiOH(aq) + 1 H2 (g) 2 moles of Li = 1 mole H2 4. Convert to desired unit The question asked for moles so 3.12 moles H2 doesn’t need to be converted and is the final answer.

15 Stoichiometry Question (1)
4NH3 + 5O2  6H2O + 4NO How many moles of H2O are produced if 2.00 moles of O2 are used? 6 mol H2O 5 mol O2 2.00 mol O2 = 2.40 mol H2O Notice that a correctly balanced equation is essential to get the right answer

16 Stoichiometry Question (2)
4 NH O2  6 H2O NO How many moles of NO are produced in the reaction if 15 mol of H2O are also produced? 4 mol NO 6 mol H2O 15 mol H2O = 10. mol NO

17 Notes Two Unit Four Mass-Mass Calculation A 402B
6/12/2018 Notes Two Unit Four Mass-Mass Calculation A 402B Group Assignment GA 402 Read pgs Do A403 during break!

18 Stoichiometry Read the chemical equation: 4NH3 + 5O2  6H2O + 4NO
6/12/2018 “stochio” = Greek for element “metry” = measurement Stoichiometry is about measuring the amounts of elements and compounds involved in a reaction. Quantitative study of reactants and products in chemical reactions. Read the chemical equation: 4NH3 + 5O2  6H2O + 4NO Molar Ratios and writing equations review

19 Balanced Equations Have Ratios
The coefficients in a chemical equation can be interpreted as the ratio of molecules of each substance. 2 CO(g) O2 (g)  CO2 (g) The image and the Balance equation mean: 2 molecules of CO reacts with 1 molecule of oxygen gas to generate 2 molecules of CO2

20 What Does The Ratio Mean? 2 CO(g) + O2 (g)  2 CO2 (g)
6/12/2018 What Does The Ratio Mean? 2 CO(g) O2 (g)  CO2 (g) If I have 6 moles of CO and 6 moles of O2 can I make 6 moles of CO2? (HINT… think how many CO must reach with each O2? 6 moles CO(g) moles O2 (g)

21 Ratio 2 CO(g) + O2 (g)  2 CO2 (g)
I can’t make 6 moles of CO2 because for every one O2 mole I need 2 CO moles That means I will run out of CO moles after I react with 3 O2 moles. 1 2 3

22 Results 6 molecules of CO create 3 molecules CO2 2 to 1 ratio
6/12/2018 Results 6 molecules of CO create 3 molecules CO2 2 to 1 ratio

23 Results Continued 6 molecules of O2 create 6 molecules CO2
1 to 1 ratio

24 Moving Along The Stoichiometry Path
6/12/2018 Moving Along The Stoichiometry Path We always use the same type of information to make the jumps between steps: grams (x)  moles (x)  moles (y)  grams (y) Molar mass of y Molar mass of x Mole ratio from balanced equation We can start anywhere along this path depending on the question we want to answer ** Notice we can’t directly convert from grams of one compound to grams of another. We must go through moles using the mole ratio.**

25 Mass-Mass Calculation (1)
6/12/2018 How many grams of ammonia will be made reacting with 14.0 grams of nitrogen reaction with hydrogen? 1N2(g) H2(g) 2NH3(l) 1 mol N2 28.0 g N2 2 mol NH3 1 mol N2 17.0 g NH3 1 mol NH3 14.0 g N2 17.0g NH3 =

26 Mass-Mass Calculation (2)
6/12/2018 How many grams of hydrogen will be formed by a reaction of 80.5g of lithium with water?  2 Li(s) H2O (l)  LiOH(aq) H2 (g) 1 mol Li 6.9 g Li 1 mol H2 2 mol Li 2.0 g H2 1 mol H2 80.5 g Li 11.7 g H2 =

27 Mass-Mass Calculation (3)
6/12/2018 How many grams of NO2 are formed by reacting 1.44 grams of NO with oxygen gas? 2NO(g) + O 2(g) → 2NO2(g) 1 mol NO 30.0 g NO 2 mol NO2 2 mol NO 46.0 g NO2 1 mol NO2 1.44 g NO 2.21 g NO2 =

28 Have We Learned It Yet? Try these on your own NH3 + 5 O2  6 H2O + 4 NO a) How many moles of H2O can be made using 1.6 mol NH3? b) How many grams of NO can be made from 47 g of NH3?

29 Answers 2.4 mol H2O 83 g NO 4 NH3 + 5 O2  6 H2O + 4 NO a) b)
6/12/2018 Answers 4 NH O2  6 H2O NO a) b) 1.6 mol NH3 6 mol H2O 4 mol NH3 2.4 mol H2O = 4 mol NO 4 mol NH3 47 g NH3 1 mol NH3 17.0 g NH3 30.0 g NO 1 mol NO 83 g NO =

30 Let’s Put All The Steps Together!
6/12/2018 Let’s Put All The Steps Together! Factor label Method: it uses UNITS to cancel and work your way through the problem Given Info (g) Mole Given (mol) Moles Requested MM Requested (g) of Requested (g) MM Given (g) Moles Given 1 Mole Requested = Given Mole to Mole Requested The given converts grams of given to moles of given. The middle converts moles of given to moles of requested. The requested converts moles of requested to grams of requested. All in one multistep process !!! THIS IS A MASS MASS PROBLEM.

31 Chemistry Purgatory Notes Three Unit Four
6/12/2018 Chemistry Purgatory Notes Three Unit Four CA 401 Mass-Mass Calculations

32 6/12/2018 Remember Stoich?? Allow Hank Green to remind you what we’ve been doing so far

33 6/12/2018 Steps To Follow Stoich

34 Mass-Mass Calculation (4)
6/12/2018 How many grams of carbon dioxide will be made by burning 6.00 grams of Isovanillin? 1C8H8(l) O2(g) 8 CO2(g) + 4 H2O(g) 1 mol C8H8 104.0 g C8H8 8 mol CO2 1 mol C8H8 44.0 g CO2 1 mol CO2 6.00 g C8H8 20.3 g CO2 =

35 Mass-Mass Calculation (5)
6/12/2018 How many grams of silver will be made by decomposing 8.00 grams of Silver oxide? 2Ag2O(s) 1O2(g)+ 4Ag(s) 1 mol AgO 231.8 g AgO 4 mol Ag 2 mol AgO 107.9 g Ag 1 mol Ag 8.00 g AgO 7.45 g Ag =

36 Notes Four Unit Four Limiting Reactant Mass-Mass Problem Molar Volume
6/12/2018 Notes Four Unit Four Limiting Reactant Mass-Mass Problem Molar Volume Mass-Volume Problem

37 6/12/2018 Limiting Reactants If the moles of the reactants exactly matches the molar ratio, then both reactants are completely consumed Otherwise, one of the reactants is only partially consumed The reactant that is used up is called the limiting reactant, since it is the one that stops the reaction My analogy: stick to cheese and ham sandwiches. My recipe: you need 2 slices of bread,1 slice of cheese and 3 slices of ham to make a cheese and ham sandwich. If you had 10 slices of bread, 6 slices of cheese and 12 of ham, how many cheese and ham sandwichs can you make? The equation is: 1c+ 2b+ 3h --> 1sandwich We are told we have:6c+ 10b+ 12h --> ?sandwichs One method is: 6 mol of cheese/1 mol of cheese= 6 mol of cheese 10 mol of bread/2 mol of bread= 5 mol of bread 12 mol of ham/3 mol of ham= 4 mol of ham The reactant present in smaller amount is the limiting reactant. In this case the ham, since it has the least number of mole. THe other two reactants the cheese and bread are in excess. This method required us to divide the moles of each reactant by its stoichiometric coefficient and then compare the three reactants to eachother. 

38 Determining Limiting Reactant
6/12/2018 How many grams of ammonia will be made reacting with 14.0 grams of nitrogen with 7.0 g of hydrogen? 1N2(g) H2(g) 2NH3(l) 1 mol N2 28.0 g N2 2 mol NH3 1 mol N2 17.0 g NH3 1 mol NH3 14.0 g N2 17.0 g NH3 = 1 mol H2 2.0 g H2 2 mol NH3 3 mol H2 17.0 g NH3 1 mol NH3 7.0 g H2 89 g NH3 = Nitrogen Is the Limiting Reactant

39 Limiting Reactant Problem
6/12/2018 How many grams of C6H4Cl2(s) will be made reacting 24.0 grams of benzene with 77.0 g of chlorine? 1C6H6(l) + 2Cl2(g)  1 C6H4Cl2(s) HCl(g) 24.0 g C6H6 1 mol C6H6 28.0 g C6H6 1 mol C6H4Cl2 1 mol C6H6 147.0 g C6H4Cl2 1 mol C6H4Cl2 126 g C6H4Cl2 = 77.0 g Cl2 1 mol Cl2 71.0 g Cl2 1 mol C6H4Cl2 2 mol Cl2 147.0 g C6H4Cl2 1 mol C6H4Cl2 Benzene C6H6 Is the Limiting Reactant 159 g C6H4Cl2 =

40 22.4L/mol 22.4L/mol Molar Volume @STP 1molN2(g) = 28.0g/mol 22.4L/mol
1molO2(g) = 32.0g/mol 22.4L/mol How do we weigh gases on a scale? We don’t we measure volume. Gases are mostly made up of empty space. One mole of any gas occupies the same volume 1molAr(g)= 39.9g/mol 22.4L/mol

41 Mass-Volume Calculation
How many liters of ammonia will be made reacting 56.0 grams of nitrogen with STP? 1N2(g) H2(g) 2 NH3(l) 1 mol N2 28.0 g N2 2 mol NH3 1 mol N2 22.4 l NH3 1 mol NH3 56.0 g N2 89.6 L NH3 =

42 Volume-Volume Calculation
How many liters of ammonia will be made reacting 33.6 liters of nitrogen with 1N2(g) H2(g) 2NH3(l) 1 mol N2 22.4 l N2 2 mol NH3 1 mol N2 22.4 l NH3 1 mol NH3 33.6 l N2 67.2 L NH3 =

43 6/12/2018 Extra

44 Stoichiometry Question (3)
4 NH O2  6 H2O NO How many grams of H2O are produced if 2.2 mol of NH3 are combined with excess oxygen? 6 mol H2O 4 mol NH3 2.2 mol NH3 18.0 g H2O 1 mol H2O 59 g H2O =

45 Stoichiometry Question (4)
4 NH O2  6 H2O NO How many grams of O2 are required to produce 0.3 mol of H2O? 5 mol O2 6 mol H2O 32.0 g O2 1 mol O2 0.3 mol H2O 8 g O2 =

46 Stoichiometry Question (5)
4 NH O2  6 H2O NO How many grams of NO is produced if 12 g of O2 is combined with excess ammonia? 1 mol O2 32.0 g O2 4 mol NO 5 mol O2 30.0 g NO 1 mol NO 12 g O2 9.0 g NO =

47 Have we learned it yet? Try these on your own NH3 + 5 O2  6 H2O + 4 NO a) How many moles of H2O can be made using 1.6 mol NH3? b) What mass of NH3 is needed to make 0.75 mol NO? c) How many grams of NO can be made from 47 g of NH3?

48 Answers 2.4 mol H2O 13 g NH3 83 g NO 4 NH3 + 5 O2  6 H2O + 4 NO a)
b) c) 1.6 mol NH3 6 mol H2O 4 mol NH3 2.4 mol H2O = 4 mol NH3 4 mol NO 17.0 g NH3 1 mol NH3 13 g NH3 = 0.75 mol NO 4 mol NO 4 mol NH3 1 mol NH3 17.0 g NH3 30.0 g NO 1 mol NO 47 g NH3 83 g NO =

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