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1 Stoichiometry Please take out your notebooks

2 Stoichiometry stochio = Greek for element metry = measurement Stoichiometry is about measuring the amounts of elements and compounds involved in a reaction. Consider the chemical equation: 4NH 3 + 5O 2 6H 2 O + 4NO There are several numbers involved. What do they all mean?

3 Stoichiometry Recall that Chemical formulas represent numbers of atoms 4NH 3 + 5O 2 6H 2 O + 4NO NH 3 1 nitrogen and 3 hydrogen atoms O 2 2 oxygen atoms H 2 O NO 2 hydrogen atoms and 1 oxygen atom 1 nitrogen atom and 1 oxygen atom

4 Stoichiometry Recall that Chemical formulas have molar masses: 4NH 3 + 5O 2 6H 2 O + 4NO NH 3 17 g/mol O 2 32 g/mol H 2 O NO 18 g/mol 30 g/mol

5 Stoichiometry 4NH 3 + 5O 2 6H 2 O + 4NO Recall that Chemical formulas are balanced with coefficients 4 X NH 3 = 4 nitrogen + 12 hydrogen 5 X O 2 = 10 oxygen 6 X H 2 O = 12 hydrogen + 6 oxygen 4 X NO = 4 nitrogen + 4 oxygen

6 Stoichiometry 4NH 3 + 5O 2 6H 2 O + 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.

7 Stoichiometry 4NH 3 + 5O 2 6H 2 O + 4NO 4 : 5 : 6 : 4 Can mean either: 4 molecules of NH 3 react with 5 molecules of O 2 to produce 6 molecules of H 2 O and 4 molecules of NO OR 4 moles of NH 3 react with 5 moles of O 2 to produce 6 moles of H 2 O and 4 moles of NO

8 Question 1 4NH 3 + 5O 2 6H 2 O + 4NO How many moles of H 2 O are produced if 2.00 moles of O 2 are used? 2.00 mol O 2 6 mol H 2 O 5 mol O 2 = 2.40 mol H 2 O *Notice that a correctly balanced equation is essential to get the right answer

9 Question 2 4 NH O 2 6 H 2 O + 4 NO How many moles of NO are produced in the reaction if 15 mol of H 2 O are also produced? 4 mol NO 15 mol H 2 O = 10. mol NO 6 mol H 2 O

10 Stoichiometry Path We always use the same type of information to make the jumps between steps: Molar mass of x Molar mass of y grams (x) moles (x) moles (y) grams (y) Mole ratio from balanced equation

11 Stoichiometry Path We will be converting: Moles to Moles Grams to Grams

12 Practice Try these on your own - 4 NH O 2 6 H 2 O + 4 NO 1) How many moles of H 2 O can be made using 1.6 mol NH 3?

13 Answers 4 NH O 2 6 H 2 O + 4 NO 1) 1.6 mol NH 6 mol H 2 O 2.4 mol 3 x = 4 mol NH 3 H 2 O How many moles of H 2 O can be made using 1.6 mol NH 3?

14 Practice Try these on your own - 4 NH O 2 6 H 2 O + 4 NO 2) How many moles of NO can be made using 1.6 mol NH 3?

15 Answers 4 NH O 2 6 H 2 O + 4 NO 2) 1.6 mol NH3 x 4 mol NO 4 mol NH3 = 1.6 mol NO How many moles of NO can be made using 1.6 mol NH 3?

16 Practice Try these on your own - 4 NH O 2 6 H 2 O + 4 NO 3) How many grams of NO can be made from 47 g of NH 3?

17 Answers 4 NH O 2 6 H 2 O + 4 NO How many grams of NO can be made from 47 g of NH 3? g NH 3 x 1 mol NH g NH 3 x 4 mol NO 4 mol NH 3 x g NO 1 mol NO = 83 g NO

18 Limiting Reactant

19 Limiting Reactant The limiting reagent in a chemical reaction is the substance that is totally consumed when the chemical reaction is complete.

20 Limiting Reactant The limiting reagent is the reactant that gets used up first during the reaction and also determines how much product can be made. We can find the limiting reagent using the stoichiometric ratios from the balanced chemical reaction. Once we know the limiting reagent, we can calculate how much product will be produced, known as the theoretical yield.

21

22 Limiting Reactant Example What is the limiting reagent if we start with 2.8 grams of Al and 4.25 grams of Cl 2? 2Al + 3Cl 2 2AlCl 3

23 Limiting Reactant Example What is the limiting reagent if we start with 2.8 grams of Al and 4.25 grams of Cl 2? 2Al + 3Cl 2 2AlCl 3 Step 1: convert grams to moles 2.80 g x 1 mol = mol Al 27 g 4.25 g x 1 mol = mol Cl 70 g

24 Limiting Reactant Example What is the limiting reagent if we start with 2.8 grams of Al and 4.25 grams of Cl 2? 2Al + 3Cl 2 2AlCl 3 Step 1: mol Al & mol Cl Step 2: Find the stoichiometric ratio of each mol Al = X 2 AlCl3 2 Al AlCl moles produced mol Cl = X 2 AlCl3 3 Cl AlCl moles produced Cl2 is limiting since it is less!

25 Limiting Reactant Example What is the limiting reagent if we start with 4 grams of CH 4 and 80 grams of O 2? CH O 2 CO H 2 O Step 1: convert grams to moles Step 2: Find the stoichiometric ratio

26 Limiting Reactant Example What is the limiting reagent if we start with 4 grams of CH 4 and 80 grams of O 2? CH O 2 CO H 2 O Step 1: CH 4 = 0.25 moles Step 2: 0.25 CH4 X 2 mole H2O = 0.5 H2O 1 mole CH4 CH4 = Limiting Reactant! moles produced O 2 = 1.25 moles 1.25 mol O2 X 2 mole H2O = 2 mol O H2O mol produced

27 On the page before, try the same problem but use CO2 as your product. How much H2O and CO2 would be produced?

28 Theoretical Yield

29 Theoretical Yield Theoretical yield is the amount of product that will be created based on the limiting factor.

30 Theoretical Yield Example What is the theoretical yield AlCl 3 that the reaction can produce with 4.25 grams of Cl 2, our limiting reagent? 2Al + 3Cl 2 2AlCl 3 Step 1 : find out how many moles of AlCl3 are created mol Cl x 2 mole AlCl 3 = moles AlCl 3 3 mole Cl 2

31 Theoretical Yield Example What is the theoretical yield AlCl 3 that the reaction can produce with 4.25 grams of Cl 2, our limiting reagent? 2Al + 3Cl 2 2AlCl 3 Step 1 : find out how many moles of AlCl3 are created Answer: moles AlCl 3 Step 2: convert moles to grams of AlCl moles AlCl3 x 133 grams (molar mass of AlCl3) = 1 mole 5.32 grams of AlCl 3

**continued on next page**

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