1. (Stoo-eek-ee-aam-et-ry)
Stoichiometry
(Stoo-eek-ee-aam-et-ry)

2. 9.1 Using Chemical Equations
How many sandwiches can you make? 20 pieces of bread, 44 slices of tomatoes, 332 slices of meat and 4 slices of cheese.  + + +
1 piece of bread + 3 tomato slices + 3 slices meat + 2 cheese slices  1 sandwich

3.  + ___ F2 + ___ W3  ____ FW2 F = frame, W = wheel
Wheels come in packages of 3
Frames come in packages of 2
A bike factory is manufacturing bikes. A bike is made from one frame and two wheels. Write a balanced equation for producing bikes. (A bike, of course, is FW2).
___ F2 + ___ W3  ____ FW2  +

4. ___ F2 + ___ W3  ____ FW2  +

5. If we order 12 cases of frames, how many cases of wheels will we need?
Use dimensional analysis! (Applause)
The numbers in the parenthesis come from the balanced chemical equation

6. Using Chemical Equations
The coefficients can represent
the number of molecules and atoms OR
The moles of molecules and atoms
N2(g) H2(g)  2NH3(g)
1 molecule N2 + 3 molecules H2  2 molecules NH3
1 mol N mol H  2 mol NH3

7. Mole Ratio: The ratio between two chemicals in a balanced chemical equation. It is used as a conversion factor.
____ Fe + ____ O2  ____ Fe2O3
4. The mole ratio for O2 to Fe2O3 is
___ mol O2 : ___ mol Fe2O3
5. How many moles of O2 are needed to form 21.0 moles of Fe2O3?
(Convert 21.0 mol Fe2O3 to mol O2)
21.0 mol Fe2O3 ______________ =

8. Stoichiometry (stoik ee ahm ih tree)Using mole ratios to convert from an amount of one substance to the amount of another substance
If you know the amount of chemical A and you want to know the amount of chemical B, then it is just converting moles of A to moles of B using the mole ratio.

9. 6. Questions may ask for the answer as a mass (in grams) rather than moles.
*Example: How many grams of Fe2O3 are
formed when 6.00 moles of O2 react?
a. Convert ____________ to ____________
b. Still use the mole ratio, but then convert mol Fe2O3 to g Fe2O3 a separate step.
6.00 mol O mol Fe2O __________
mol O2

10. 7. Or, the question could start with the mass of the given chemical.
What mass (in grams) of Fe is needed to react with 525 g of O2?

11. Limiting Reactant and Percent Yield

12. A new adventure in sales
We are going to sell hot dogs on the street (to raise money for chemistry experiments).
Each hot dog we sell will require one bun and one hotdog, so we order 200 packages of each.
But then we find that hot dogs are in packages of 10 and buns are in packages of 8.
So, which will we use up first? Hot dogs or buns? 12

13. So…
Since the hot dog business was to unprofitable (400 extra hot dogs got moldy while in storage waiting for the state fair), we go back to bikes. 13

14. Bike stoichiometry F = frame, W = wheel Wheels come in packages of 3
Frames come in packages of 2
3 packages of frames and 4 packages of wheels make six bikes:
3 F2 + 4 W3  6 FW2
We have 21 cases of frames left in storage, but no wheels. How many packages of wheels must we buy?
Oops. Actually, I just found 24 packages of wheels under my desk. So, do we use up the wheels, or do we have extra wheels? 14

15. Mole Ratio: The ratio between two chemicals in a balanced chemical equation. It is used as a conversion factor.
4 Fe + 6 O2  2 Fe2O3
The mole ratio for O2 to Fe2O3 is 6 mol O2 / 2 mol Fe2O3

16. 9.2 Calculating mass You can think of a chemical equation as
Number of molecules, moles AND grams
N2(g) H2(g)  2NH3(g)
1 molecule N2 + 3 molecules H2  2 molecules NH3
1 mol N mol H  2 mol NH3
28 g N x 2.02 g H2  2 x 17g NH3

17. 9.2 Calculating mass
How many grams of NH3 can be made from 38.4 grams H2?
N2(g) + 3H2(g)  2NH3(g)
The equation only gives the “mole” ratio, so we need to convert grams to moles.
Plan:
Grams H2  moles H2  moles NH3  grams NH3

18. 38.4 g H2 grams NH3 moles H2 moles NH3 17.04 g/ mol NH3 2.02 g/ mol H2
2 mol NH3/ 2 mol H2
moles H2
moles NH3

19. 9.3 Limiting Reactants and Percent Yield

21. Imagine that we want to make sandwiches (and I love sandwiches). + + +
We have: 20 pieces of bread, 44 slices of tomatoes, 332 slices of meat and 4 slices of cheese.
How many sandwiches can you make?
Yes, two. We need to buy more cheese if we want to make more, and I want to watch the soccer game, so I can’t go to the store right now.

22. Determining the Limiting Reactant
In the sandwich example, cheese was the limiting reactant (also called “limiting reagent).
The limiting reactant is completely used up in a reaction. 22

23. 3 F2 + 4 W3  6 FW2
We have 21 cases of frames left in storage, but no wheels. How many packages of wheels must we buy? (Show work!)
Oops. Actually, I just found 24 packages of wheels under my desk. So, do we use up the wheels, or do we have extra wheels?

24. N2(g) + 3H2(g)  2NH3(g)
To use all 16.0 mol N2, you would need 48.0 mol H2.
So what if you had 16.0 mol N2 and 19.0 mol H2. Which would you use up first?

25. Now, with chemicals N2 + 3 H2  2 NH3
You have 16.0 moles of N2. How many moles of H2 would be required? 25

27. Using the Limiting Reactant
You have 16.0 mol N2 and 19.0 mol H2. How many moles of NH3 will form?
Since limiting reactant controls the amount of product formed, just convert from 19.0 mol H2 to mol NH3.
How many moles of the excess reactant would remain? 27

28. Example: 25. 0 kg N2 react with 5. 00 kg H2
Example: 25.0 kg N2 react with 5.00 kg H2. How much ammonia (NH3) will be made?
N2(g) + 3H2(g)  2NH3(g)
Calculate moles of H2 and N2.
Calculate how many moles N2 you need to react with H2. Use the mole ratio.
3. Ask yourself: Do you have enough H2?
Yes  H2 is excess, N2 is limiting.
No  H2 is limiting, N2 is excess
4. Use the limiting reactant to calculate grams NH3.

29. Tin(II) fluoride is used in some toothpastes.
It is made by reacting tin with hydrogen fluoride to produce tin(II) fluoride and hydrogen gas.
Write a balanced chemical equation for this reaction.
You have 3.15 mol of Sn and 4.96 mol HF.
Which is the limiting reactant (show work!)?
How many moles of tin(II) fluoride will form?
You have 21.1 g Sn and 84.5 g HF.
Which will be limiting?
What mass of tin(II) fluoride will form? 29

30. Percent Yield
In a real experiment, usually you get less product than you would expect. Sometimes not all the chemicals react.
Theoretical Yield – calculated amount of product
Actual Yield – amount of product actually collected in lab
Knowing both of these, you can calculate percent yield.
% yield = actual yield  theoretical yield 30

31. Example
In an experiment, Jenny collected 57.1 g of product. However, stiochiometrically she calculated that she should have gotten 66.8 g. Find the percent yield.
57.1 g  100% = 85.5% yield g 31