1. Stoichiometry

2. Airports Charles Hartsfield De Gaulle Birmingham Barcelona Chattanooga
Manchester
Columbia, SC
Provence

3. Chemical Reactions Known Unknown Mole Mole Mass Mass Volume Volume
Substance A Substance B
Mass
Mass
1 mole = molar mass (g)
1 mole = molar mass (g)
Use coefficients
from balanced
chemical equation
Volume
Mole
Mole
Volume
1 mole = STP
1 mole = STP
(gases)
(gases)
1 mole = x 1023 particles
(atoms or molecules)
1 mole = x 1023 particles
(atoms or molecules)
Particles
Particles

4. Practice Problems
When 80 grams of aluminum is reacted with excess chlorine gas, how many formula units of AlCl3 are produced?
2Al +3Cl2→2AlCl3 
What are you given?
What do you want to find?
Sketch a path through the airport diagram to get from what you’re given to what you want.

5. Sb2S3(s) + 3Fe(s)→2Sb(s) +3FeS(s)
Practice Problems
If 3.87×1023 particles of Sb2S3(s) are reacted with excess Fe(s), what mass of FeS(s) is produced?
Sb2S3(s) + 3Fe(s)→2Sb(s) +3FeS(s) 
What are you given?
What do you want to find?
Sketch a path through the airport diagram to get from what you’re given to what you want.

6. Practice Problems
At STP, what volume of H2(g) is needed to react completely with 8.02×1023molecules of CO(g)?
CO(g) +2H2(g)→CH3OH(g)  
What are you given?
What do you want to find?
Sketch a path through the airport diagram to get from what you’re given to what you want.

7. 4NH3(g) + 6NO(g)→5N2(g) + 6H2O(g)
Practice Problems
How many moles of each reactant were there if 13.7 moles of N2(g) is produced.
4NH3(g) + 6NO(g)→5N2(g) + 6H2O(g)
What are you given?
What do you want to find?
Sketch a path through the airport diagram to get from what you’re given to what you want.

8. Stoichiometry Methods
Verify that the chemical equation is balanced
Write down what the problem gives you
Write down what the problem asks you to find
Sketch the air port diagram and draw your path through it.
Write out the conversion factors that you will need
Complete the conversion
Verify that the units you get are the units you wanted

9. Water from a Camel
Camels store the fat tristearin (C57H110O6) in the hump. As well as
being a source of energy, the fat is a source of water, because when
it is used the reaction
takes place.
2 C57H110O6(s) O2(g)  114 CO2(g) H2O(l)
What mass of water can be made from 1.0 kg of fat?

10. 2 C57H110O6(s) + 163 O2(g)  114 CO2(g) + 110 H2O(l)
Water from a Camel
Verify that the equation is balanced:
2 C57H110O6(s) O2(g)  114 CO2(g) H2O(l)
Clickers:
Balanced
Not Balanced A
Reactants
Products
C: 114
H: 220
O: 338

11. Water from a Camel 2. Write down what the problem gives you:
Camels store the fat tristearin (C57H110O6) in the hump. As well as
being a source of energy, the fat is a source of water, because when
it is used the reaction takes place. What mass of water can be made from 1.0 kg of fat?

12. Water from a Camel 3. Write down what the problem asks you to find:
Camels store the fat tristearin (C57H110O6) in the hump. As well as
being a source of energy, the fat is a source of water, because when
it is used the reaction takes place. What mass of water can be made from 1.0 kg of fat?

13. 4. Draw airport diagram Unknown Mass H2O 1 kg Fat Moles Fat Moles H2O
1 mole = molar mass (g)
Moles Fat
Moles H2O
1 mole = molar mass (g)
Use coefficients
from balanced
chemical equation
Volume
Mole
Mole
Volume
1 mole = STP
1 mole = STP
(gases)
(gases)
1 mole = x 1023 particles
(atoms or molecules)
1 mole = x 1023 particles
(atoms or molecules)
Particles
Particles

14. Water from a Camel
5. Write out the conversion factors 1 kg C57H110O6 = 1000 g C57H110O6 890 g C57H110O6 = 1 mol C57H110O6 2 mol C57H110O6 = 110 mol H2O 1 mol H2O = 18 g H2O

15. 6. Complete the Conversion
1000 g “fat”
1 mol “fat”
110 mol H2O
18 g H2O
x g H2O = 1 kg ‘fat”
1 kg “fat”
890 g “fat”
2 mol “fat”
1 mol H2O
X = g H2O

16. Water from a Camel
7. Verify that the units you get are the units you wanted From Step 3: From Step 6: X = 1112 g H2O
Camels store the fat tristearin (C57H110O6) in the hump. As well as
being a source of energy, the fat is a source of water, because when
it is used the reaction takes place. What mass of water can be made from 1.0 kg of fat?

17. Rocket Fuel
The compound diborane (B2H6) was at one time
considered for use as a rocket fuel. How many grams
of liquid oxygen would a rocket have to carry to burn
10 kg of diborane completely?
(The products are B2O3 and H2O).
B2H6 + O2
B2O3 + H2O
Chemical equation

18. Clicker Question 2 Is this chemical equation balanced? Yes No
B2H6 + O2
B2O3 + H2O B

19. Clicker Question 4
Which of the following ratios represents a balanced equation for this chemical reaction?
1:1:2:3
1:2:1:2
1:3:1:3
2:3:1:1
B2H6 + O2
B2O3 + H2O C

20. Clicker Question 5 What is the molar mass of B2H6? 27.68 g/mol
8.00 g/mole
32.45 g/mole A

21. Clicker Question 6
According to the balanced equation below, how many moles of O2 do you get for each mole of B2H6? 1 2 3 4
B2H O B2O H2O C

22. Clicker Question 7 What is the molar mass of O2? 15.99 g/molD

23. Rocket Fuel B2H6 + O2 B2O3 + H2O B2H6 + O2 B2O3 + 3H2O 3 3
The compound diborane (B2H6) was at one time
considered for use as a rocket fuel. How many grams
of liquid oxygen would a rocket have to carry to burn
10 kg of diborane completely?
(The products are B2O3 and H2O).
B2H6 + O2
B2O3 + H2O
Chemical equation
Balanced chemical equation
B2H O B2O H2O 3 3
10 kg x g
1000 g B2H6
1 mol B2H6
3 mol O2
32 g O2
x g O2 = 10 kg B2H6
1 kg B2H6
28 g B2H6
1 mol B2H6
1 mol O2
X = 34,286 g O2