1. Chapter 11 and supplemental Ms. Lockhart Chemistry
Stoichiometry
Chapter 11 and supplemental
Ms. Lockhart
Chemistry

2. Stoichiometry Importance
By understanding the mole we can use the information to
Predict mass or volume of a product.
Predict how much reactant is needed for a reaction.
Make substances of all kinds like
Your sneakers
Glue
Your clothes
Gum
Candy
Petrochemicals (oils, vaseline, gas)

3. Other uses % by mass (% composition) Empirical Formula
Formula of a Hydrate
Stoichiometric calculations
Limiting Reagent
% yield

4. Stoichiometry
You can interpret a lot from a balanced chemical reaction.
Iron is added to oxygen gas (O2) to yield iron (III) oxide (ferric oxide).
4 Fe O2  2Fe2O3
Atoms
Moles
Mass
Total mass

5. Stoichiometry
Nitrogen gas (N2) is added to hydrogen gas (H2) to make ammonia (NH3).
N H2  NH3
Atoms
Moles
Mass
Total mass

6. Practice Stoichiometry
3.00 g Magnesium (Mg) is heated with excess oxygen gas (O2) to make magnesium oxide.
2 Mg O2  MgO

7. Steps to Stoichiometry
Copy the word equation (write the chemical reaction in words).
Write the word equation into a formula equation.
Balance the chemical reaction.
2 Mg O2  MgO

8. Steps to Stoichiometry
Write given information under the balanced chemical reaction
2 Mg O2  MgO
3.00 g

9. Steps to Stoichiometry
Write what you are looking for.
2 Mg O2  MgO
3.00 g ? O2

10. Steps to Stoichiometry
Convert given information into moles.
2 Mg O2  MgO
3.00 g ? O2
3.00 g Mg x 2 moles Mg = 3x2/24.31 = moles Mg
24.31 g Mg

11. Steps to Stoichiometry
Use mole ratio to get moles to the correct representative particles.
2 Mg O2  MgO
3.00 g ? O2
0.247 moles
0.247 moles Mg x 1 mole O2 = 0.247x1/2 = moles O2
2 moles Mg

12. Steps to Stoichiometry
Convert mole to grams, particles or whatever the answer ask for.
Calculate and write the answer.
2 Mg O2  MgO
3.00 g ? O2
0.247 moles moles
0.124 moles O2 x 32 g O2 = 0.124x32/1 = 3.97 g O2
1 moles O2

13. Practice Stoichiometry
Correct significant figures (sig figs) and rewrite the answer.
3.00 g Mg = 3 S.F.
S.F. Answer: 3.97 g O2

14. Let’s Take It Slow…