1. Chapter 9 Stoichiometry part I
Mole-mole problems
Mass-mass problems

2. Stoichiometry Calculations of quantities in chemical reactions
This means using balanced equations to calculate quantities of chemicals used in a chemical reaction

3. A chemical equation is like a recipe; it shows you how much of each “ingredient” is used and how much product you will have in the end.

4. N2 + 3H2 a 2NH3 How many molecules of N2 are there?
How many molecules of H2 are there?
How many molecules of NH3 are there?
So one molecule of N2 will react with 3 molecules of H2 to form 2 molecules of NH3.
You could also say that one mole of N2 will react with 3 moles of H2 to form 2 moles of NH3.

5. The heart of stoichiometry is using a balanced chemical equation as a conversion factor for dimensional analysis.

6. Zn + HCl a ZnCl2 + H2
For the above reaction, how many moles of zinc chloride can be produced with 0.27 moles of zinc?
For the above reaction, how many moles of zinc will react with 1.39 moles of hydrochloric acid?

7. Na + H2O a NaOH + H2 As an experiment...
What is the ratio of the reaction of adding sodium to water, producing sodium hydroxide and hydrogen gas?
Na + H2O a NaOH + H2

8. So if we started with 0.15 moles of sodium metal, how many moles of hydrogen gas was produced?

9. Why are mole/mole problems impractical in a laboratory setting?

10. If you have 2.7 grams of sodium to begin with, how many liters of hydrogen gas can be produced?

11. Fe + O2 a Fe2O3
How many grams of iron (III) oxide can be produced with 17.2g Fe?
How many grams of iron will react with 5.25 liters of O2
How many molecules of O2 are needed to produce 3.92g Fe2O3?