1. Warm-up 50 grams of H2O 100 grams of CaCO3 150 grams of NaOH
Convert the following to moles (start by drawing the mole hill):
50 grams of H2O
100 grams of CaCO3
150 grams of NaOH

2. Stoichiometry: Mol-Mol Ratios
Unit Seven, Day One

3. What is stoichiometry?
Stoichiometry is the study of the quantitative relationships in reactions.
The coefficients in a reaction correspond to how many moles of each substance is needed for the reaction to occur.
Use mole ratios (the coefficients) to convert between one substance to another in a BALANCED equation.

4. Using the mole ratio N2 + H2  NH3 Balance the equation!!!
3 moles of H2 = ? moles of NH3

5. Why do we need the mol-mol ratio?
We’re going to use the mol-mol ratio to convert between different substances in our formula
N2 + 3H2  2NH3

6. Steps for stoichiometry
Balance the equation
Determine the mol-mol ratio
Convert to moles (if you don’t have moles)
Use, and only use, the mole ratio to convert between substances.

7. How many moles??
N2 + 3H2  2NH3
15 moles of N2 = x moles of NH3

8. N2 + 3H2  2NH3
30 moles of H2 = x moles of NH3

9. Example Mol-mol Al + HCl  AlCl3 + H2
Using the above reaction. How many moles of aluminum do I need to produce 6.75 moles of Hydrogen?