1. WARM UP
4 Li + O2  2 Li2O
If you have 804 g of Li available for the reaction, calculate the amount of O2 you will need to pump into the reaction to ensure that all the Li reacts.

2. Limiting vs. Excess

3. Limiting Reagents

4. Limiting vs. Excess Limiting reagent
The first reactant used up in a reaction
After it’s gone, no more product formed

5. Limiting vs. Excess Excess reagent
Not used up in a reaction, extra left over

6. Limiting vs. Excess

7. Calculating Limiting Reagent
Ex:
Write balanced equation
Calculate yield (in grams) from each reactant
Less product = limiting reagent
More product = excess reagent

8. Calculating Yield Theoretical yield is determined by limiting reagent
Lesser amount of product

9. WRAP UP H3PO4 + 3 KOH  K3PO4 + 3 H2O
Given 5.0 moles of KOH and 2.0 moles of H3PO4, how many moles of K3PO4 can be prepared?
Which reactant is the limiting reagent? Which is the excess?

10. WARM UP
2 Al + Fe2O3  2 Fe + Al2O3
If you reacted 24 grams of aluminum with 190 grams of Fe2O3 and obtained .28 moles of Al2O3…
What is your limiting reagent? Excess reagent? Percent yield?

11. WRAP UP
SO2 + CaO  CaSO3
If 975 g of SO2 is to be removed by the reaction, what mass of CaO will be required to completely react the SO2 and make it the limiting reagent?

12. WARM UP
Take out your Production of Salt lab report with a Question, Hypothesis, and Procedure.

13. WARM UP Measure your beaker with the dry salt.
Clean up you lab station.
Begin your calculations at your desk.