1. WARM UP
Write oxidation and reduction half-reactions for the reaction: 2 H2 + O2  2 H2O.
Write a net ionic equation for the reaction Pb(NO3)2 + 2NaI  PbI2 + 2NaNO3.

2. Stoichiometry
Chemistry II

3. Stoichiometry Quantitative study of chemical reactions
Number measurements
Moles, grams, etc.

4. Yield Product made from reactant Mole method Use balanced coefficients
Ex: 2 CO (g) + O2(g)  2 CO2(g)
2 moles CO will yield 2 moles CO2
2 moles O2 will yield 4 moles CO2

5. Limiting and Excess Reagents
Limiting reagent
Used up first, limits/determines yield
Mole method
Find moles of product formed from each reactant
Reactant that gives lesser yield is limiting

6. Limiting and Excess Reagent
Not used up, extra left over
Mole method
Amount of limiting reagent used
Convert to excess reagent needed
Subtract from given amount of excess reagent

7. WRAP UP
Given the equation below, if you mix 17 moles of H2 and 13 moles of O2, how many moles of water will you make? What will be your limiting and excess reagents? How much excess reagent will you have left over?