2.  How far away you are from a theoretical or “actual” value.

3.  Stoichiometry tells us the theoretical yield of a chemical reaction.  The actual yield of a chemical reaction is usually less. ◦ Incomplete reactions ◦ Impure reactants ◦ Side reactions occurring ◦ Reversible reactions

5.  If 5.50g of hydrogen reacts with nitrogen to form 20.4g of ammonia, what is the percent yield? N 2 (g) + H 2 (g)  NH 3 (g) 32

6. 31.2g NH 3 (Theoretical)

7. 65.4% NH 3

8.  Actual yield: What you actually get. ◦ Results from lab  Theoretical Yield: What you should get. ◦ Need to use stoichiometry.  Actual Yield is always a product. ◦ Yield(ing)  product forms