1. Limiting Reactants

2. Limiting Reactant – limits the extent of the reaction
Excess Reactant – left-over reactants
For example:
For your birthday, you are given 10 bicycle frames and 15 wheels/tires
How many bicycles can be made?
What is the “limiting reactant”?
What is the “excess reactant”

3. 6Na + Fe2O3  3Na2O + 2Fe
If 100.0g sodium and 100.0g iron(III) oxide are used in this reaction, determine:
a. the limiting reactant

4. 6Na + Fe2O3  3Na2O + 2Fe
If 100.0g sodium and 100.0g iron(III) oxide are used in this reaction, determine:
b. the reactant in excess

5. 6Na + Fe2O3  3Na2O + 2Fe
If 100.0g sodium and 100.0g iron(III) oxide are used in this reaction, determine:
c. the mass of the solid iron

6. 6Na + Fe2O3  3Na2O + 2Fe
If 100.0g sodium and 100.0g iron(III) oxide are used in this reaction, determine:
d. the mass of the excess reactant that remains after the reaction is complete