Name:

1. Compare the limiting reactant and the excess reactant in a chemical reaction.
   

2. Compare the actual yield to the theoretical yield.
   

3. Why is it necessary to balance a chemical reaction in order to do stoichiometry calculations?
   

4. Use the balanced chemical equation below to show mole ratios for the situations that follow.

                            2H₂(g)  +  O₂(g)  --> 2H₂O(g)

    a. mol of H₂O produced from 2 mol of H₂
    b. mol of O₂ required if 2 mol H₂O are produced
    c. mol of H₂ required if 1 mol of O₂ reacts

5. Describe the relationship between the limiting reactant and the theoretical yield.
   

6. In the reaction below, 64 grams of CaC₂ react with 64 grams of H₂O.

            CaC₂  +  2H₂O  --> C₂H₂  +  Ca(OH)₂

    a. Which is the excess reactant?
    b. Which is the limiting reactant?
    c. How many grams of Ca(OH)2 are produced?

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