Honors Chemistry
Define the following:
1. Stoichiometry
Chapter 9
Chemical Quantities: Stoichiometry
Test Review
2. Limiting Reactant
3. Theoretical Yield
4. Excess Reactant
5. Actual Yield
6. Percent Yield
7. What do the coefficients in a balanced equation tell you?
8. When NaCl is prepared from 37 g of Na, and an excess of Cl2, the theoretical yield of NaCl is 94.0 g.
When this reaction is carried out in an experiment, only 90.0 g are actually produced.
What is the percentage yield?
9. For the reaction:
2 Cl2 + 4 NaOH Æ 3 NaCl + NaClO2 + 2 H2O
12.3 g C12 is reacted with 12.0 g of NaOH. Determine which is the limiting reactant?
10. Consider the reaction:
2 Mg + O2 Æ 2MgO
Which of the reactants is in excess if we start with 25.0 g of each reactant?
11. If 4.0 moles of H2 are used up in the following balanced reaction, how many moles of H2O will be
2H2 + O2 Æ 2H2O
12. If 10.0 g of hydrogen react with excess oxygen and 86.0g of water are produced, what is the
percent yield?
2H2 + O2 Æ 2H2O
13. If 5.03 moles of ZnS are combined with 6.00 moles of O2 how many moles of ZnO can be
2 ZnS + 3 O2 Æ 2 ZnO + 2S O2
14. How many moles of water are produced when 2.03 mol of CH4 undergoes complete combustion?
2 CH4(l) + 3 O2(g) Æ 2 CO2(g) + 2 H2O(l)