1. REVIEW

2. Know Your Terms Excess reactant Actual yield Limiting reactant
Percent yield
Theoretical yield
Law of conservation of mass
Mole ratio
Stoichiometry

3. 6K + B2O2 → 3K2O + 2B Particles = Moles = Mass =
Law of conservation of mass =

4. _____Mg + _____O2 → _____MgO
Particles =
Moles =
Mass =
Law of conservation of mass =

5. The ___________ the % yield, the more efficient the reaction is

6. _____________ are added when balancing chemical equations

7. ______________ are added when writing out chemical equations

8. To convert mass to moles, ______________ by molar mass

9. In the equation C3H8 + 5O2 → 3CO2 + 4H2O, how many mole ratios can be written?
a c
b d. 16

10. If you were given the equation 2Mg + O2 → 2MgO, which mole ratio would you use to find the moles of MgO produced if you know O2?
a. 2MgO/O2 c. 2Mg/2MgO
b. 2Mg/O2 d. O2/2Mgo

11. To convert 35 g of C to moles of C, you would need to…
a. Multiply by molar mass
b. Multiply by correct mole ratio
c. Divide by molar mass
d. Divide by correct mole ratio

12. One mole of (NH4)2Cr2O7 contains:
a. One mole of Nitrogen
b. seven moles of Oxygen
c. One mole of Chromium
d. four moles of Hydrogen

13. To convert 52 moles of Boron to grams of Boron, you would need to…
a. Divide by molar mass
b. multiply by correct mole ratio
c. Multiply by molar mass
d. divide by correct mole ratio

14. In the equation 2Mg + O2 → 2MgO, how many moles of magnesium oxide will be produced for each mole of oxygen?
a c
b d

15. The numbers in mole ratios are found using …
The subscripts
Avogadro’s number
The molar mass of the elements
The coefficients

16. If an equation contains 5 substances, how many mole ratios can be written?
a c
b d

17. 3Fe + 4H2O → Fe3O4 + 4H2
# of mole ratios = ___________

18. 2AgNO₃ + K₂CrO₄ = Ag₂CrO₄ +2KNO₃
If you have g of silver nitrate (AgNO₃), determine the theoretical yield of Ag₂CrO₄.

19. 2AgNO₃ + K₂CrO₄ = Ag₂CrO₄ +2KNO₃
If the experiment is performed and the actual yield is g Ag₂CrO₄, what is the percent yield?

20. The reaction between sodium and iron(III) oxide is one in a series of reactions that inflates an airbag: 6 Na Fe2O3 → 3 Na2O Fe If 80.0 g of Na and g of Fe2O3 are used in this reaction, determine the following:
Limiting reactant =
Reactant in excess =
Mass of solid iron produced =
Mass of excess reactant that remains after the reaction is complete =