1. Chapter 12 Review

2. In a chemical reaction………
Mass is conserved
Atoms are conserved
Moles are conserved
Both mass and atoms are conserved

3. Which of the following is a correct interpretation of this balanced equation? 2Al + 3Pb(NO3) Al(NO3)3 + 3Pb
2 atoms Al + 3 molecules Pb(NO3)2 makes 2 molecules Al(NO3)3 + 3 atoms Pb
2 grams Al + 3 grams Pb(NO3)2 makes 2 grams Al(NO3)3 + 3 grams Pb
2 moles Al + 3 moles Pb(NO3)2 makes 2 moles Al(NO3)3 + 3 moles Pb
Both a and c

4. If 3.00 mole CaCO3 decomposes to form CaO and CO2, how many grams of CO2 are produced?

5. If 18 grams of carbon reacts with Oxygen to produce carbon dioxide, how many molecules of oxygen would be required?
1.5 molecules
48 molecules
9.0 x 1023 molecules
3.2 x 1024 molecules

6. Given the reaction 2NO + O2 2NO2, if 6
Given the reaction 2NO + O2 2NO2, if 6.5 L O2 reacts at STP, how many liters of NO2 are produced?
6.5 L
3.2 L
13 L
26 L

7. Given the reaction of a single replacement with Zinc and Hydrochloric acid, if 2.0 mol of Zn and 5.0 mol of HCl are allowed to react ….
Zn is limiting
HCl is limiting
1.0 mole of ZnCl2 is produced
5.0 mole H2 is produced

8. Given the reaction CaCO3 CaO + CO2, if 50
Given the reaction CaCO CaO + CO2, if 50.0g of CaCO3 reacts to produce 20.0 g of CO2, what is the percent yield of CO2?
66.7 %
40.0 %
90.9 %
250 %

9. The substance that determines the amount of product is formed is the _______________.
Actual yield
Excess reactant
Limiting reactant
Percent yield

10. The calculations of quantities in chemical reactions is _____________________.
Stoichiometry
Mole ratios
Theoretical yield
Limiting reactant

11. How many liters of oxygen are required to react completely with 1
How many liters of oxygen are required to react completely with 1.2 liters of hydrogen to form water. 2H O2 2H2O
1.2 L
0.6 L
2.4 L
4.8 L

12. Things to know!
Mass – Mass calculations Quantity – Quantity calculations Percent yield (actual and theoretical) Definitions