1. Chapter 11 Review

2. Define the following: Stoichiometry Mole ratio
Excess reactant
Limiting reactant
Theoretical yield
Actual yield
Percent yield
You can find all the definitions in the book. Look them up and
STUDY!!!!

3. Find the following molar masses:
O2 : 16 x 2 = 32 g/mol
O : g/mol
AlPO4 : ( x 3) = g/mol
NaCl : = g/mol
C6H5Cl : ( x 6) + ( x 5) = g/mol
CuO : = g/mol

4. Determine the number of steps for the following problems (1, 2, or 3):
Given the following equation: 2 KClO3 –> 2 KCl + 3 O2
How many moles of O2 can be produced by letting moles of KClO3 react? 1 step
How many grams of O2 can be produced by letting 34.7g of KClO3 react? 3 steps
How many moles of O2 can be produced by letting 14.6g of KClO3 react? 2 steps

5. Create the following mole ratios:
_4_Ag(s) + _2_H2S(g) + _1_O2(g) _2_Ag2S(s) + _2_H2O(l) (Equation must first be balanced.)
Ag : H2S 4:2 = 2:1
O2 : Ag2S 1: 2
Ag2S : H2O 2:2 = 1:1
O2 : H2S 1:2
Ag : O :1
H2O : H2S 2:2 = 1:1
How many ratios can this equation form?

6. What is the molar ratio of all elements/compounds shown?
2 : 3 : 2

7. Solve the following:
Given the following equation: 2 KClO3 –> 2 KCl + 3 O2
How many moles of O2 can be produced by letting moles of KClO3 react?

8. Solve the following:
Given the following equation: 2 KClO3 –> 2 KCl + 3 O2
How many grams of O2 can be produced by letting 34.7g of KClO3 react?

9. Solve the following:
Given the following equation: 2 KClO3 –> 2 KCl + 3 O2
How many moles of O2 can be produced by letting 14.6g of KClO3 react?

10. Solve the following:
Given the following equation: Al2(SO3)3 +  6 NaOH  3 Na2SO3  +  2 Al(OH)3
If 10.0 g of Al2(SO3)3 is reacted with 10.0 g of NaOH to form Na2SO, determine the limiting reactant

11. Solve the following:
Given the following equation: 2 FePO4 + 3 Na2SO4  1 Fe2(SO4)3 + 2 Na3PO4
What is the percent yield of this reaction if takes place with 25g of FePO4 and an excess of Na2SO4, and produces 18.5g of Fe2(SO4)3