1. 14.6 – NOTES Limiting Reactants

2. B.10 Incomplete combustion Based on limiting reactants
You can only make as much as your least reactant
Cars and car tires: How many complete cars can you make?

3. Attempt to solve the next three problems!
B.10 Incomplete combustion
Sometimes in reactions, products other than the desired ones form
Stoichiometry
In order to solve these problems, you must have a balanced equation. The balanced equation provides the mole ratio, which is the moles of what you are looking for in the problem, over the moles of what you were initially given information about
Attempt to solve the next three problems!

4. Use the equation 2 KClO3 ---> 2 KCl + 3 O2 for the next few examples
You are given 4.5 moles of KClO3. How many moles of O2 can you make?
6.75 mol of O2

5. Use the equation 2 KClO3 ---> 2 KCl + 3 O2 for the next few examples
You make 2.3 grams of KCl. How many moles of KClO3 did you start with?
0.03 mol of 2 KClO3

6. Use the equation 2 KClO3 ---> 2 KCl + 3 O2 for the next few examples
You are given 43 grams of KClO3. How many grams of KCl can you make?
35.9 g KCl

7. Based on limiting reactants
Examples: a. If 5.0 grams of nickel and 5.0 grams of chlorine gas are reacted completely, how many grams of product could be formed, theoretically?
Ni + Cl2  NiCl2 Given: 5.0 g Ni ( = 58.7g/mol)
5.0 g Cl2 ( =71.0g/mol)
Find: g NiCl2 ( = 129.7g/mol)

8. If Ni is the limiting reactant….
5.0g Ni x 1 mol Ni x 1 mol NiCl2 x g NiCl2
58.7g Ni mol Ni 1 mol NiCl2 = 11g NiCl2
If Cl2 is the limiting reactant….
5.0g Cl2 x 1 mol Cl2 x 1 mol NiCl2 x g NiCl2
71.0 g Cl mol Cl mol NiCl2 = 9.1g NiCl2

9. b. If you react 13. 5 grams of HCl with 14
b. If you react 13.5 grams of HCl with 14.8 grams of FeS, how many grams of H2S could be produced?
2HCl + FeS  H2S + FeCl2 Given: 13.5g HCl (= 36.5g/mol)
14.8g FeS (=87.9g/mol)
Find: g H2S (= 33.1g/mol)

10. If HCl is the limiting reactant……
13.5g HCl x 1 mol HCl x 1 mol H2S x g H2S
36.5g HCl mol HCl mol H2S = 6.12g H2S
If FeS is the limiting reactant……
14.8g FeS x 1 mol FeS x 1 mol H2S x g H2S
87.9g FeS mol FeS mol H2S = 5.57g H2S