1. Drill – 2/28/11
Sodium chloride decomposes into sodium and chlorine. How much (in grams) sodium chloride is required to produce 50.0g of chlorine gas?

2. Limiting Reagents

3. Example
Your job is to attach arms on dolls in a doll factory. If you have 600 arms and 350 dolls, how many finished dolls can you make?
What is limiting your production – the arms or the dolls?
What do you have
in excess?

4. Reagent –reactant in a chem reaction
Limiting Reagent – the reactant that is completely consumed. This reactant limits the amount of product that is formed.
Excess Reagent – the reactant that is not limiting the reaction. There will be leftovers of this reactant.

5. How to solve for limiting reagent
Write the balanced chemical equation
Determine the moles of each reactant
Determine how many moles of product each reactant would make using a mole ratio
The reactant that yields less product is the limiting reagent.

6. Copper reacts with sulfur to form copper (I) sulfide
Copper reacts with sulfur to form copper (I) sulfide. What is the limiting reagent when 80.0g Cu reacts with 25.0g S?
Write the balanced chemical equation 2 Cu + S 
Cu2S

7. Copper reacts with sulfur to form copper (I) sulfide
Copper reacts with sulfur to form copper (I) sulfide. What is the limiting reagent when 80.0g Cu reacts with 25.0g S?
2. Determine the moles of each reactant.
1 mole Cu
80.0 g Cu x
= 1.26 mol Cu
63.55 g Cu
1 mole S
25.0 g S x
= .780 mol S
32.06 g S

8. Copper reacts with sulfur to form copper (I) sulfide
Copper reacts with sulfur to form copper (I) sulfide. What is the limiting reagent when 80.0g Cu reacts with 25.0g S?
3. Determine how many moles of product each reactant would make using a mole ratio
1 mol Cu2S
1.26 mol Cu x
= .630 mol Cu2S
2 mol Cu
1 mol Cu2S
.780 mol S x
= .780 mol Cu2S
1 mol S

9. So Copper is the limiting reagent
Copper reacts with sulfur to form copper (I) sulfide. What is the limiting reagent when 80.0g Cu reacts with 25.0g S?
4. The reactant that yields less product is the limiting reagent.
Copper yields .630 mol Cu2S
Sulfur yields .780 mol Cu2S
So Copper is the limiting reagent

10. What is the excess reagent?
How many moles of Cu2S will be produced?

11. Amount of Excess?
In order to determine how much (mass) of excess reagents there are, you must figure out what mass of the excess reagent got used up…then subtract that from the initial mass.

12. Amount of Excess?
Step 1 – Start with moles of product formed (from limiting reagent).
Step 2 – Convert back to moles of excess reagent.
Step 3 – Convert from moles to mass of excess reagent.
Step 4 – Subtract this value from the original mass of excess reagent (given in problem)

13. Hydrogen fluoride reacts with aluminum oxide to produce aluminum fluoride and water.
If 60.0g of hydrogen fluoride react with 25.0g of aluminum oxide, how many grams of aluminum fluoride will be produced?
Determine the mass of excess reactant remaining.

14. Drill – 3/1/11
If 5.0g of hydrogen react with 9.0g of oxygen, what mass of water will be produced?