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#### Presentation Transcript

**1. **Stoichiometry Chapter 11

**2. **So Far, we have Learned to convert
Mass Mole
Mole Mass
Particle Mole
Mole Particle
Mass Particle
Particle Mass
Mole Volume
Volume- Mole
And More

**3. **Chemistry Learning Objective Student should be able to perform the following types of stoichiometric calculations using balanced chemical equations:
mole-mole
mass-mass
mass-volume
volume-volume

**4. **Stoichiometric Definition The study of the quantitative, or measurable, relationships that exist in chemical formulas & chemical reactions

**5. **Interpreting Balanced Chemical Equations NH4NO3 ? N2O + 2 H2O
The coefficients represent any of the following:
Moles 1 mole NH4NO3 decomposes to produce 1 mole N2O and 2 moles H2O
# particles
Molecules/Atoms
Volume if gas at STP

**6. **Mole Mole Problems NH4NO3 ? N2O + 2 H2O
How many moles of H2O are produced if 3.65 moles of NH4NO3 are decomposed?

**7. **N2 + H2 ? NH3 If 4.0 moles of H2 react, how many moles of NH3 will be produced?
Step 1: Balance the Equation
Step 2: Determine mole ratio of H2 to NH3
Step 3: Set up equation
N2 + 3H2 ? 2NH3

**8. **KClO3 ? KCl + O2 What mass of KClO3 do you need to produce 0.50 mol of O2
Step 1: Balance Equation
Step 2: Determine Mole ratio
Step 3: Set up equation (always start with what you are given and set up conversions from that!)

**9. **END OF PART I

**10. **WARM Ups FOR TODAY 1. Phosphorus will react with bromine to produce phosphorus tribromide. How many moles of Phosphorus tribromide will be produced if 0.78 mol of bromine is reacted?
A. Write a balanced equation.
B. Set up the problem like we have been in class.
C. Solve
What mass of Sodium Chloride is produced when chlorine reacts with 0.29 g of sodium iodide?
A. Write a balanced equation.
B. Set up the problem like we have been in class.
C. Solve

**11. **Warm up 1

**12. **Solving Stoichiometric Problems other types
Mass mass
Mass volume
Volume volume

**14. **Remember Moles to Liters??? at STP, 1 mole of a gas = 22.4L
How many liters are present in 10g of H2 at STP?

**15. **Mass Volume problems:

**16. **If an airbag contains 125 g sodium azide, NaN3, what volume of nitrogen gas is produced at STP? (0oC & 1 atm) 2NaN3 ? 2Na + 3N2

**17. **Volume Volume Problems If a mole of any gas occupies the same volume as any other gas at STP (22.4L) then mole ratios are also volume ratios at STP

**18. **Volume Volume Problems

**19. **Summary Stoichiometry is the math of chemical reactions
Mole ratios from chemical equations allow us to convert between amounts of substances in chemical reactions.
MUST use balanced chemical equation in calculations

**20. **Summary (YES WRITE THESE) Mole ratios are HEART of all conversion problems and can be used to:
Mole to mole
Mass to mole
Mass to mass
Mass to volume
Volume to volume