Stoichiometry Chapter 11

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So Far, we have. Learned to convertMass ? MoleMole ? MassParticle ? MoleMole ? ParticleMass ? ParticleParticle ? MassMole ? VolumeVolume- MoleAnd More?????. Empirical Formula and Molecular Formula. Chemistry Learning Objective. Student should be able to perform the following types of stoich

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Stoichiometry Chapter 11

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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

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