1. Stoichiometry Calculating Reactants and Products

2. Stoichiometry Defined The calculation of quantities in chemical reactions The use of balanced equations to determine numbers of reactants and products used and needed

3. Another Way To Look at It Just like a recipe is needed to bake cookies, these balanced equations act as the recipe What if you need to triple or quadruple the recipe? You need to recalculate your ingredients

4. Why is this important? Nearly everything we use is made of chemicals. Chemicals that need to be mixed in exact quantities Soap, medicine, make-up, clothes, shampoos, fertilizers, and so on

5. How it Works You’ll be given a balanced equation Next you will be asked to determine the amount of reactants needed to yield so much product Or You may be asked to determine how much product will be yielded if so much of a reactant is added

6. Example Given the following equation: 2 KClO 3  2 KCl + 3 O 2 1. How many moles of O 2 can be produced by letting 12.00 moles of KClO 3 react?

7. How to Solve 1 st and always 1 st use the following conversion guide Units given  moles of given  moles of needed  units needed

8. Units given  moles

9. Example 2 2 K + Cl 2  2 KCl How many grams of KCl are produced from 2.50 g of K and excess Cl 2 Also from 1.00 g of Cl 2 and excess K

10. Solve Grams to moles  moles to moles  moles to grams

11. Answer

14. Practice problem 1 st balance the following Na 2 O + H 2 O  NaOH Next answer the following 1.How many grams of water are needed to produce 20 grams of product 2.How many molecules of product will be produced from 50 grams of Na 2 O

15. The Many Possible Conversions Grams to grams Grams to moles Moles to moles Moles to grams Liters to moles or grams or liters Grams to molecules Molecules to all the above

16. Homework You will have 1 example problem to work and specific instructions on what to do with that answer on e- companion tonight Remember mhsfirst.last first

17. Gases and the Mole At equal temperatures and equal pressures, equal volumes of gases contain the same number of molecules

18. STP Standard temperature and pressure The values for gasses at STP are as follows –Temp. is 0 o C –Pressure is 1 atm (atmosphere)

19. IdeaL Gas Law PV = nRT –P is pressure (101.3 kPa) –V is volume (?) –n is number of moles (1) –R is called the ideal gas constant (8.31) –T is temperature (273 K)

20. Find V V = nRT/P V=(1)(8.31)(273)/101.3 V= 22.4

21. What’s this tell us? 1 mole of ANY gas at STP is equal to a volume of 22.4 liters

22. Example 2SO 2 (g) + O 2 (g)  2SO 3 (g) Assuming STP, how many liters of oxygen are needed to produce 19.8L SO 3