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2. Stoichiometry: Introduction At the conclusion of our time together, you should be able to: 1.Explain what stoichiometry is 2.Define what a mole is 3.Describe how the mole was discovered 4.Convert a mole of a chemical into its molar mass

3. Stoichiometry: Conversions At the conclusion of our time together, you should be able to: 1. Convert a mole of a chemical to particles or grams of that chemical 2. Convert grams of a chemical to moles or particles 3. Convert particles of a chemical to moles or grams

4. STOICHIOMETRYSTOICHIOMETRY - the study of the quantitative aspects of chemical reactions.

5. The Mole is the Quantity We Use in Stoichiometry 6.02 X 10 23

6. The Mole A counting unit Similar to a dozen, except instead of 12, it’s 602 billion trillion 602,000,000,000,000,000,000,000 6.02 X 10 23 (in scientific notation) Amedeo Avogadro (1776 – 1856) This number is named in honor of Amedeo Avogadro (1776 – 1856), who studied quantities of gases and discovered that no matter what the gas was, there were the same number of molecules present

7. Everybody Has Avogadro’s Number! But Where Did it Come From? It was NOT just picked! It was MEASURED. One of the better methods of measuring this number was the Millikan Oil Drop Experiment Since then we have found even better ways of measuring using x-ray technology

8. Just How Big is a Mole? Enough soft drink cans to cover the surface of the earth to a depth of over 200 miles. If you had Avogadro's number of unpopped popcorn kernels, and spread them across the United States of America, the country would be covered in popcorn to a depth of over 9 miles. If we were able to count atoms at the rate of 10 million per second, it would take about 2 billion years to count the atoms in one mole.

9. A Mole of Particles Contains 6.02 x 10 23 Particles = 6.02 x 10 23 C atoms = 6.02 x 10 23 H 2 O molecules = 6.02 x 10 23 NaCl “formula units” 6.02 x 10 23 Na + ions and 6.02 x 10 23 Cl – ions 1 mole C 1 mole H 2 O 1 mole NaCl

10. H H 1.008 1 Avogadro asked... Q: If ONE Hydrogen atom masses at 1.008 amu’s, how many Hydrogen atoms would it take to mass at 1.008 grams ?

11. Answer: 6.023 x 10 23  that many 602,300,000,000,000,000,000,000

12. Na 22.990 11 Q: If ONE Sodium atom masses at 22.99 amu, how many Sodium atoms would it take to mass at 22.99 grams ?

13. Molar Mass of Molecules and Compounds Mass in grams of 1 mole is equal numerically to the sum of the atomic masses 1 mole of NaCl = 1 mole Na x + 1 mole1 Cl x

14. Calculations with Molar Mass molar mass Grams Moles

15. Molar Mass as a Conversion Factor Molar Mass of the Compound 1 mole or 1 mole Molar Mass of the Compound Note that the molar mass could be that of an atom OR a molecule!

16. Example of Converting Moles to Grams Aluminum is often used for the structure of light-weight bicycle frames. How many grams of Al are in 3.00 moles of Al? 3.00 moles Al ? g Al

17. 1. Molar mass of Al1 mole Al = 26.98 g Al 2. Conversion factors for Al 26.98 g Al or 1 mol Al 1 mol Al 26.98 g Al 3. Setup3.00 moles Al x 26.98 g Al 1 mole Al Answer = 80.94 g Al

18. Learning Check! The artificial sweetener aspartame (Nutra-Sweet) formula C 14 H 18 N 2 O 5 is used to sweeten diet foods, coffee and soft drinks. How many moles of aspartame are present in 225 g of aspartame? = 0.764 mol