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the Mole !

It’s time to learn about . . . the Mole !. My new book on GOLF will give the reader valuable playing tips and insider information I've gained through my years of lessons, struggles and experiments. Here are just a few of the chapter titles: .

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the Mole !

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  1. It’s time to learn about . . . the Mole !

  2. My new book on GOLF will give the reader valuable playing tips and insider information I've gained through my years of lessons, struggles and experiments. Here are just a few of the chapter titles:  Chapter 2 - How to Hit a Nike from the Rough, when you Hit a Titleist from the Tee. Chapter 18 - When to Regrip Your Ball Retriever.

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

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

  5. STOICHIOMETRY • Composition Stoichiometry • Reaction Stoichiometry • Molar Ratio

  6. The Mole is the Quantity We Use in Stoichiometry 6.02 X 1023

  7. 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 1023 (in scientific notation) • 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

  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. 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

  10. Here’s Another Way of Looking at the Mole… Suppose we invented a new collection unit called a toburen. One toburen contains 8 objects. 1. How many paper clips in 1 toburen? a) 1 b) 4 c) 8 2. How many oranges in 2.0 toburens? a) 4.0 b) 8.0 c) 16 3. How many toburens contain 40 gummy bears? a) 5 b) 10 c) 20

  11. 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 ? 1 H 1.008

  12. Answer: 6.023 x 1023 that many 602,300,000,000,000,000,000,000 one Mole

  13. The Mole is just Another Counting Unit • 1 dozen cookies = 12 cookies • 1 mole of cookies = 6.02 X 1023 cookies • 1 dozen cars = 12 cars • 1 mole of cars = 6.02 X 1023 cars • 1 dozen Al atoms = 12 Al atoms • 1 mole of Al atoms = 6.02 X 1023 atoms Note that the mole NUMBER is always the same, but the mole MASS is very different! Mole is abbreviated mol (gee, that’s a lot quicker to write, huh?)

  14. Septic Tank Humor

  15. A Mole of ParticlesContains 6.02 x 1023 Particles = 6.02 x 1023 C atoms = 6.02 x 1023H2O molecules = 6.02 x 1023NaCl “formula units” 6.02 x 1023 Na+ ions and 6.02 x 1023Cl– ions 1 mole C 1 mole H2O 1 mole NaCl

  16. Hittite Innovations:

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

  18. What does one Mole ofLithiumatoms mass at? What does one Mole ofCarbonatoms mass at? What does one Mole ofO2molecules mass at? What does one Mole ofWatermolecules mass at?

  19. Molar Mass • The Mass of 1 mole (in grams) • Equal to the numerical value of the average atomic mass (use your periodic table, round to 2 places) 1 mole of C atoms = 12.01 g 1 mole of Mg atoms = 24.31 g 1 mole of Cu atoms = 63.55 g

  20. Other Names Related to Molar Mass Molecular Mass: If you have a single molecule, mass is measured in amu’s instead of grams. The molecular mass is the same numerical value as 1 mole of molecules, only the units are different - grams and not amu’s. (This is the beauty of Avogadro’s Number!) Formula Mass: Same goes for ionic compounds. But again, the numerical value is the same, only the units are different.

  21. 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 CaCl2 = 1 mole Ca x 40.08 g/mol + 2 moles Cl x 35.45 g/mol = 110.98 g/mol CaCl2 1 mole of N2O4 = 92.02 g/mol N2O4

  22. I wonder if he ducked fast enough??

  23. Stoichiometry: IntroductionLet’s see if you can: Explain what stoichiometry is Define what a mole is Describe how the mole was discovered Convert a mole of a chemical into its molar mass

  24. What Is The Difference Between a Harley And a Hoover? The Location Of The Dirt Bag.

  25. STOICHIOMETRY - the study of the quantitative aspects of chemical reactions.

  26. The Mole is the Quantity We Use in Stoichiometry 6.02 X 1023

  27. 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 1023 (in scientific notation) 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

  28. Learning Check! Find the mole (molar) mass (round to the hundredths place) • 1 mole of Br atoms • 1 mole of Sn atoms = 79.90 g/mole = 118.71 g/mole

  29. Learning Check! • Molar Mass of K2O = ? g/mol 94.20 g/mol • MolarMass of antacid Al(OH)3 = ? g/mol 78.01 g/mol

  30. Learning Check! Help Mr. T!! • Molar Mass of chalk (calcium carbonate) = ? g/mol 100.09 g/mol

  31. The End!!

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