1. Moles and Molar Mass A number to remember!

2. Avogadro and his Number

3. 6.022 x 10 23 Currently best sig. fig.= 6.02214129(27)×10 23 Avogadro’s Number, Now officially, Avogadro’s Constant – since it’s a unit

4. What??? It’s the ratio of the mass of a single Proton to a gram! It is the number of Carbon atoms in 12.011 grams of Carbon

5. Molar Mass The Mass of a Mole of Atoms H – 1.00794- 1 C – 12.011- 12 N – 14.00674- 14 O – 15.9994- 16

6. OK, What’s the Molar Mass of: H 2 O 2 H 2 O CH 4 CO 2 CH 3 CH 2 OH CH 3 COOH C 6 H 12 O 6

7. Mole Day October 23 from 6:02am to 6:02pm

8. moles to g - g to moles Now we have to actually use this…. If I have 1 mole of Copper, How many grams do I have? g = moles x molar mass g = 1 mole x 63.546 g/mole => 63.546g

9. How many g in? 1.3 moles of water 6.55 moles of salt 12.1 moles of methane 645.9 moles of carbon dioxide

10. Grams to Moles moles = g / molar mass How many moles in? 128 g of water 97.99 g of salt 429 g of methane 10 g of carbon dioxide

11. How many molecules? If I have 1 mole of molecules, I have 6.022 x 10 23 molecules. So: molecules = moles x 6.022 x 10 23 How many molecules in? 36g of water 176g of carbon dioxide

12. Can you do it backwards? moles = molecules / 6.022 x 10 23 How many moles in? 2.8 x 10 24 10 3.011 x 10 12

13. Disclaimer Aloha I put together these power points for use in my science classes. You may use them in your classes. Some images are public domain, some are used under the fair-use provisions of the copyright law, some are mine. Copyright is retained by the owners! Ted Brattstrom