1. Warm Up11-18-15 1.Which atom did Avogadro based his experiment on? 2.How many molecules are in 1 mol of oxygen gas? 3.The molar mass of 1 CO 2 compound is ___ 4.What is the mass of 3 CO 2 compounds? 5.Define sophmole. Homework Nov 20 - Quiz Unit 5 Nov 21 - Online HW Unit 5 Dec 9 - Deadline to retake quizzes and turn in absent work Agenda Notes Unit 5-5 Group solving problems Online HW

3. Notes Unit 5-5 Moles Conversion

4. Bubble Diagram Using moles to convert between mass and the amount of atoms in a compound

5. Conversion Types Moles to grams Moles to atoms/molecules Grams to moles Atoms/molecules to moles *Grams to atoms *Atoms to grams

6. Mole to Gram Conversions 1) What is the mass of 2.5 moles of phosphorus?

7. Multiple the # of moles given by the molar mass Example: What is the mass of 2.5 moles of phosphorus? Molar mass=30.97 g/mol 2.5 mol P30.97 g P = 2.5 x 30.97 g P =77 g P 1 mol P1 Mole to Gram Conversions moles A  grams A Molar mass (from periodic table)

8. Gram to Mole Conversions 2) How many moles are in 12 grams of FeO?

9. Multiply the # of grams given by the inverse of the molar mass. Example: How many moles of iron are in 12 grams of iron? 12 g Fe1 mol FeO = 12 mol Fe = 0.169 moles Fe 71.85 g Fe 71.85 Gram to Mole Conversions grams A  moles A Molar mass (from periodic table)

10. Mole to Atoms 3) How many atoms are in 3.00 moles of Na?

11. Multiple the # of moles given by Avogadro’s number Example: How many atoms are in 3.00 moles of Na? Mole to Atoms 3.00 mol Na 6.02 x 10 23 atoms Na = 3.00 x (6.02 x 10 23 ) atoms Na = 1.81 x 10 24 atoms Na 1 mol Na1 moles A  atoms A Avogadro’s Number (6.02 x 10 23 particles/mol)

12. Atoms to Moles 4) If you have 7.45 x 10 25 molecules of O 2 gas, how many moles do you have?

13. Multiple the # of moles given by the inverse of Avogadro’s number Example: If you have 7.45 x 10 24 molecules of Cu, how many moles do you have? 7.45 x 10 25 molecules Cu1 mol Cu = 7.45 x 10 25 mol Cu = 124 mol Cu 6.02 x 10 23 molecules Cu 6.02 x 10 23 Atoms to Moles atoms A  moles A Avogadro’s Number (6.02 x 10 23 particles/mol)

14. Grams to Atoms 5) How many atoms are in 26 grams of cobalt?

15. 2 steps! 1 st multiply by the inverse of the molar mass, 2 nd multiply by Avogadro’s number Example: How many atoms are in 26 grams of cobalt? 26 g Co1 mol Co6.02 x 10 23 molecules Co = 2.7 x 10 23 molecules Co 58.93 g Co1 mol Co Grams to Moles to Atoms Grams A  moles A  molecules A Avogadro’s Number (6.02 x 10 23 particles/mol) Molar mass (from periodic table)

16. Atoms to Grams 6) What is the mass of 8.60 x 10 23 atoms of NaCl?

17. 2 steps! 1 st multiply by the molar mass, 2 nd multiply by the inverse of Avogadro’s number Example: What is the mass of 8.60 x 10 23 molecules of As? 8.60 x 10 23 molecules As1 mol As74.92 g As =107 g As 6.02 x 10 23 molecules As 1 mol As Atoms to Moles to Grams molecules A  moles A  Grams A Avogadro’s Number (6.02 x 10 23 particles/mol) Molar mass (from periodic table)

18. Group work Work on questions #1-9 with a partner ANSWERS: 1) 1 x 10 3 2) 7.16 x 10 -3 3) 1.67 x 10 -4 4) 4.454 x 10 24 5) 2.53 x 10 21 6) 3.01 x 10 24 7) 96 grams 8) 5.778 x 10 -2 9) 722.16 grams

19. Assignments Summary Online HW https://quest.cns.utexas.edu/