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# 12 15 Mole Review

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### 12 15 Mole Review

1. 1. Launch: 12/15   Grab your binder and immediately take a seat!   Place HW (Review Worksheet #1), binder paper, and a pen/pencil on your desk. Review Objective #2: Tonight’s HW: Finish Review Worksheet #2
2. 2. Launch 12/15 4.  Which of the following is a balanced equation for the combustion of ethanol (C2H5OH)? a.  C2H5OH + 3O2  CO2 + 2H2O b.  C2H5OH + 3O2  2CO2 + 3H2O c.  C2H5OH + O2  2CO2 + 3H2O d.  C2H5OH + 2O2  3CO2 + 2H2O
3. 3. Launch 12/15 __C2H2 + __H2  __CH4 5.  When the equation above is completely balanced, the coefficient for H2 would be a.  1 b.  2 c.  3 d.  4
4. 4. Launch 12/15 4.  Which of the following is a balanced equation for the combustion of ethanol (C2H5OH)? a.  C2H5OH + 3O2  CO2 + 2H2O b.  C2H5OH + 3O2  2CO2 + 3H2O c.  C2H5OH + O2  2CO2 + 3H2O d.  C2H5OH + 2O2  3CO2 + 2H2O
5. 5. Launch 12/15 __C2H2 + __H2  __CH4 5.  When the equation above is completely balanced, the coefficient for H2 would be a.  1 b.  2 c.  3 d.  4
6. 6. Announcements   Unit #5 Exam on Thursday   2 days to review   Ask questions!   No copying HW or classwork!   Make-up work is due on Wednesday   Binder check this week
7. 7. Exam Information   30 multiple-choice questions   Balancing equations (6 questions = 20%)   The mole (9 questions = 30%)   Conversions (15 questions = 50%)   gram  mole (6 questions)   gram  atoms (3 questions)   gram  gram (6 questions)   3 free response
8. 8. Review: The Mole Mr. Heffner 12/15/09
9. 9. What’s a mole?
10. 10. What’s a mole?   A mole is…   a unit of measurement   the number of atoms in 12g of carbon-12   6.02 X1023 atoms   Avogadro’s # ..or particles, or molecules
11. 11. What’s molar mass?   Molar mass is…   the sum of the atomic masses in a molecule   a.k.a “molecular mass” C2H2 Molar mass = mass of C + mass of C + mass of H + mass of H = 2X(mass of C) + 2X(mass of H) = 2X(12.01) + 2X(1.01) = 24.02 + 2.02 = 26.04 g/mol Units!
12. 12. Conversions ? grams 6.02 X 1023 atoms 1 mole 1 mole ? moles Grams ? moles Moles Atoms 1 mole 1 mole ? grams 6.02 X 1023 atoms
13. 13. Conversions   There is a 3-step process for conversions: 1.  Write down the starting information and look at the ending information. 2.  Using the “Heart of Chemistry”, pick the correct conversion number “How many…” factor(s). 3.  Cancel like terms and do the math!
14. 14. Example #1 How many moles of H2O are there in 9.01 grams of H2O?   Step #1: Write down the starting information and look at the ending information. 9.01 grams
15. 15. Example #1 How many moles of H2O are there in 9.01 grams of H2O?   Step #2: Using the “Heart of Chemistry”, pick the correct conversion factor(s). 9.01 grams X
16. 16. Example #1 How many moles of H2O are there in 9.01 grams of H2O?   Step #2: Using the “Heart of Chemistry”, pick the correct conversion factor(s). ? grams 6.02 X 1023 atoms 1 mole 1 mole ? moles Grams ? moles Moles Atoms Start 1 mole 1 mole ? grams 6.02 X 1023 atoms End Molar mass
17. 17. Example #1 How many moles of H2O are there in 9.01 grams of H2O?   Step #2: Using the “Heart of Chemistry”, pick the correct conversion factor(s). 1 mole 9.01 grams X = 18.02 grams
18. 18. Example #1 How many moles of H2O are there in 9.01 grams of H2O?   Step #3: Cancel like terms and do the math! 1 mole 9 X 1 mole 9.01 grams X = 18.02 grams 18 = .5 moles units!
19. 19. Example #2 How many atoms are there in 1.5 moles of CO2?   Step #1: Write down the starting information and look at the ending information. 1.5 moles
20. 20. Example #2 How many atoms are there in 1.5 moles of CO2?   Step #2: Using the “Heart of Chemistry”, pick the correct conversion factor(s). 1.5 moles
21. 21. Example #2 How many atoms are there in 1.5 moles of CO2?   Step #2: Using the “Heart of Chemistry”, pick the correct conversion factor(s). ? grams 6.02 X 1023 atoms 1 mole 1 mole ? moles Grams ? moles Moles Atoms 1 mole 1 mole End ? grams 6.02 X 1023 atoms Start
22. 22. Example #2 How many atoms are there in 1.5 moles of CO2?   Step #2: Using the “Heart of Chemistry”, pick the correct conversion factor(s). 6.02 X 1023 atoms 1.5 moles X = 1 mole
23. 23. Example #2 How many atoms are there in 1.5 moles of CO2?   Step #3: Cancel like terms and do the math! Ignore 6.02 X 1023 atoms 1.5 X 6 X 1023 atoms 1.5 moles X = 1 mole 1 = 9 X 1023 atoms
24. 24. Example #3 How many grams of CH4 are there in 12.04 X 1023 molecules?   Step #1: Write down the starting information and look at the ending information. 12.04 X 1023 molecules
25. 25. Example #3 How many grams of CH4 are there in 12.04 X 1023 molecules?   Step #2: Using the “Heart of Chemistry”, pick the correct conversion factor(s). 12.04 X 1023 molecules X =
26. 26. Example #3 How many grams of CH4 are there in 12.04 X 1023 molecules?   Step #2: Using the “Heart of Chemistry”, pick the correct conversion factor(s). ? grams 6.02 X 1023 atoms 1 mole 1 mole ? moles Grams ? moles Moles Atoms End 1 mole 1 mole Start ? grams 6.02 X 1023 atoms
27. 27. Example #3 How many grams of CH4 are there in 12.04 X 1023 molecules?   Step #2: Using the “Heart of Chemistry”, pick the correct conversion factor(s). 1 mol 16.05 g 12.04 X 1023 molecules X X 1 mol = 6.02 X 10 23 molecules
28. 28. Example #3 How many grams of CH4 are there in 12.04 X 1023 molecules?   Step #3: Cancel like terms and do the math! 1 mol 16.05 g 12.04 X 1023 molecules X X 1 mol = 6.02 X 10 23 molecules 12 X 1 X 16 g = 6X1 32 g = 2 X 16 g =
29. 29. Conversion Rotations   Directions:   Pick a problem and fill in the blanks   Solve showing all work   When finished, Mr. Heffner will come around to stamp your work   Rules:   If you pick it, solve it   Only one card at a time   Show your work!   Work together
30. 30. Exit Slip 1.  What is the molar mass of Al(OH)3? a.  43.99 g/mol b.  78.01 g/mol c.  300.03 g/mol d.  303.00 g/mol
31. 31. Exit Slip 2.  How many moles of N2 are there in 28.02g of N2? a.  1 moles b.  2 mole c.  .5 moles d.  28.02 moles
32. 32. Exit Slip 3.  Choose the answer below that shows how to calculate: “How many atoms are there in 2 moles of O2?” 32.00 grams a.  16 moles X 1 mole 1 mole b.  2 moles X 16.00 grams 1 atoms c.  2 moles X 6.02 X 1023 moles 6.02 X 1023 atoms d.  2 moles X 1 mole
33. 33. Exit Slip 4.  Which of the following correctly shows how to convert 64.00g of O2 to atoms? 6.02 X 1023 atoms a.  32.00g X 32.00g 1 mole b.  64.00g X 32.00 g 1 mole 6.02 X 1023 atoms c.  64.00g X 32.00 g X 1 mole 1 mole 1 atoms d.  64.00 g X X 6.02 X 10 23 g 32.00 moles
34. 34. Exit Slip 5.  How many grams does 12.04 X 1023 molecules of H2O weigh? a.  9.01g b.  18.02g c.  27.03g d.  36.04g
35. 35. Homework   Finish practice questions worksheet
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