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Introduction to the Mole and Molar Mass

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Purpose At the completion of this unit students will Have a conceptual understanding of the mole as the method of “counting” items and finding the mass of items that can’t be seen. Be able to calculate the number of items (molecules, atoms, ions, and formula units) if given the number of moles. Be able to calculate the number of moles if given the number of items. Be able to calculate the mass of a sample if given the number of moles in a sample. Be able to calculate the number of moles in a sample if given the mass of a sample. Be able to prepare a sample containing a given number of moles. Be able to determine the molar mass of a compound.

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Background When you buy eggs you usually ask for a _______ eggs. You know that one dozen of any item is ______. Dozen 12

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Paper Paper is packaged by a ream. A ream of paper has 500 sheets. Why is it useful to use units like a dozen or a ream?

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What determines how many items should make up a particular unit?

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If you were asked to design a new unit to count something, what would you consider when choosing how many items should be included in your new counting unit?

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ANALYSIS AND INTERPRETATION As you know, a dozen represents 12 items. What if I decided to make a new counting unit? I called this unit a DART. Each dart is _____ items. 1 Dart = 4 items, just like 1 Dozen = 12 items 4

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1. A DART of oranges will have _____ oranges. 4

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2. A DART of pretzels has ____ pretzels. 4

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3. A DART of molecules of water has ____ molecules of water. 4

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4. A DART of particles has ___ particles. 4

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5. A DART of atoms of iron has _____ atoms of iron. 4 26 Fe 55.85

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6. A DART of formula units of salt has _______ formula units of salt. 4

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7. How many Hershey’s Kisses are in 2 DARTS? _______ 8

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8. How many caramels are in 10 DARTS? _______ 40

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9. How many Dum Dum Pops are in 400 DARTS? _______ 1600

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10. How many Starbursts are in 1/2 DART? _____ 2

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15. How many atoms of silver are in 20 DARTS? _______ 80 47 Ag 107.9

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Write the directions for finding the number of items if given the number of DARTS

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17. How many DARTS are 16 Hershey’s Kisses? ______ 4

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18. How many DARTS are 100 pretzels? ____ 25

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19. How many DARTS are 400 Starbursts? ____ 100

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20. How many DARTS is 1 orange? ________ (Write a fraction or a decimal.) ¼ 0.25

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21. How many DARTS are 2 caramels? _____ 0.5

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23. How many DARTS are 48 Hershey’s Kisses? ____ 12

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25. How many DARTS are 24 Jolly Ranchers? ______ 6

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27. How many DARTS are 20 caramels? ______ 5

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Write your own directions for finding the number of DARTS given the number of pieces

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DARTS DART of molecules of water would be too small to see. Scientists had to select a bigger unit for counting molecules of substances. The unit scientists use is called a MOLE.

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One MOLE of anything has 602,200,000,000,000,000,000,000 items.

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AVOGADRO’S NUMBER 6.02 x 10 23 One MOLE of anything has 6.02 x 10 23 items.

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A. What is the Mole? A counting number (like a dozen) Avogadro’s number (N A ) 1 mol = 6.02 10 23 items A large amount!!!!

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n 1 mole of hockey pucks would equal the mass of the moon! A. What is the Mole? 1 mole of pennies would cover the Earth 1/4 mile deep! n 1 mole of basketballs would fill a bag the size of the earth!

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28. How many Hershey’s Kisses make up 1 MOLE? 6.02 x 10 23

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A mole of Caramels is _____ caramels. 6.02 x 10 23

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A mole of Jolly Ranchers is ______ Jolly Ranchers 6.02 x 10 23

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A mole of silver atoms is _______ atoms of silver. 47 Ag 107.9 6.02 x 10 23

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29. How many caramels make up 10 MOLES? 10 [6.02 x 10 23 ] 60.2 x 10 23 Which is 6.02 x 10 24

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30. Find the number of Jolly Ranchers in 4 MOLES. 4 [6.02 x 10 23 ] = 2.408 x 10 24

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31. Find the number of atoms of sodium in 2 MOLES. 2[6.02 x 10 23 ]= 1.20 x 10 24 11 Na 22.99

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32. Find the number of molecules of water in 6 MOLES. 6[6.02 x 10 23 ]= 3.61 x 10 24

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33. Find the number of caramels in 0.5 MOLES..5[6.02 x 10 23 ]= 3.011 x 10 23

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34. How many moles of caramels is 6.02x10 23 of caramels? ___ 1

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35. How many moles of Starbursts is 6.02x10 23 of Starbursts? ___ 1

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36. How many moles of Gobstoppers is 12.04x10 23 of Gobstoppers? ___ 2 12.04 x 10 23 = 2 6.022 x 10 23

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37. How many atoms of potassium make up one MOLE? 6.02 x 10 23 19 K 39.10

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38. How many atoms of potassium make up 2 MOLES? 2[6.02 x 10 23 ] 12.044 x 10 23 1.20 x 10 24 19 K 39.10

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39. How many molecules of water make up 1 MOLE? 6.02 x 10 23

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40. How many molecules of water make up 5 MOLES? 5[6.02 x 10 23 ]= 3.01 x 10 24

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41. How many moles are 6.022 x 10 23 atoms of sodium? _____ 1

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42. How many moles are 12.04 x 10 23 atoms of carbon? _____ 2 12.04 x 10 23 = 2 6.022 x 10 23

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43. How many moles are 18.06 x 10 23 atoms of sodium? _____ 3 18.06 x 10 23 = 3 6.022 x 10 23

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44. How many moles are 60.22 x 10 23 atoms of sodium? _____ 10 60.22 x 10 23 = 10 6.022 x 10 23

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45. How many moles are 6.02 x 10 23 molecules of water? _____ 1

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46. How many moles are 12.04 x 10 23 molecules of water? _____ 2 12.04 x 10 23 = 2 6.022 x 10 23

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47. How many moles are 30.10 x 10 23 molecules of water? _____ 5 30.10 x 10 23 = 5 6.022 x 10 23

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Part 2

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Molar Mass Scientists use the Periodic Table to determine the mass of a mole of atom of an element. For example, a mole of carbon (C) atoms would have a mass of 12.01g.

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Periodic Table

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1 mole carbon atoms = __________ atoms = __________ g.. 6 C 12.01 6.02 x 10 23

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1 mole helium atoms = __________ atoms = _______ g.. 2 He 4.00 6.02 x 10 23

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1 mole iron atoms = __________ atoms = _______ g.. 26 Fe 55.85 6.02 x 10 23

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1 mole boron atoms = __________ atoms = _______ g.. 5 B 10.81 6.02 x 10 23

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1 mole He atoms is 4.00 g, so 2 mole He atoms = ______ g. 2 He 4.00 8.00

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1 mole Fe atoms is 55.85 g, so 0.5 mole Fe atoms = ______ g. 26 Fe 55.85 27.93

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1 mole C atoms is 12.01 g, so 12 mole C atoms = ______ g 6 C 12.01 144.12

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1 mole B atoms is 10.81 g, so 3 mole B atoms = ______ g 5 B 10.81 32.43

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120.1 g C atoms = ______ mol 6 C 12.01 10 120.1 ÷ 12.01 = 10

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8.00 g He atoms = ______ mol 2 He 4.00 2 8.00 ÷ 4.00 = 2

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167.55 g Fe atoms = ______ mol 26 Fe 55.85 3 167.55 ÷ 55.85 = 3

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5.405 g B atoms = ______ mol 5 B 10.81 0.5 5.405 ÷ 10.81 = 0.5

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66. The mass of 1 mole of Nickel (Ni) is ____ g. 28 Ni 58.69

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67. The mass of 4 moles of Strontium (Sr) is _____g. 38 Sr 87.62 350.48

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68. The mass of 0.5 moles of Lead (Pb) is ____ g. 82 Pb 207.2 103.6

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69. The mass of 100 moles of (Ni) is _____ g. 28 Ni 58.69 5869.00

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Molar Mass Scientists also use the Periodic Table to determine the molar mass (formula weight) of compounds. The molar mass of the compound is the sum of the molar masses of the elements that make up the compound.

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Potassium Chloride The molar mass of Potassium Chloride is: Potassium (K) 39.10 g/mole Chloride (Cl) +34.45 g/mole 73.55 g/mole

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Potassium Permanganate The molar mass of KMnO 4 is the sum of all the molar masses times the number of atoms of each element for the molecule (subscript).

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Potassium Permanganate KMnO 4 Potassium (K) 39.10 g/mole Manganese (Mn) 54.94g/mole Oxygen (O) 4[16.00 g/mole] 158.04 g/mole.

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70. The molar mass of 1 mole of Sodium Chloride (NaCl) is____ g. 58.44

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71. The molar mass of 1 mole of Lead Iodide (PbI 2 ) is _____ g. 461.0

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72. The mass of 100 moles of Nickel Sulfide (NiS) is ________ g. 9076.00

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73. The mass of 1 mole of is Glucose (C 6 H 12 O 6 ) is ______ g. 180.156

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74. The mass of 1 mole of is Sucrose (C 12 H 24 O 12 ) _______ g. 306.31

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75. The mass of 4 moles of Glucose (C 6 H 12 O 6 ) is _________ g. 720.624

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Mole Conversions In chemistry, the mole is the standard measurement of amount. However, balances DO NOT give readings in moles. Balances give readings in grams. So the problem is that, while we compare amounts of one substance to another using moles, we must also use grams, since this is the information we get from balances.

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There are three steps to converting grams of a substance to moles. 1. Determine how many grams are given in the problem. 2. Calculate the molar mass of the substance. 3. Divide step one by step two.

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The three steps above can be expressed in the following proportion: Grams Moles --------------- = -------------- Molar Mass 1 Mole

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Example #1 - Convert 25.0 grams of KMnO 4 to moles. Step One: The problem will tell you how many grams are present. Look for the unit of grams. The problem gives us 25.0 grams. Step Two: You need to know the molar mass of the substance. The molar mass of KMnO4 is 158.034 grams/mole. Potassium (K) =39.10 x 1=39.10 g Manganese (Mn) =54.94 x 1=54.94 g Oxygen (O)=16.00 x 4=64.00 g --------------- 158.04 g Step Three: You divide the grams given by the substance's molar mass (25.0/158.04) The answer of 0.16 mole has been rounded off.

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Example #2 - Calculate how many moles are in 57.0 grams of Mg(NO 3 ) 2 Step One: 57.0 grams are given in the text of the problem. Step Two: The molar mass is 148 grams/mole. Mg (Magnesium) =24 x 1=24 g N (Nitrogen) =14 x 2=28 g O (Oxygen) =16 x 6=96 g Step Three: Again you divide the grams by the substances molar mass (57.0 g/148 g). This answer has been rounded to 0.39 moles.

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Practice Problems

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1. Calculate the moles present in: 2.00 grams of H 2 O.11 moles water

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2. Calculate the moles present in: 75.57 grams of KBr.635 moles KBr

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3. Calculate the moles present in: 100.0 grams of KClO 4.72 moles KClO 4

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4. Calculate the moles present in: 225.5 grams of Sucrose (C 12 H 24 O 12 ).63 moles Sucrose

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5. Calculate the moles present in: 350.0 grams of Glucose (C 6 H 12 O 6 ) 1.943 moles Glucose

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Homework

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1. Calculate the moles present in: 3.00 grams of NaCl.05 moles

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2. Calculate the moles present in: 25.0 grams of NH 3 1.47 moles NH 3

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3. Calculate the moles present in: 16.0 grams of KCl.21 moles KCl

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4. Calculate the moles present in: 30.25 grams of BeCl 2.38 moles KCl

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5. Calculate the moles present in: 175.25 grams of Li 2 S 3.81 moles Li 2 S

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6. Calculate the moles present in: 75.62 grams of CO 2 1.72 moles CO 2

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7. Calculate the moles present in: 56.5 grams of H 2 O 3.14 moles H 2 O

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8. Calculate the moles present in: 22.6 grams of CH 3 COOH.38 moles CH 3 COOH

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9. Calculate the moles present in: 18.4 grams of AgCl.13 moles AgCl

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10. Calculate the moles present in: 68.3 grams of HCN 2.53 moles HCN

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