introduction to the mole and molar mass
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Introduction to the Mole and Molar
Mass
PurposeAt 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.
Background
• When you buy eggs you usually ask for a _______ eggs.
• You know that one dozen of any item is ______.
Dozen
12
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?
• What determines how many items should make up a particular unit?
• 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?
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 like1 Dozen = 12 items
4
1. A DART of oranges will have _____ oranges.4
2. A DART of pretzels has ____ pretzels. 4
3. A DART of molecules of water has ____ molecules of water.
4
4. A DART of particles has ___ particles.4
5. A DART of atoms of iron has _____ atoms of iron.
4
26Fe
55.85
6. A DART of formula units of salt has _______ formula units of salt.
4
7. How many Hershey’s Kisses are in 2 DARTS? _______8
8. How many caramels are in 10 DARTS? _______40
9. How many Dum Dum Pops are in 400 DARTS? _______1600
10. How many Starbursts are in 1/2 DART? _____2
15. How many atoms of silver are in 20 DARTS? _______80
47Ag
107.9
Write the directions for finding the number of items if given the number of DARTS
17. How many DARTS are 16 Hershey’s Kisses? ______4
18. How many DARTS are 100 pretzels? ____25
19. How many DARTS are 400 Starbursts? ____100
20. How many DARTS is 1 orange? ________
(Write a fraction or a decimal.)
¼ 0.25
21. How many DARTS are 2 caramels? _____0.5
23. How many DARTS are 48 Hershey’s Kisses? ____12
25. How many DARTS are 24 Jolly Ranchers? ______6
27. How many DARTS are 20 caramels? ______5
Write your own directions for finding the number of DARTS given the number of pieces
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.
One MOLE of anything has 602,200,000,000,000,000,000,000 items.
AVOGADRO’S NUMBER
•6.02 x 1023 • One MOLE of anything
has 6.02 x 1023 items.
A. What is the Mole?• A counting number (like a dozen)
• Avogadro’s number (NA)
• 1 mol = 6.02 1023 items
A large amount!!!!
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!
1 mole of basketballs would fill a bag the size of the earth!
28. How many Hershey’s Kisses make up 1 MOLE? 6.02 x 1023
A mole of Caramels is _____ caramels.6.02 x 1023
A mole of Jolly Ranchers is ______Jolly Ranchers
6.02 x 1023
A mole of silver atoms is _______ atoms of silver.
47Ag
107.9
6.02 x 1023
29. How many caramels make up 10 MOLES?
10 [6.02 x 1023]
60.2 x 1023
Which is
6.02 x 1024
30. Find the number of Jolly Ranchers in 4 MOLES.
4 [6.02 x 1023] =
2.408 x 1024
31. Find the number of atoms of sodium in 2 MOLES.
2[6.02 x 1023]=
1.20 x 1024
11Na
22.99
32. Find the number of molecules of water in 6 MOLES.
6[6.02 x 1023]=
3.61 x 1024
33. Find the number of caramels in 0.5 MOLES.
.5[6.02 x 1023 ]=
3.011 x 1023
34. How many moles of caramels is 6.02x1023 of caramels? ___1
35. How many moles of Starbursts is 6.02x1023 of Starbursts? ___1
36. How many moles of Gobstoppers is 12.04x1023 of Gobstoppers? ___2
12.04 x 1023 = 26.022 x 1023
37. How many atoms of potassium make up one MOLE? 6.02 x 1023
19K
39.10
38. How many atoms of potassium make up 2 MOLES?
2[6.02 x 1023 ]
12.044 x 1023
1.20 x 1024
19K
39.10
39. How many molecules of water make up 1 MOLE?
6.02 x 1023
40. How many molecules of water make up 5 MOLES?
5[6.02 x 1023 ]=
3.01 x 1024
41. How many moles are 6.022 x 1023 atoms of sodium? _____1
42. How many moles are 12.04 x 1023 atoms of carbon? _____2
12.04 x 1023 = 26.022 x 1023
43. How many moles are 18.06 x 1023 atoms of sodium? _____3
18.06 x 1023 = 36.022 x 1023
44. How many moles are 60.22 x 1023 atoms of sodium? _____10
60.22 x 1023 = 106.022 x 1023
45. How many moles are 6.02 x 1023 molecules of water? _____1
46. How many moles are 12.04 x 1023 molecules of water? _____2
12.04 x 1023 = 26.022 x 1023
47. How many moles are 30.10 x 1023 molecules of water? _____5
30.10 x 1023 = 56.022 x 1023
Part 2
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.
Periodic Table
1 mole carbon atoms = __________ atoms = __________ g..
6C
12.01
12.01
6.02 x 1023
1 mole helium atoms = __________ atoms = _______ g..
2He
4.00
4.00
6.02 x 1023
1 mole iron atoms = __________ atoms = _______ g..
26Fe
55.85
55.85
6.02 x 1023
1 mole boron atoms = __________ atoms = _______ g..
5B
10.81
10.81
6.02 x 1023
1 mole He atoms is 4.00 g, so
2 mole He atoms = ______ g.
2He
4.00
8.00
1 mole Fe atoms is 55.85 g, so
0.5 mole Fe atoms = ______ g.
26Fe
55.85
27.93
1 mole C atoms is 12.01 g, so
12 mole C atoms = ______ g
6C
12.01
144.12
1 mole B atoms is 10.81 g, so
3 mole B atoms = ______ g
5B
10.81
32.43
120.1 g C atoms = ______ mol
6C
12.01
10
120.1 ÷ 12.01 = 10
8.00 g He atoms = ______ mol
2He
4.00
2
8.00 ÷ 4.00 = 2
167.55 g Fe atoms = ______ mol
26Fe
55.85
3
167.55 ÷ 55.85 = 3
5.405 g B atoms = ______ mol
5B
10.81
0.5
5.405 ÷ 10.81 = 0.5
66. The mass of 1 mole of Nickel (Ni) is ____ g.
28Ni
58.69
58.69
67. The mass of 4 moles of Strontium (Sr) is _____g.
38Sr
87.62
350.48
68. The mass of 0.5 moles of Lead (Pb) is ____ g.
82Pb
207.2
103.6
69. The mass of 100 moles of (Ni) is _____ g.
28Ni
58.69
5869.00
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.
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
Potassium Permanganate
• The molar mass of KMnO4 is the sum of all the molar masses times the number of atoms of each element for the molecule (subscript).
Potassium Permanganate KMnO4
• Potassium (K) 39.10 g/mole
• Manganese (Mn) 54.94g/mole
• Oxygen (O) 4[16.00 g/mole] 158.04 g/mole.
70. The molar mass of 1 mole of Sodium Chloride (NaCl) is____ g.58.44
71. The molar mass of 1 mole of Lead Iodide (PbI2) is _____ g.461.0
72. The mass of 100 moles of Nickel Sulfide (NiS) is ________ g.9076.00
73. The mass of 1 mole of is Glucose (C6H12O6) is ______ g.180.156
74. The mass of 1 mole of is Sucrose (C12H24O12 ) _______ g.306.31
75. The mass of 4 moles of Glucose (C6H12 O6) is _________ g.720.624
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.
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.
The three steps above can be expressed in the following proportion:
Grams Moles
--------------- = --------------
Molar Mass 1 Mole
Example #1 - Convert 25.0 grams of KMnO4 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 gManganese (Mn) = 54.94 x 1 = 54.94 gOxygen (O) = 16.00 x 4 = 64.00 g --------------- 158.04 gStep 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.
Example #2 - Calculate how many moles are in 57.0 grams of Mg(NO3)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 gN (Nitrogen) = 14 x 2= 28 gO (Oxygen) = 16 x 6= 96 gStep 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.
Practice Problems
1. Calculate the moles present in:
2.00 grams of H2O
.11 moles water
2. Calculate the moles present in:
75.57 grams of KBr
.635 moles KBr
3. Calculate the moles present in:
100.0 grams of KClO4
.72 moles KClO4
4. Calculate the moles present in:
225.5 grams of Sucrose (C12H24O12)
.63 moles Sucrose
5. Calculate the moles present in:
350.0 grams of Glucose (C6H12O6)
1.943 moles Glucose
Homework
1. Calculate the moles present in:
3.00 grams of NaCl
.05 moles
2. Calculate the moles present in:
25.0 grams of NH3
1.47 moles NH3
3. Calculate the moles present in:
16.0 grams of KCl
.21 moles KCl
4. Calculate the moles present in:
30.25 grams of BeCl2
.38 moles KCl
5. Calculate the moles present in:
175.25 grams of Li2S
3.81 moles Li2S
6. Calculate the moles present in:
75.62 grams of CO2
1.72 moles CO2
7. Calculate the moles present in:
56.5 grams of H2O
3.14 moles H2O
8. Calculate the moles present in:
22.6 grams of CH3COOH
.38 moles CH3COOH
9. Calculate the moles present in:
18.4 grams of AgCl
.13 moles AgCl
10. Calculate the moles present
in: 68.3 grams of HCN
2.53 moles HCN
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