1. The Mole

2. 1 amu = 1.66 x grams
1 C-12 atom = 12 amu
(12)(1.66 x g) = x g
1.992 x grams is the mass of one carbon-12 atom
But … we do not work with single atoms or with gram values this small
We need reasonable numbers to work with in the laboratory

3. The Mole Concept

4. NO… not that kind of mole !!!!

5. The Mole The mole is a number….. A HUGE number……
But still just a number…..
A mole is a collection of
6.02 x 1023 particles
602,000,000,000,000,000,000,000
These particles may be atoms, molecules, ions, or electrons

6. 1 dozen = 12
1 gross = 144
1 mole = 6.02 x 1023
Just how large is this number?
602,000,000,000,000,000,000,000
It is really hard to relate to a number this large ……….but let’s try and see if we can make sense the enormity of the number.

7. If all 5 billion people on Earth were to do nothing but count the atoms in 1 mole of an element, 24 hours a day, at the rate of 1 atom per second…….

8. It would take 4 million years !!

9. 1 mole of seconds represents a span of time…..

10. 4 million times as long as the Earth has already existed !!

11. 1 mole of marbles is enough marbles to cover the entire Earth…

12. to a depth of 50 miles

13. 1 mole of rice grains has a mass equal to….

14. each of the 5 billion people on earth having 1 million cars each

15. A mole of dollars ??

16. How many years would it take you to spend 1 mole of dollars, if you spend at a rate of $1 billion per second ?
$ 6.02 x 1023 = ? Years

17. Using dimensional analysis:
$6.02x1023
1sec
1min
1hr
1day
1 yr
$1x109
60sec
60min
24hr
365day
= 19,089, years
over 19 million years!!!

18. And yet there is 1 mole of water molecules – 6
And yet there is 1 mole of water molecules – x 1023 molecules of water in only 18 mL of water !!

19. Questions ???

20. A Mole Poem

21. Say you had a mole of paper and stacked it toward the sky,
Paper's really thin, but that pile would get so high,
It'd reach up into outer space, in fact I think you'd find,
It'd go up to the moon and back, eighty billion times.

22. Say you had a mole of atoms, would the pile be immense?
Should I say the answer now, or leave you in suspense?
Well, atoms are so very, very small, you understand,
You could hold a mole of atoms in the palm of your hand.

23. So shake a little sugar in the middle of your palm
Now you don't want to spill it, so try and stay calm.
You hardly can imagine and barely realize,
There are more atoms in that sugar than stars up in the sky.

24. Why is this number so special?
The mole is defined as the number of atoms of 12C in exactly grams of pure 12C
There are exactly 1 mole of atoms in the atomic mass of an element when that mass is expressed in grams

25. Avogadro’s Number 1 mole = 6.022 x 1023 particles
1 mole = Avogadro’s number
1 mole = the atomic mass of an element expressed in grams

26. What is the mass of 1 mole of carbon ?
grams
How many atoms?
6.022 x 1023 atoms
What is the mass of ½ mole of carbon ?
grams

27. 12.011 grams of carbon contains the same # of atoms as 1 mole of carbon

28. What is the mass of 1 mole of gold ?
grams
How many atoms?
6.022 x 1023 atoms
What is the mass of ½ mole of gold ?
grams

29. 12. 011 grams of carbon contains the same # of atoms as 196
grams of carbon contains the same # of atoms as grams of gold.

30. What is the mass of 1 mole of Mg ?
grams
What is the mass of 2 moles of Mg ?
grams
How many atoms?
1.204 x 1024 atoms

31. 12. 011 grams of carbon contains the same # of atoms as 196
grams of carbon contains the same # of atoms as grams of gold and the same # of atoms as grams of magnesium.

32. What is the mass of 1 mole of Cu ?
grams
What is the mass of ¼ mole of Cu ?
grams
How many atoms?
x 1023 atoms

33. 12. 011 grams of carbon contains the same # of atoms as 196
grams of carbon contains the same # of atoms as grams of gold and the same # of atoms as grams of magnesium and the same # of atoms as grams of copper.

34. Questions ???

35. Molar Mass: The mass of 1 mole of a substance in grams
The substance can be a compound or an element

36. Calculating Formula Mass
Calculate the formula mass of magnesium carbonate, MgCO3.
84.3 g
24.3 g g x (16.0 g) =
Thus, 84.3 grams is the formula mass
for MgCO3.

37. Molar Mass of a Compound
H2O
2 H = 2 x = g
1 O = 1 x = g
16.00 g g = g
molar mass of water = grams

38. Calculate the molar masses:1. 2. 3. 7. 8.
KMnO4
158.0 g
KCl
74.6 g
Na2SO4
142.1g
CuSO4  5H2O
249.7 g
Mg3(PO4)2
262.9 g

39. Questions ???

40. Mole Conversions

41. Math problems
To solve all math problems in this class you will use the “u,k,p,s” method.
u: unknown
k: known
p: plan
s: solve
Scientific method

42. Molar mass of substance
Moles to Mass
Molar mass of substance
Moles of substance
Mass of substance 27 27

43. Learning Check!
The artificial sweetener aspartame (Nutra-Sweet) formula C14H18N2O5 is used to sweeten diet foods, coffee and soft drinks. How many moles of aspartame are present in 225 g of aspartame?

44. Dimensional Analysis Ex: 225 g C14H18N2O5 = ___________ mole u: mole
Begin with KNOWN – what you want to convert from.
Ex: 225 g C14H18N2O5 = ___________ mole
u: mole
k: 225 g C14H18N2O5
p: 1mole = g C14H18N2O5 s:
225 g C14H18N2O5 1
mole
Known
294.0 g C14H18N2O5

45. Dimensional Analysis 0.765 mole C14H18N2O5 225 g C14H18N2O5

46. U: mole NaCl K: 25 g NaCl P: 1 mole NaCl = 58.5 g NaCl 25 g NaCl
Calculate the number of moles in 25 g of NaCl:
U: mole NaCl
K: 25 g NaCl
P: 1 mole NaCl = 58.5 g NaCl
25 g NaCl
1 mol NaCl
= 0.43 mol NaCl
58.5 g NaCl

47. U: g NaCl K: 2.5 mole NaCl P: 1 mole NaCl = 58.5 g NaCl 58.5 g NaCl
Calculate the number of g in 2.5 moles of NaCl:
U: g NaCl
K: 2.5 mole NaCl
P: 1 mole NaCl = 58.5 g NaCl
58.5 g NaCl
2.5 mol NaCl
= 150 g NaCl
1 mol NaCl

48. Molar Volume
The volumes of gases can be compared at STP, (Standard Temperature and Pressure) when they have
The same temperature
Standard temperature (T)
0°C or 273 K
The same pressure.
Standard pressure (P)
1 atm (760 mm Hg)

49. Molar Volume The molar volume of a gas
Is measured at STP (standard temperature and pressure).
Is 22.4 L for 1 mole of any gas.

50. Everything must go through Moles!!!
Calculations
Moles of substance
Everything must go through Moles!!!
Molar Volume
Volume of
substance

51. = 22.4 L H2 What is the volume occupied by 1.00 moles H2 gas at STP?
U: volume H2
K: 1.00 moles H2
P: 1mole H2 = 22.4 L H2 S:
1.00 mols H2
22.4L H2
Known
= 22.4 L H2
1 mole H2

52. Moles to Number of Entities
Number of atoms or molecules
Avogadro’s number
Moles of substance 23 23

53. Dimensional Analysis 1.2 E 24 molecules
Begin with KNOWN – what you want to convert from.
Ex: 2.0 moles = ___________ molecules
u: molecules
k: 2.0 moles
p: 1mole = 6.02 E23 molecules s:
2.0 moles
Known
6.02 E 23 molecules 1
mole
1.2 E 24 molecules

54. Dimensional Analysis 1.00 mole
Begin with KNOWN – what you want to convert from.
Ex: E 23 molecules = ___________ mole
u: mole
k: 6.02 E 23 molecules
p: 1mole = 6.02 E23 molecules s:
6.02 E 23 molecules 1
mole
Known
6.02 E 23 molecules
1.00 mole

55. Atoms/Molecules and Grams
Since 6.02 X 1023 particles = 1 mole AND 1 mole = molar mass (grams)
You can convert atoms/molecules to moles and then moles to grams! (Two step process)
You can’t go directly from atoms to grams!!!! You MUST go thru MOLES.
That’s like asking what is the weight in ounces of 2 dozen cookies, if 1 cookie weighs 4 oz? You have to convert to dozen first!

56. Everything must go through Moles!!!
Calculations
Avogadro’s number molar mass particles Moles mass
Volume
Everything must go through Moles!!!
Molar Volume

57. Questions ???

58. P: 1mole CO2 = 6.02 E 23 molecules CO2 1mole CO2 = 44.0 g CO2 S:
How many grams are there in 1.5 E 25 molecules CO2?
U: grams CO2
K: 1.5 E 25 molecules CO2
P: 1mole CO2 = 6.02 E 23 molecules CO2
1mole CO2 = 44.0 g CO2 S:
1.5 E 25 CO2
1 mol CO2
44.0g CO2
= 1.1E3g CO2
6.02 x 1023 molecules CO2
1 mol CO2

59. P: 1mole CO2 = 6.02 E 23 molecules CO2 1mole CO2 = 22.4 LCO2 S:
How many liters are there in 1.5 E 25 molecules O2?
U: L CO2
K: 1.5 E 25 molecules CO2
P: 1mole CO2 = 6.02 E 23 molecules CO2
1mole CO2 = 22.4 LCO2 S:
1.5 E 25 CO2
1 mol CO2
22.4 LCO2
= 560 L CO2
6.02 x 1023 molecules CO2
1 mol CO2

60. Questions ???

61. Atoms/Molecules and Volume
How many molecules of O2 are present in 35.4 L of O2 at STP?
U: molecules O2
K: 35.4 L O2
P: 1 mole O2 = 22.4L O2;
1 mole O2 = 6.02 E 23 O2
6.02 X 1023 molecules O2
35.4 L O2
1 mol O2
22. 4 L O2
1 mol O2
= 9.51 X 1023 molecules O2

62. Atoms/Molecules and Grams
How many atoms of Cu are present in 35.4 g of Cu?
U: atoms Cu
K: 35.4 g Cu
P: 1 mole Cu = 63.5 g Cu;
1 mole = 6.02E 23 atoms Cu
6.02 X 1023 atoms Cu
35.4 g Cu
1 mol Cu
63.5 g Cu
1 mol Cu
= 3.36 X 1023 atoms Cu

63. Molar mass of substance Number of atoms or molecules
Avogadro’s number
Molar mass of substance
Number of atoms or molecules
Moles of substance
Mass of substance
Molar Volume
Volume of
substance

64. Calculate the number of grams of Na present in 3
Calculate the number of grams of Na present in 3.00 x atoms of Na:
3.00 x 1018 Na
1 mol Na
23 g Na
6.02 x 1023 Na
1 mol Na
= g or 1.15 x g of Na

65. Calculate the number of atoms of Na in 160.00 grams of Na:
1 mol Na
6.02 x 1023 Na
g Na
23.0 g Na
1 mol Na
= x 1024 atoms of Na

66. Americium is an element that does not occur naturally.
It can be made in very small amounts in a particle accelerator.
Calculate the mass in grams of a sample of americium containing only six atoms.

67. 1 mol Am 243 grams Am 1 mol Am = 2. x 10 -21 grams of Am 6 atoms Am
6.02 x 1023 Am
1 mol Am
= 2. x grams of Am

68. A silicon chip used in an integrated circuit of a microcomputer has a mass of 5.68 mg. How many silicon (Si) atoms are present in the chip?

69. = 1.22 x 10 20 atoms of Si 6.02 x 1023 atoms 1 g 5.68 mg 1 mol Si
28.1 g Si
1 mol Si
= x atoms of Si

70. Aluminum is often used for the structure of light-weight bicycle frames. How many atoms of Al are in grams of Al?

71. 6.02 x 1023 atoms Al
20.00 g Al
1 mol Al
1 mol Al
27.0 g Al
= x 1023 atoms Al

72. The artificial sweetener aspartame (Nutri-Sweet) formula C14H18N2O5 is used to sweeten diet foods, coffee and soft drinks. How many moles of aspartame are present in 225 mg of aspartame?

73. = 7.65 x 10-4 mol C14H18N2O5 = 294.0 g/mol 225 mg C14H18N2O5 1 g

74. Prozac, C17H18F3NO, is a widely used antidepressant that inhibits the uptake of serotonin by the brain. How many atoms of carbon are in grams of Prozac?

75. C17H18F3NO = 309 g/mol = 1 x 1020 atoms C Check your sig figs!!!
1 mol C17H18F3NO
17 mol C
309 g
1 mol C17H18F3NO
1 mol C
= 1 x 1020 atoms C
Check your sig figs!!!

76. Questions ???

77. More Calculations with the Mole

78. Penicillin, the first of a now large number of antibiotics, has the formula C14H20N2SO4. Calculate the mass of x 1010 molecules of penicillin.

79. = 1.0 x 10-11 grams of penicillin
Molar mass C14H20N2SO4 = grams
312.1 grams
C14H20N2SO4
1 mol
C14H20N2SO4
2.0 x 1010 molecules
C14H20N2SO4
6.02 x 1023 C14H20N2SO4
1 mol
C14H20N2SO4
= x grams of penicillin

80. A student drinks 3 cups of coffee in order to stay awake and study
A student drinks 3 cups of coffee in order to stay awake and study. Coffee contains the compound caffeine, a stimulant , with the formula C8H10N4O2
If the caffeine content in an average cup of coffee is 0.5 mg. How many molecules of caffeine did the student ingest?

81. = 4.7 x 1018 molecules of caffeine
(0.5 mg) (3) = 1.5 mg
molar mass caffeine = grams
1 mol
C8H10N4O2
1.5 mg
C8H10N4O2
1 g C8H10N4O2
6.02 x 1023 C8H10N4O2
1000 mg
C8H10N4O2
194.0 g
C8H10N4O2
1 mol C8H10N4O2
= 4.7 x 1018 molecules of caffeine

82. Isopentyl acetate (C7H14O2) is the compound responsible for the scent of bananas. Bees release about 1g of this compound when they sting. The resulting scent attracts other bees to join the attack.

83. How many molecules of isopentyl acetate (C7H14O2) are released in a typical bee sting of about 1g (1 x 10-6 g) ?

84. Molar mass = grams
1.0 x 10-6 g
C7H14O2
1 mol
C7H14O2
6.02 x 1023 C7H14O2
130.0 g
C7H14O2
1 mol C7H14O2
= 4.6 x 1015 molecules C7H14O2

85. How many atoms of carbon would be in the 4
How many atoms of carbon would be in the x 1015 molecules of isopentyl acetate (C7H14O2) ?

86. C7H14O2 Has 7 atoms of carbon for every one molecule
4.626 x 1015 molecules
7 atoms C
1 molecule C7H14O2
= x 1016 atoms of C

87. Diamond is a natural form of pure carbon
A diamond contains 5.0 x1021 atoms of carbon. How many moles of carbon and how many grams of carbon are in this diamond?

88. = 0.099 g C 1 mol C 5.01 x 1021 atoms C 6.022 x 1023 atoms C
8.32 x 10-3 mol C
12.01 g C
1 mol C
= g C

89. How many atoms of carbon are in a 2.00 carat diamond?
( 1.00 carat = grams )

90. = 2.006 x 1022 atom of carbon 0.200 g 1 mol 6.022 x 1023 atoms 2 carat

91. The formula for acetylsalicylic acid (aspirin) is C9H8O4
A typical aspirin tablet contains x 1021 molecules of aspirin. How many moles and how many grams of aspirin are in a typical tablet?

92. C9H8O4 = grams
1 mol
1.67 x 1021 molecules
6.022 x 1023 molecules g
mol
= g
1 mol
500 mg

93. Sucrose or table sugar has the formula C12H22O11
How many moles of sugar are in 20 grams of sugar?
What is the mass of 1.00 x 1020 molecules of sugar?

94. Molar mass = 342.296 g 1 mol 20 g = 0.058 mol sugar 342.296 g
1.00 x 1020 molecules
1 mol g
= g
6.022 x 1023 molecules
1 mol

95. What is the mass of 2.00 moles of Iron (III) oxide, commonly known as rust?

96. Rust = Fe2O3 Molar mass = 159.70 g 159.70 g 2.00 mol = 319.40 g Fe2O3

97. A chemistry student prepares 2
A chemistry student prepares 2.09 grams of the compound copper (II) sulfate in the laboratory.
How many moles of the compound does he make? What is the % copper in the compound?

98. CuSO4 = 159.62 grams 1 mol 2.09 g = 0.0131 mol 159.62 grams
% Cu = ( mass Cu / mass of CuSO4) x 100
63.55 g
% Cu =
x 100
= 39.81% Cu g

99. Calcium carbonate is the principle compound found in pearls, marble, shells, and chalk.

100. A certain sample of calcium carbonate contains 4. 86 moles
A certain sample of calcium carbonate contains 4.86 moles. What is the mass of this sample and how many formula units of calcium carbonate are present in the sample?
CaCO3 is an ionic compound and is not a molecule, but a crystal lattice with the simplest ratio of ions.

101. = 486.44 grams CaCO3 Formula = CaCO3 Molar mass = 100.09 grams
4.86 mol CaCO3
1 mol CaCO3
= grams CaCO3

102. How many atoms of carbon are in the 486.44 grams of CaCO3 ?
6.022 x 1023
molecules
g CaCO3
1 mol CaCO3
1 mol
grams
= x 1027 molecules CaCO3
= x 1027 atoms of C

103. Juglone is a natural herbicide produced from the husks of black walnuts. The formula for juglone is C10H6O3.
Calculate the molar mass of juglone and how many moles of juglone would be in a 1.56 x gram sample.

104. (10 x 12.01) + (6 x 1.008) + (3 x 16.00)
Molar mass = grams
1.56 x 10-2 g
1 mol juglone
174.1 g juglone
= x 10 –5 mol juglone

105. Questions ???