1. Please pick up the materials in the front and take a seat
Happy New Year!
Please pick up the materials in the front and take a seat

2. How was my break?

3. Policies and Procedures
- Test Corrections
- Pink Sheets & Late Work
- Notes & Practice Problems

4. Chapter 8 BEAT Sheet
Calculate the percent composition of any element in a compound
Determine the empirical formula of a compound given its percent composition
Determine the molecular formula of a compound given its percent composition and
molar mass
Determine the empirical formula of a hydrate from lab data
Perform mole road calculations to determine atoms, molecules, ions, mass, or moles
from relevant data
Describe the labs you performed this unit and what the key concept/learning was from
each lab

5. We have talked about this
What is a mole?
We have talked about this
6.02 X 1023 times!

6. What is a mole?
A mole is the base unit used to measure the amount of a substance, abbreviated mol. One mol of anything is equal to x 1023 pieces of that thing.

7. Mole Practice
1. How many moles in 5.4 x 1020 atoms of Pb?

8. Mole Practice
2. How many atoms in 3.5 moles of Ag?

9. Mole Practice
3. How many total molecules in 1 mole of glucose: C6H12O6?

10. Molecular and Formula Weight
Last semester we learned about molecular weight and touched on formula weight. It is important to remember that a single atom’s weight in amu is the same as one mole of that atom in grams.
Example:
 The weight of a single atom of aluminum is grams. Therefore 1
mol of Al weighs grams.

11. Molecular and Formula Weight
This is known as the atomic mass: the mass of 1 mole of atoms of any element. This is the number that’s on the periodic table. But atoms are rarely by themselves—they are usually in compounds.
How do you find the mass of a mole of a compound??

12. Molecular and Formula Weight
Example:
Find the molecular mass of CO2
C: 1 x = g
O: 2 x = g g

13. Molecular and Formula Weight
Example:
Find the formula mass of (NH4)CO3
N: 1 x = g
H: 4 x = g
C: 1 x = g
O: 3 x = g g

14. Molecular and Formula Weight Practice Problems
4. Find the molecular mass of C6H12O6

15. Molecular and Formula Weight Practice Problems
5. Find the molecular mass of dinitrogen pentaoxide

16. Molecular and Formula Weight Practice Problems
6. Find the Formula mass of Na2SO4

17. Molecular and Formula Weight Practice Problems
7. Find the Formula mass of potassium phosphate

18. Molar Mass of a Substance
When trying to find the mass of one mole of a substance we will make life easier by just referring to the molar mass of a material. It can be an atom, a molecule, or an ionic compound. We use the same technique to calculate the mass of a mole of O2, Pb, CH4, or NaCl.

19. Molar Mass Practice Problems
8. Find the molar mass of O2

20. Molar Mass Practice Problems
9. Find the molar mass of Pb

21. Molar Mass Practice Problems
10. Find the molar mass of CH4

22. Molar Mass Practice Problems
11. Find the molar mass of NaCl

23. Molar Mass Practice Problems
12. When do you use atomic mass, molecular weight, and formula weight to find the molar mass?

24. Molar Mass Conversion
Since molar mass gives you the amount of grams in one mole of a substance you can use the molar mass to convert from grams to moles or vice versa.

25. 56.8 𝑔 𝑀𝑛𝑂2 1 1 𝑚𝑜𝑙 𝑀𝑛𝑂2 86.9368 𝑔 𝑀𝑛𝑂2 = .653 𝑚𝑜𝑙 𝑀𝑛𝑂2
Molar Mass Conversion
Examples:
How many moles in 56.8 g of MnO2?
  𝑔 𝑀𝑛𝑂 𝑚𝑜𝑙 𝑀𝑛𝑂 𝑔 𝑀𝑛𝑂2 = .653 𝑚𝑜𝑙 𝑀𝑛𝑂2

26. Molar Mass Conversion Examples: How many grams in 3.4 moles of C6H6?
  3.4 𝑚𝑜𝑙 𝐶6𝐻 𝑔 𝐶6𝐻6 1 𝑚𝑜𝑙 𝐶6𝐻6 =260 𝑔 𝐶6𝐻6

27. Molar Mass Conversion Practice Problems
13. How many moles are in g of HNO3

28. Molar Mass Conversion Practice Problems
14. How many moles are in 19.5 grams of NaCl

29. Molar Mass Conversion Practice Problems
15. How many grams are in 15 mols of AlPO4

30. Molar Mass Conversion Practice Problems
16. How many grams are in 5.34 mols of KBr

31. The Volume of a Mole of Gas
Until this point we have only converted from mass to moles, but what happens when we convert from volume to moles?
Describe how we can measure the mass of a solid substance:
 Describe how we can measure the mass of a liquid substance:
 Can we measure the mass of a gaseous substance?

32. The Volume of a Mole of Gas
When we convert from volume to moles or moles to volume we use a constant of 22.4 liters per mole. This constant tells us that one mole of a gas has a volume of 22.4 liters. When using this constant we assume the gas is at STP (standard temperature and pressure) which is 1 atm and 0C

33. The Volume of a Mole of Gas
Also remember that if there is one mole of a sample of gas, that sample must have 6.02 x 1023 atoms in it!
But since gases have different masses than their solid form, one mole of a gas does not weigh the same as its solid state!

34. The Volume of a Mole of Gas
Example:
If the density of a gas is 2.3 g/L, what is its molar mass?
2.3 𝑔 1 𝐿 𝐿 1 𝑚𝑜𝑙 =51.52 𝑔/𝑚𝑜𝑙

35. The Volume of a Mole of Gas
Example:
What is the density of F2 at STP?

36. The Volume of a Mole of Gas Practice Problems
17. Since we know that the gaseous state of a substance does not have the same mass as the solid state of the same substance, what can we say about the density of the two?

37. The Volume of a Mole of Gas Practice Problems
18. How many moles are in 22.4 Liters of O(gas)?

38. The Volume of a Mole of Gas Practice Problems
19. How many milliliters of Neon gas are in 2 mols?

39. The Volume of a Mole of Gas Practice Problems
20. What is the molar mass of a gas that has a density of g/L? Which diatomic gas do you think it is?

40. The Volume of a Mole of Gas Practice Problems
21. What is the density of Cl2 at STP?

41. 22.4 g/L
Molar
Mass
Volume
Avogadro’s number
Moles
Atoms

42. Mole Conversion Practice Problems
22. How many moles in 9.0 liters of a gas at STP?

43. Mole Conversion Practice Problems
23. How many moles in 15 g of NaOH?

44. Mole Conversion Practice Problems
24. How many liters would 2.9 moles of CO2 occupy at STP?

45. Mole Conversion Practice Problems
25. How many grams would 30 L of CO2 gas weigh?

46. Mole Conversion Practice Problems
26. How many atoms are in 50 L of H2 gas?

47. Calculating Percent Composition
Percent Composition is the percent by mass of each element in a compound. You find the percent composition by dividing the mass of the element by the total mass of the molecule.
If you think back to the separation lab we have done this already by calculating the % of salt, % of sand, and % of iron!!

48. Calculating Percent Composition
Example:
How many students are in this class? Find the percentage of Males and the percentage of Females.

49. Calculating Percent Composition
Example:
What percentage of students in the class are 15? 16? 17?

50. Calculating Percent Composition
Example:
What is the percent composition of each element in C6H12O6?

51. Calculating Percent Composition
Example:
What is the percent by mass of each element in H2O?

52. Calculating Percent Composition
Example:
How many grams of nitrogen are in 59 g of AgNO3?

53. Percent Composition Practice Problems
27. Which compound has the smallest percentage of Chlorine?
HCl
KCl
LiCl
NaCl

54. Percent Composition Practice Problems
28. Of the following compounds, which does Strontium have the highest percent composition?
SrCl2
SrI2
SrO
SrS

55. Percent Composition Practice Problems
29. What is the percent composition of Oxygen in the compound propanal (CH3CH2CHO)?

56. Percent Composition Practice Problems
30.  What is the percent by mass of Oxygen in H2SO4?

57. Percent Composition Practice Problems
31. What is the total mass of oxygen in 1.00 mol of Al2(CrO4)3?

58. Percent Composition Practice Problems
32. What is the percent composition of Carbon in CO?

59. Calculation Empirical Formulas
An empirical formula is the lowest whole number ratio of the atoms of the elements in a compound. The empirical formula may or may not be the same as the molecular formula.

60. Calculation Empirical Formulas
Example:
The molecular formula for CO2 is the same as the empirical formula for CO2 because the atoms are in the lowest whole number ratio.

61. Calculation Empirical Formulas
Example:
The molecular formula for C2H2, could be that, or it could be C6H6. But the empirical formula for both is CH, since that is the lowest whole number ratio.

62. Calculation Empirical Formulas
It is important to understand that the empirical formula gives you an idea of the ratio of between elements within a compound.

63. Calculation Empirical Formulas
Example:
Calculate the empirical formula of a compound made up of:
32.00% C
42.66% O
18.67 % N
6.67% H

64. Calculation Empirical Formulas Practice Problems
33. A compound contains 40% calcium, 12% carbon, 48% oxygen by mass. What is the empirical formula for this compound?

65. Calculation Empirical Formulas Practice Problems
34. Write the empirical formula for the following compound: P4O10

66. Calculation Empirical Formulas Practice Problems
35. A compound is 86% carbon and 14% hydrogen by mass. What is the empirical formula for the compound?

67. Calculation Empirical Formulas Practice Problems
36. Which of the following is an empirical compound?
C4H10
C6H12O6
P2O5
C2H2O2

68. Calculation Empirical Formulas Practice Problems
37. A compound was analyzed and was found to contain 75% carbon and 25% hydrogen by mass. What is the compounds empirical formula?

69. Calculation Empirical Formulas Practice Problems
38. What is the simplest ration of nitrogen to oxygen in the compound nitrogen (IV) oxide

70. Calculation Molecular Formulas
Knowing that the Molecular formula of a substance is not always equal to the Empirical Formula of the substance, what can we say about Molecular Weight vs Empirical Formula Weight?

71. Calculation Molecular Formulas
We can determine the molecular formula we first know the molar mass and the empirical formula of the substance. We then compare the molar mass to the Empirical Formula Weight to determine the ratio.

72. Calculation Molecular Formulas
Examples:
 The molar mass of a substance is 60g and its empirical formula is CH4N. Find the Molecular Formula.

73. Calculation Molecular Formulas
Examples:
The molar mass of a substance is 78g and its empirical formula is CH. Find the Molecular Formula.

74. Calculation Molecular Formulas
Examples:
Find the molecular formula for a compound that has:
54.5% C
13.6% H
31.8 % N
molar mass = 88g

75. Calculation Molecular Formulas Practice Problems
39. What’s the molecular formula of a compound given the empirical formula P2O5 and molar mass 284 g?

76. Calculation Molecular Formulas Practice Problems
41. What is the molecular formula of a compound that has a molecular mass of 42 g and empirical formula of CH2?

77. Calculation Molecular Formulas Practice Problems
42. Find the molecular formula for a compound that has:
54.5% C
13.6% O
31.8 % N
molar mass = 176 g/mol

78. Calculation Molecular Formulas Practice Problems
43. Find the molecular formula for a compound that has:
25.9% N
74.1% H
molar mass = 108 g/mol

79. Calculation Molecular Formulas Practice Problems
44. Find the molecular formula for a compound that has:
22.8 g Ba
2.00 g C
8.00 g O
molar mass = g/mol

80. Hydrates
Hydrated compounds have water molecules attached to them. CuSO45H2O is copper (II) sulfate pentahydrate. For every formula unit of CuSO4, there are 5 water molecules attached to it. There are always numerous waters for one salt.

81. Hydrates
Example:
Start with 1.54 g wet magnesium phosphate. Dry it so that there are only 1.28 g residue left. Find the formula of the hydrate.

82. Hydrates
Example:
Calculate the percent composition in NaCl ∙ 5H2O?

83. Hydrates Practice Problems
45. Calculate the percent composition in BaCl2 ∙ 2H2O

84. Hydrates Practice Problems
46. What is the percent by mass of the water in the hydrate
Na2CO3 ∙ 10H2O?

85. Hydrates Practice Problems
47. If you start with 1.54 g wet magnesium phosphate. Dry it so that there are only 1.02 g residue left. Find the formula of the hydrate.

86. Hydrates Practice Problems
48. Start with 1.62 g of hydrated cobalt (II) chloride. After heating, there are 0.88 g of solid reside. Find the formula of the hydrate.