Stoichiometry

1
Stoichiometry

• Study of mass and chemical amounts.
• 1. Compound stoichiometry
• 2. Reaction stoichiometry

2
Connecting the Macro and Atomic Scales The Mole

• Chemical macroscopic counting unit
• 1 mole contains 6.022 x 1023 particles
• 6.022 x 1023 is Avogadros number, named after
• Amedeo Avogadro.
• Avogadros number is not special, like pi, but is
  invented by us for our convenience.

3
Why it works.

• The mass of 1 mol of an element is equal to its
  atomic mass in grams
• Molar mass is in g/mol
• Molar mass of Al 26.98 g/mol
• Unit sign mole mol sometimes,
  molar mass M

4
How it works

• Two new conversion factors
• Avogadros number
• Molar mass

5
How many atoms are in 2.60 mol of Ne?
6
How many atoms are in 3.84 mol of B?

1. 3.84
2. 2.31 x 1025
3. 2.31 x 1024
4. 6.38 x 10-24

7
How many moles do 4.00 x 1022 atoms of Ne make?
8
How many moles do 6.84 x 1021 atoms of B make?

1. 6.84 x 1021 mol
2. 0.0114 mol
3. 4.12 x 1045 mol
4. 6.84 x 10-21 mol

9
How many moles do 45.0 g of Ne make?
10
How many moles do 45.0 g of Al make?

1. 1.67 mol
2. 1214 mol
3. 7.47 x 10-23 mol
4. 2.71 x 1025 mol

11
What is the mass of 2.60 mol of C?
12
What is the mass of 2.60 mol of O?

1. 8.90 g
2. 0.163 g
3. 2.60 g
4. 41.6 g

13
How many moles are represented by 1.00 g of C?
14
How many atoms are in 1.00 g of O?
15
What is the mass of one Au atom?
16
How many C atoms are in a 1.00 caret diamond?
17
Compounds and Moles

• 1 mole of a compound contains 6.022 x 1023
  molecules or units
• Molar mass sum of atomic molar masses
• H2O
• CO2
• Fe(NO3)3

18
(No Transcript)
19
Molecules, Atoms and Moles

• Consider UF6
• 0.50 mol UF6 contains

20
Language for nonmolecular compounds

• 1 mol CO2 contains 6.022 x 1023 molecules
• 1 mol NaCl contains 6.022 x 1023 formula units

21
(No Transcript)
22
Percent Composition
What fraction of a compound is made up of one of
its elements? Consider FeO2 ( added the
2)
23
(No Transcript)
24
Determining Formulas from Percent Composition

• The key the ratio of atoms in the formula is the
  same as the ratio of moles of those elements

25
Determining Formulas from Percent Composition

• The key the ratio of atoms in the formula is the
  same as the ratio of moles of those elements
• If you determine the ratio of moles, you know the
  formula.

26
Determining Formulas from Percent Composition

• The key the ratio of atoms in the formula is the
  same as the ratio of moles of those elements
• If you determine the ratio of moles, you know the
  formula.
• But! You get the empirical formula.

27
Example
A compound has Ca, S, and O. Ca 29.45 S 23.
55 O 47.00 What is the empirical formula?
28
Example 20.48 Zn 79.51 I
29
Example
A compound has Ca, S, and O. Ca 29.45 S 23.
55 O 47.00 What is the empirical formula?
30
Empirical vs. Molecular Formulas
Example Ethene is C2H4 Percent composition
tells us mol H/mol C 2 The empirical formula
is CH2. The molecular formula is C2H4.
31
Example A hydrocarbon has 82.65 C and 17.34
H ----Molar mass is 58.12 g/mol ----What are the
empirical and molecular formulas?
32
(No Transcript)
33
Hydrated Compounds

• Solids in which molecules of water are trapped
  and become part of the compound.
• Ex Gypsum CaSO4 2H2O
• is hydrated calcium sulfate
• CaSO4 is anhydrous calcium sulfate

34
Determining the number of waters of hydration

• 1.023 g CuSO4 x H2O is heated to drive off the
  water. The resulting anhydrous CuSO4 has a mass
  of 0.654 g.
• What is the value of x?

35
(No Transcript)