The%20Mole

1
The Mole

• Chap. 11

No, not that mole!
2

1. Counting Particles

3

1. Counting Particles

1. There are common units to count things

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1. Counting Particles

1. There are common units to count things

1. Pair

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1. Counting Particles

1. There are common units to count things

1. Pair 2
2. Dozen

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1. Counting Particles

1. There are common units to count things

1. Pair 2
2. Dozen 12
3. Ream

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1. Counting Particles

1. There are common units to count things

1. Pair 2
2. Dozen 12
3. Ream 500 sheets
4. Gross

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1. Counting Particles

1. There are common units to count things

1. Pair 2
2. Dozen 12
3. Ream 500
4. Gross 144
5. Scop (not really)

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1. Counting Particles

1. There are common units to count things

1. Pair 2
2. Dozen 12
3. Ream 500
4. Gross 144
5. Scop (not really) 64
6. Mole

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1. Counting Particles

1. There are common units to count things

1. Pair 2
2. Dozen 12
3. Ream 500
4. Gross 144
5. Scop (not really) 64
6. Mole Avogadros

11
Avogadros number
A value equal to 6.0221367 x 1023.
Well round it to 6.02 x 1023
12

1. Counting Particles

1. Converting with moles

1. Finding the number of particles from moles.

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Self Check Ex. 1
How many atoms are in 2 moles of helium?
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Self Check Ex. 2
How many molecules are in 7.5 moles of carbon
dioxide?
15

1. Counting Particles

1. Converting with moles

1. Finding the number of particles from moles.
2. Finding the number of moles from particles.

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Self Check Ex. 3
A sample of lead contains 1.5 x 1024 atoms. How
many moles of lead atoms are there?
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Self Check Ex. 4
A sample of zinc chloride contains 2.150 x 1018
formula units. How many moles of zinc chloride
are there?
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1. Massing a Mole

1. Different atoms have different masses.

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1 atom of carbon would weigh ____ times more than
1 atom of helium.
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dozen atoms
1 atom of carbon would weigh ____ times more than
1 atom of helium.
3
dozen atoms
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mole of
1 atom of carbon would weigh ____ times more than
1 atom of helium.
3
mole of
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1. Massing a Mole

1. Different atoms have different masses.
2. The mass on the P.T. represents. . .

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1. Massing a Mole

1. Different atoms have different masses.
2. The mass on the P.T. represents. . .

1. The mass of 1 atom (in amu)

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1. Massing a Mole

1. Different atoms have different masses.
2. The mass on the P.T. represents. . .

1. The mass of 1 atom (in amu)
2. The mass of 1 mole of atoms (in grams)

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1. Massing a Mole

1. Different atoms have different masses.
2. The mass on the P.T. represents. . .
3. This value is called the molar mass.

The mass of 1 mole of particles
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If you weigh out 40 grams of argon you have
essentially counted ______________ atoms.
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If you weigh out 40 grams of argon you have
essentially counted ______________ atoms.
6.02 x 1023
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1. Massing a Mole

1. Calculating with molar mass

1. Using molar mass you can convert from
   to .

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1. Massing a Mole

1. Calculating with molar mass

1. Using molar mass you can convert from grams to
   moles.

30
Self Check Ex. 5
If a sample of aluminum has a mass 81.0 g how
many moles are present?
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1. Massing a Mole

1. Calculating with molar mass

1. Using molar mass you can convert from grams to
   moles.
2. You can also convert from _____ to .

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1. Massing a Mole

1. Calculating with molar mass

1. Using molar mass you can convert from grams to
   moles.
2. You can also convert from moles to grams.

33
Self Check Ex. 6
What is the mass of 0.25 moles of chromium?
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1. Massing a Mole

1. Calculating with molar mass
2. Calculating the molar mass of compound

35
Example
One mole of CH4 contains
1 mole of carbon
moles of hydrogen
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Example
One mole of CH4 contains
1 mole of carbon
4 moles of hydrogen
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Example
One mole of CH4 contains
1 mole of carbon
4 moles of hydrogen
weighs 12 g
weighs ______
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Example
One mole of CH4 contains
1 mole of carbon
4 moles of hydrogen
weighs 12 g
weighs 4 x (1) g
39
Example
One mole of CH4 contains
1 mole of carbon
4 moles of hydrogen
weighs 12 g
weighs 4 x (1) g
16 g/mol
40

1. Massing a Mole

1. Calculating with molar mass
2. Calculating the molar mass of compound

1. Add the masses of each of the atoms in the
   compound.

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1. Massing a Mole

1. Calculating with molar mass
2. Calculating the molar mass of compound

1. Add the masses of each of the atoms in the
   compound.
2. Remember to multiply each atoms mass by the
   number atoms in the compound.

42
Self Check Ex. 7
What is the molar mass of lithium nitrate, LiNO3?
43
Self Check Ex. 8
What is the molar mass of calcium acetate,
Ca(C2H3O2)2?
44

1. Molar Volume of Gas

The volume of 1 mole of gas particles when
measured at STP
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1. Molar Volume of Gas

1. This is determined at specific conditions.

STP standard temperature (0ºC) and standard
pressure (1 atm)
46

1. Molar Volume of Gas

1. This is determined at specific conditions.
2. Its the same for all gases.

1 mole of gas at STP 22.4 L
47

1. Molar Volume of Gas

1. This is determined at specific conditions.
2. Its the same for all gases.
3. Conversions

48
Self Check Ex. 9
What is the volume of 3 moles of carbon dioxide
gas at STP?
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Self Check Ex. 10
How many moles of air are in a 64 L that is at 1
atm and 0ºC.
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1. Multiple step conversions

Just remember the mole is the central unit
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Mass (grams)
Volume (liters)
MOLE
particles (atoms, molecules, formula units)
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Self Check Ex. 11
What is the mass of 11.2 L of carbon dioxide gas?
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Self Check Ex. 12
How many molecules of ammonia, NH3 are in a 68-g
sample?
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1. Mole ratios in chemical formulas

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1. Mole ratios in chemical formulas

1. The subscripts can give a ratio of atoms in a
   compound.

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1 mole of ammonia, NH3
1 mole of N
mole of N
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1 mole of ammonia, NH3
1 mole of N
3 mole of N
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1 mole of ammonia, NH3
1 mole of N
3 mole of N
1 mole NH3 1 mole N
1 mole NH3 3 mole H
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1 mole of ammonia, NH3
1 mole of N
3 mole of N
1 mole NH3 1 mole N
1 mole NH3 3 mole H
1 mole NH3
1 mole NH3
1 mole N
1 mole N
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1. Mole ratios in chemical formulas

1. The subscripts can give a ratio of atoms in a
   compound.
2. Conversions

61
Self Check Ex. 13
How many moles of hydroxide ions are in 1.2 moles
of magnesium hydroxide, Mg(OH)2?
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Self Check Ex. 14
What is the mass of the oxygen atoms in 4 moles
of sodium sulfate?
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The end.