Transcript chemistry - Canisteo-Greenwood Central School

chemistry
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10.2
Mole–Mass and Mole–Volume
Relationships
How can you guess the number of
jelly beans in a jar? You estimate
the size of a jelly bean and then
estimate the dimensions of the
container to obtain its volume. In a
similar way, chemists use the
relationships between the mole and
quantities such as mass, volume,
and number of particles to solve
chemistry problems.
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10.2
Mole–Mass and Mole–
Volume Relationships
>
The Mole–Mass Relationship
The Mole–Mass Relationship
How do you convert the mass of a
substance to the number of moles of the
substance?
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10.2
Mole–Mass and Mole–
Volume Relationships
>
The Mole–Mass Relationship
Use the molar mass of an element or
compound to convert between the mass
of a substance and the moles of a
substance.
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SAMPLE PROBLEM 10.5
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SAMPLE PROBLEM 10.5
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SAMPLE PROBLEM 10.5
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SAMPLE PROBLEM 10.5
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Practice Problems for Sample Problem 10.5
Problem Solving 10.16 Solve
Problem 16 with the help of an
interactive guided tutorial.
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SAMPLE PROBLEM 10.6
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SAMPLE PROBLEM 10.6
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SAMPLE PROBLEM 10.6
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SAMPLE PROBLEM 10.6
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Practice Problems for Sample Problem 10.6
Problem Solving 10.18 Solve
Problem 18 with the help of an
interactive guided tutorial.
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10.2
Mole–Mass and Mole–
Volume Relationships
>
The Mole–Volume Relationship
The Mole–Volume Relationship
What is the volume of a gas at STP?
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10.2
Mole–Mass and Mole–
Volume Relationships
>
The Mole–Volume Relationship
Avogadro’s hypothesis states that equal volumes
of gases at the same temperature and pressure
contain equal numbers of particles.
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10.2
Mole–Mass and Mole–
Volume Relationships
>
The Mole–Volume Relationship
The volume of a gas varies with temperature
and pressure. Because of these variations, the
volume of a gas is usually measured at a
standard temperature and pressure.
Standard temperature and pressure (STP)
means a temperature of 0°C and a pressure of
101.3 kPa, or 1 atmosphere (atm).
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10.2
Mole–Mass and Mole–
Volume Relationships
>
The Mole–Volume Relationship
At STP, 1 mol or, 6.02  1023 representative
particles, of any gas occupies a volume of
22.4 L.
The quantity 22.4 L is called the molar
volume of a gas.
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10.2
Mole–Mass and Mole–
Volume Relationships
>
The Mole–Volume Relationship
Calculating Volume at STP
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SAMPLE PROBLEM 10.7
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SAMPLE PROBLEM 10.7
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SAMPLE PROBLEM 10.7
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SAMPLE PROBLEM 10.7
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Practice Problems for Sample Problem 10.7
Problem Solving 10.20 Solve
Problem 20 with the help of an
interactive guided tutorial.
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10.2
Mole–Mass and Mole–
Volume Relationships
>
The Mole–Volume Relationship
Calculating Molar Mass from Density
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SAMPLE PROBLEM 10.8
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SAMPLE PROBLEM 10.8
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SAMPLE PROBLEM 10.8
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SAMPLE PROBLEM 10.8
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Practice Problems for Sample Problem 10.8
Problem Solving 10.22 Solve
Problem 22 with the help of an
interactive guided tutorial.
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10.2
Mole–Mass and Mole–
Volume Relationships
>
The Mole Road Map
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10.2
Mole–Mass and Mole–
Volume Relationships
>
The Mole Road Map
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10.2
Mole–Mass and Mole–
Volume Relationships
>
The Mole Road Map
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10.2
Mole–Mass and Mole–
Volume Relationships
>
The Mole Road Map
The Mole Road Map
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Mole–Mass and Mole–
Volume Relationships
>
Simulation 10
Simulation 10
Use the mole road map to convert among
mass, volume, and number of representative
particles.
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10.2 Section Quiz.
Assess students’ understanding
of the concepts in Section 10.2.
Continue to:
-or-
Launch:
Section Quiz
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10.2 Section Quiz.
1. Calculate the mass in grams of a sample
containing 1.85 x 1034 molecules of water.
a. 3.07 x 1010 g
b. 5.53 x 1011 g
c. 188 g
d. 8.46 x 103 g
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10.2 Section Quiz.
2. Calculate the number of moles in a spoonful
of table sugar (C12H22O11) having a mass of
10.5 g.
a. 32.6 mol
b. 3.59  103 mol
c. 3.07  10–3 mol
d. 1.85  1022 mol
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10.2 Section Quiz.
3. What is the volume of 0.35 mol of oxygen gas
at STP?
a. 32 L
b. 64 L
c. 7.8 L
d. 16 L
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END OF SHOW