Chapter10 section01 By Hamdy Karim

© Copyright Pearson Prentice Hall
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The Mole: A Measurement of Matter
You could measure the amount
of sand in a sand sculpture by
counting each grain of sand,
but it would be much easier to
weigh the sand. You’ll discover
how chemists measure the
amount of a substance using a
unit called a mole, which
relates the number of particles
to the mass.
10.1

The Mole: A Measurement of
Matter
>
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Measuring Matter
Measuring Matter
What are three methods for measuring
the amount of something?
10.1

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Matter
> Measuring Matter
You often measure the amount of
something by one of three different
methods—by count, by mass, and by
volume.
10.1

SAMPLE PROBLEM
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10.1

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Practice Problems for Sample Problem 10.1
Problem Solving 10.1 Solve
Problem 1 with the help of an
interactive guided tutorial.

Matter
>
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What is a Mole?
What Is a Mole?
How is Avogadro’s number related to a
mole of any substance?
10.1

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Matter
> What is a Mole?
A mole of any substance contains
Avogadro’s number of representative
particles, or 6.02  1023 representative
particles.
The term representative particle refers to
the species present in a substance: usually
atoms, molecules, or formula units.
10.1

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Matter
> What is a Mole?
Converting Number of Particles to Moles
One mole (mol) of a substance is 6.02  1023
representative particles of that substance and is
the SI unit for measuring the amount of a
substance.
The number of representative particles in a
mole, 6.02  1023, is called Avogadro’s number.
10.1

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Matter
> What is a Mole?10.1

SAMPLE PROBLEM
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10.2

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Matter
> What is a Mole?
Converting Moles to Number of Particles
10.1

SAMPLE PROBLEM
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10.3

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Matter
>
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The Mass of a Mole of an
Element
The Mass of a Mole of an Element
How is the atomic mass of an element
related to the molar mass of an
element?
10.1

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Matter
> The Mass of a Mole of an
Element
The atomic mass of an element
expressed in grams is the mass of a mole
of the element.
The mass of a mole of an element is its
molar mass.
10.1

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Matter
Element
One molar mass of carbon, sulfur, mercury, and
iron are shown.
10.1

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Matter
> Animation 11
Animation 11
Find out how Avogadro’s number is based on
the relationship between the amu and the
gram.

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Matter
Element
10.1

Matter
>
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The Mass of a Mole of a
Compound
The Mass of a Mole of a Compound
How is the mass of a mole of a
compound calculated?
10.1

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Matter
> The Mass of a Mole of a
Compound
To calculate the molar mass of a
compound, find the number of grams of
each element in one mole of the
compound. Then add the masses of the
elements in the compound.
10.1

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Matter
Compound
Substitute the unit grams for atomic mass units.
Thus 1 mol of SO3 has a mass of 80.1 g.
10.1

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Matter
Compound
Molar Masses of Glucose, Water, and
Paradichlorobenzene
10.1

SAMPLE PROBLEM
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10.4

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Section Quiz
-or-
Continue to: Launch:
Assess students’ understanding
of the concepts in Section
10.1 Section Quiz.
10.1.

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10.1 Section Quiz.
1. Three common ways of measuring the amount
of something are by count, by mass, and
a. by temperature.
b. by volume.
c. by area.
d. by density.

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10.1 Section Quiz.
2. A mole of hydrogen gas, H2(g), contains 6.02
x 1023
a. molecules.
b. atoms.
c. amu.
d. grams.

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10.1 Section Quiz.
3. The atomic mass of fluorine is 19.0 amu, so
the molar mass is
a. 19.0 amu.
b. 19.0 g.
c. 6.02 x 1023 amu.
d. 6.02 x 1023 g.

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10.1 Section Quiz.
4. Calculate the molar mass of ammonium nitrate.
a. 45.02 g
b. 80.05 g
c. 60.06 g
d. 48.05 g

Chapter10 section01 By Hamdy Karim

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Chapter10 section01 By Hamdy Karim