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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
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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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The Mole: A Measurement of 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
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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.
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The Mole: A Measurement of 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?
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The Mole: A Measurement of 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.
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The Mole: A Measurement of 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.
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The Mole: A Measurement of Matter
> What is a Mole?10.1
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Practice Problems for Sample Problem 10.2
Problem Solving 10.4 Solve Problem 4 with the help of an interactive guided tutorial.
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The Mole: A Measurement of Matter
> What is a Mole?
Converting Moles to Number of Particles
10.1
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Practice Problems for Sample Problem 10.3
Problem Solving 10.5 Solve Problem 5 with the help of an interactive guided tutorial.
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The Mole: A Measurement of 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?
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The Mole: A Measurement of 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.
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The Mole: A Measurement of Matter
> The Mass of a Mole of an Element
One molar mass of carbon, sulfur, mercury, and iron are shown.
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The Mole: A Measurement of 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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The Mole: A Measurement of Matter
> The Mass of a Mole of an Element
10.1
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The Mole: A Measurement of 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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The Mole: A Measurement of 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.
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The Mole: A Measurement of Matter
> The Mass of a Mole of a Compound
Substitute the unit grams for atomic mass units. Thus 1 mol of SO3 has a mass of 80.1 g.
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The Mole: A Measurement of Matter
> The Mass of a Mole of a Compound
Molar Masses of Glucose, Water, and Paradichlorobenzene
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Practice Problems for Sample Problem 10.4
Problem Solving 10.7 Solve Problem 7 with the help of an interactive guided tutorial.
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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