chapter10 section01 by hamdy karim

of 43

Chemistry10.1

© Copyright Pearson Prentice Hall

Slide 2 of 43

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



>

Slide 3 of 43

Measuring Matter

Measuring Matter

What are three methods for measuring the amount of something?

10.1

of 43



> 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

Slide 5 of 43

10.1


SAMPLE PROBLEM

Slide 6 of 43

10.1


SAMPLE PROBLEM

Slide 7 of 43

10.1


SAMPLE PROBLEM

Slide 8 of 43

10.1


Slide 9 of 43

Practice Problems for Sample Problem 10.1

Problem Solving 10.1 Solve Problem 1 with the help of an interactive guided tutorial.



>

Slide 10 of 43

What is a Mole?

What Is a Mole?

How is Avogadro’s number related to a mole of any substance?

10.1

of 43



> 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

of 43



> 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

of 43



> What is a Mole?10.1


SAMPLE PROBLEM

Slide 14 of 43

10.2


SAMPLE PROBLEM

Slide 15 of 43

10.2


SAMPLE PROBLEM

Slide 16 of 43

10.2


SAMPLE PROBLEM

Slide 17 of 43

10.2


Slide 18 of 43



of 43



> What is a Mole?

Converting Moles to Number of Particles

10.1


SAMPLE PROBLEM

Slide 20 of 43

10.3


SAMPLE PROBLEM

Slide 21 of 43

10.3


SAMPLE PROBLEM

Slide 22 of 43

10.3


SAMPLE PROBLEM

Slide 23 of 43

10.3


Slide 24 of 43





>

Slide 25 of 43

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

of 43



> 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

of 43




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

10.1


Slide 28 of 43


> Animation 11

Animation 11

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

of 43




10.1



>

Slide 30 of 43

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


Slide 31 of 43


> 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

of 43




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

10.1

of 43




Molar Masses of Glucose, Water, and Paradichlorobenzene

10.1


SAMPLE PROBLEM

Slide 34 of 43

10.4


SAMPLE PROBLEM

Slide 35 of 43

10.4


SAMPLE PROBLEM

Slide 36 of 43

10.4


SAMPLE PROBLEM

Slide 37 of 43

10.4


Slide 38 of 43




Slide 39 of 43

Section Quiz

-or-Continue to: Launch:

Assess students’ understanding of the concepts in Section

10.1 Section Quiz.

10.1.


Slide 40 of 43

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.


Slide 41 of 43

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.


Slide 42 of 43

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.


Slide 43 of 43

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

END OF SHOW

chapter10 section01 by hamdy karim

Education

measurement of matter

mole mol

measuring matter

molar mass of carbon

atomic mass units

number of particles

number of grams

practice problems