chapter 10: chemical quantities (topic pre-viewed in lab) activities in-class workshops calculation...

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Chapter 10: Chemical Quantities (Topic pre-viewed in lab) Activities •In-class workshops calculation of molar mass (gram-formula mass) •Open-notes evaluations •Quizes and tests •Homework •Lab activities Mole ratios lab – Qualitative Lab 5 Mole labs – Quantitative Labs 6 , 8, 9 Na 2 CO 3 + CaCl 2 yields CaCO 3 and 2 NaCl NaHCO 3 and HCl yields CO 2 + H 2 O + NaCl Percent composition of water in a hydrate The mole: A measurement of matter TB section 10.1 Mole-Mass and Mole- Volume relationships: TB section 10.2 Percent Composition and Chemical Formula TB section10.3

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Chapter 10: Chemical Quantities (Topic pre-viewed in lab)

Activities

•In-class workshops calculation of molar mass (gram-formula mass)

•Open-notes evaluations

•Quizes and tests

•Homework

•Lab activitiesMole ratios lab – Qualitative Lab 5

Mole labs – Quantitative Labs 6 , 8, 9

Na2CO3 + CaCl2 yields CaCO3 and 2 NaCl

NaHCO3 and HCl yields CO2 + H2O + NaCl

Percent composition of water in a hydrate

The mole: A measurement of matter

TB section 10.1

Mole-Mass and Mole-Volume relationships:

TB section 10.2

Percent Composition and Chemical Formula

TB section10.3

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© Copyright Pearson Prentice Hall

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 term representative particle refers to the species present in a substance: usually atoms, molecules, or formula units.

The number of representative particles in a mole, 6.02 1023, is called Avogadro’s number.

10.1

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© Copyright Pearson Prentice Hall

The Mole: A Measurement of Matter

> What is a Mole?10.1

© Copyright Pearson Prentice Hall

SAMPLE PROBLEM

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10.2

© Copyright Pearson Prentice Hall

SAMPLE PROBLEM

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10.2

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© Copyright Pearson Prentice Hall

The Mole: A Measurement of Matter

> What is a Mole?

Converting Moles to Number of Particles

10.1

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10.3

Read the question CAREFULLY. What do you need to find?

Hints:

(1)How many molecules of propane are in one mole of propane?

(2)How many atoms are there in one molecule of propane?

© Copyright Pearson Prentice Hall

SAMPLE PROBLEM

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10.3

© Copyright Pearson Prentice Hall

SAMPLE PROBLEM

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10.3

© Copyright Pearson Prentice Hall

SAMPLE PROBLEM

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10.3

© Copyright Pearson Prentice Hall

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Practice Problems for Sample Problem 10.3

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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 (use Periodic Table)

How is the atomic mass of an element related to the molar mass 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 (gram-formula mass).

10.1

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© Copyright Pearson Prentice Hall

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.

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?

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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© Copyright Pearson Prentice Hall

The Mole: A Measurement of Matter

> The Mass of a Mole of a Compound

One SO3 molecule has a mass of 80.1 amu. Substitute the unit grams for atomic mass units. Thus 1 mol of SO3 has a mass of 80.1 g. One mole of SO3 molecules has a mass of 80.1 grams

10.1

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© Copyright Pearson Prentice Hall

The Mole: A Measurement of Matter

> The Mass of a Mole of a Compound

Molar Masses of Glucose, Water, and Paradichlorobenzene

10.1

© Copyright Pearson Prentice Hall

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.

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.

© Copyright Pearson Prentice Hall

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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