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Chemistry10.1

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**The Mole: A Measurement of Matter**

10.1 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.

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**Measuring Matter Measuring Matter**

10.1 Measuring Matter Measuring Matter What are three methods for measuring the amount of something?

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10.1 Measuring Matter You often measure the amount of something by one of three different methods—by count, by mass, and by volume. You can buy items by different types of measurements, such as a count, a weight or mass, or a volume. Classifying Which of these common items are being sold by weight? By volume? By count?

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

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**Sample problem 10.1 Answer: 0.50 bushel x 1 dozen__ x 2.0kg__**

We are solving mass of 0.50 bushels of apples We know: 0.20 bushels = 1 dozen apples 1 dozen apples = 2.0 kg Answer: 0.50 bushel x 1 dozen__ x 2.0kg__ 0.20 bushel dozen = 5.0 kg

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10.1 What is a mole?

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**What is a Mole? What Is a Mole?**

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

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

10.1 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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10.1 What is a Mole?

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for Sample Problem 10.2 Sample problem 10.2 Problem Solving 10.4 Solve Problem 4 with the help of an interactive guided tutorial.

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

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**Sample problem 10.2 ? Moles is 2.17x1023 particles of Br**

We know 1 mole = 6.02x1023 Answer: 2.17x1023 X 1 mole = 0.360mol Br 6.02x1023

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for Sample Problem 10.3 Sample problem 10.3 Problem Solving 10.5 Solve Problem 5 with the help of an interactive guided tutorial.

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**Sample problem 10.3 We are looking for the # of atoms in 1.14 mol SO3**

We know there are 4 molecules in SO3 We know 1 mole of SO3 is 6.02x1023 moles Answer: 1.14 mol X 6.02x1023 mol X 4 atoms mol molecule = 2.75x1024

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**The Mass of a Mole of an Element**

10.1 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 Mass of a Mole of an Element**

10.1 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 Mass of a Mole of an Element**

10.1 The Mass of a Mole of an Element One molar mass of carbon, sulfur, mercury, and iron are shown. One molar mass of carbon, sulfur, mercury, and iron are shown. Each of the quantities contains one mole of the element. Applying Concepts How many atoms of each element are shown?

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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 Mass of a Mole of an Element**

10.1 The Mass of a Mole of an Element

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**The Mass of a Mole of a Compound**

10.1 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?

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**The Mass of a Mole of a Compound**

10.1 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 Mass of a Mole of a Compound**

10.1 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 Mass of a Mole of a Compound**

10.1 The Mass of a Mole of a Compound Molar Masses of Glucose, Water, and Paradichlorobenzene One molar mass is shown for each of three molecular compounds. Inferring How can you know that each sample contains Avogadro’s number of molecules?

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for Sample Problem 10.4 Problem Solving 10.7 Solve Problem 7 with the help of an interactive guided tutorial.

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END OF SHOW

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