Mole–Mass and Mole–Volume Relationships

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Mole–Mass and Mole–Volume Relationships

How can you guess the number of jelly beans in a jar? You estimate the size of a jelly bean and then estimate the dimensions of the container to obtain its volume. In a similar way, chemists use the relationships between the mole and quantities such as mass, volume, and number of particles to solve chemistry problems.

10.2



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The Mole–Mass Relationship

The Mole–Mass Relationship

How do you convert the mass of a substance to the number of moles of the substance?

10.2

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> The Mole–Mass Relationship

Use the molar mass of an element or compound to convert between the mass of a substance and the moles of a substance.

10.2


SAMPLE PROBLEM

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10.5


SAMPLE PROBLEM

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10.5


SAMPLE PROBLEM

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10.5


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Practice Problems for Sample Problem 10.5

Problem Solving 10.16 Solve Problem 16 with the help of an interactive guided tutorial.


SAMPLE PROBLEM

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10.6


SAMPLE PROBLEM

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10.6


SAMPLE PROBLEM

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10.6


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The Mole–Volume Relationship

The Mole–Volume Relationship

What is the volume of a gas at STP?

10.2

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> The Mole–Volume Relationship

Avogadro’s hypothesis states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles.

10.2

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The volume of a gas varies with temperature and pressure. Because of these variations, the volume of a gas is usually measured at a standard temperature and pressure.

Standard temperature and pressure (STP) means a temperature of 0°C and a pressure of 101.3 kPa, or 1 atmosphere (atm).

10.2

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At STP, 1 mol or, 6.02 1023 representative particles, of any gas occupies a volume of 22.4 L.

The quantity 22.4 L is called the molar volume of a gas.

10.2

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Calculating Volume at STP

10.2


SAMPLE PROBLEM

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10.7


SAMPLE PROBLEM

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10.7


SAMPLE PROBLEM

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10.7


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Calculating Molar Mass from Density

10.2


SAMPLE PROBLEM

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10.8


SAMPLE PROBLEM

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10.8


SAMPLE PROBLEM

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10.8


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> The Mole Road Map10.2


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> The Mole Road Map

The Mole Road Map

10.2


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10.2 Section Quiz.

1. Calculate the mass in grams of a sample containing 1.85 x 1034 molecules of water.

a. 3.07 x 1010 g

b. 5.53 x 1011 g

c. 188 g

d. 8.46 x 103 g


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10.2 Section Quiz.

2. Calculate the number of moles in a spoonful of table sugar (C12H22O11) having a mass of 10.5 g.

a. 32.6 mol

b. 3.59 103 mol

c. 3.07 10–3 mol

d. 1.85 1022 mol


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10.2 Section Quiz.

3. What is the volume of 0.35 mol of oxygen gas at STP?

a. 32 L

b. 64 L

c. 7.8 L

d. 16 L

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Mole–Mass and Mole–Volume Relationships