chapter10 section02 mole–mass and mole–volume relationships by hamdy karim

of 39

chemistry

© Copyright Pearson Prentice Hall

Slide 2 of 39

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



>

Slide 3 of 39

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

of 39



> 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

Slide 5 of 39

10.5


SAMPLE PROBLEM

Slide 6 of 39

10.5


SAMPLE PROBLEM

Slide 7 of 39

10.5


SAMPLE PROBLEM

Slide 8 of 39

10.5


Slide 9 of 39

Practice Problems for Sample Problem 10.5

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


SAMPLE PROBLEM

Slide 10 of 39

10.6


SAMPLE PROBLEM

Slide 11 of 39

10.6


SAMPLE PROBLEM

Slide 12 of 39

10.6


SAMPLE PROBLEM

Slide 13 of 39

10.6


Slide 14 of 39





>

Slide 15 of 39

The Mole–Volume Relationship

The Mole–Volume Relationship

What is the volume of a gas at STP?

10.2

of 39



> 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

of 39




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

of 39




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

of 39




Calculating Volume at STP

10.2


SAMPLE PROBLEM

Slide 20 of 39

10.7


SAMPLE PROBLEM

Slide 21 of 39

10.7


SAMPLE PROBLEM

Slide 22 of 39

10.7


SAMPLE PROBLEM

Slide 23 of 39

10.7


Slide 24 of 39



of 39




Calculating Molar Mass from Density

10.2


SAMPLE PROBLEM

Slide 26 of 39

10.8


SAMPLE PROBLEM

Slide 27 of 39

10.8


SAMPLE PROBLEM

Slide 28 of 39

10.8


SAMPLE PROBLEM

Slide 29 of 39

10.8


Slide 30 of 39




Slide 31 of 39


> The Mole Road Map10.2


Slide 32 of 39




Slide 33 of 39




Slide 34 of 39


> The Mole Road Map

The Mole Road Map

10.2


Slide 35 of 39


> Simulation 10

Simulation 10

Use the mole road map to convert among mass, volume, and number of representative particles.


Slide 36 of 39

Section Quiz

-or-Continue to: Launch:

Assess students’ understanding of the concepts in Section

10.2 Section Quiz.

10.2.


Slide 37 of 39

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


Slide 38 of 39

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


Slide 39 of 39

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

END OF SHOW

chapter10 section02 mole–mass and mole–volume relationships by hamdy karim

Education

interactive guided tutorial

mole road map

mole road map10

39 practice problems

molevolume relationship

2 section quiz

sample problem 10

standard temperature