libretto - unit 3 phasesofmatter - libretto regents …3+phasesofmatter+... · 11/9/10 1 54 10/18...

11/9/10

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54

10/18 Objective: SWBAT describe how vapor pressure

interacts with atmospheric pressure. Do Now: pg 21 question D – have answer out. . hw – pg 22 Questions

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56

Test/Quiz Review (hand back)

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Lab Write-‐up You know: •  Amount of heat given off by water •  Amount of heat needed to raise temp of ice

•  Figure out Hf Ice

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Unit 3: Phases of Matter Lesson 3: Gasses and Pressure 59

Why Balloons Float (and why they don’t)

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How does a gas behave? Kinetic Molecular Theory (KMT)-

Describes an “ideal” gas. We imagine how it would behave. It would have five properties: 1.  Be made of particles with negligible volume 2.  Particles move in random, straight-lines 3.  Completely elastic collisions 4.  No intermolecular attractive forces 5.  Speed of particles is directly proportional to

Kelvin temperature 60

10/20

Objective: SWBAT describe the relationship between vapor pressure and boiling. Do Now: Why do we use the idea of an ideal gas? HW – pg 23-24 Questions

61

Ideal is not Real Real gasses violate some/all of the KMT But-

Only when the particles are moving slow and are squeezed together.

Low Temperature & High Pressure =

62

When would this happen?

They all contain equal numbers of molecules!!!

Amedeo Avogadro (1776 – 1856)

Avogadro’s Hypothesis

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How can this be?!?

Equal numbers of gas par;cles occupy equal volumes of space under the same condi;ons of temperature and pressure.

Standard Temperature and Pressure (STP) Because things happen differently at different

temperatures and pressures (particularly for gasses), we have to set a standard reference point.

Standard Temperature: 0° C = 273 K

Standard Pressure: 1.000 atm = 101.3 kPa = 760 mmHg (torr)

These are in Reference Table A.

64

What is this “Pressure” of which we speak Pressure =

Force exerted over an area. Anything with mass can exert a force. This includes the atmosphere. Standard Pressure:

1 atmosphere of pressure (at sea level)= 14.7 pounds per square inch (psi).

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11/9/10

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Brief notes on Torr. Torr = millimeters of mercury (mmHg)

Refers to the column of mercury in a barometer.

760 torr = Standard pressure

66

Why do we use

mercury?

Evangelista Torricelli (1608 – 1647)

Pressure conversions 1.000 atm = 14.7 psi = 101.3 kPa = 760.0 mmHg

67

Convert 2.35 atm to kPa: Convert 1.234 kPa to atm:

Vapor Pressure When a liquid in a sealed container is at vapor-liquid

equilibrium, the vapor exerts a pressure (like any gas).

Stronger IMAF = Lower vapor pressure. Higher vapor pressure = faster rate of evaporation. Volatile=

Substances that evaporate quickly.

68 69

70

10/21 Objective: SWBAT compare the vapor pressures of three different substances. Do Now: How is altitude and atmospheric pressure related? HW – Test tomorrow; mole due Monday.

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72

Why do things boil? Boiling happens when the vapor pressure of a

liquid is greater than the atmospheric pressure the liquid is under.

Boiling Point =

Vapor pressure = atmospheric pressure.

73

How Can you increase vapor pressure?

Normal Boiling Point The boiling point of a liquid at Standard

Atmospheric Pressure. What happens to boiling point if atmospheric

pressure increases? Decreases?

74

Reference Table H

75

Reference Tables for Physical Setting/CHEMISTRY 3

Table HVapor Pressure of Four Liquids

0 25 50 75 100 125

200

150

100

50

0

Vapo

r P

ress

ure

(kP

a)

Temperature (!C)

101.3 kPa

propanone

ethanol

water

ethanoicacid

Problem: What is the vapor pressure of ___ at ___°C?

76

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Use Method A!

Problem: What is the boiling point of ___ at a pressure of ___kPa?

77

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Use Method B!

11/9/10

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Problem: What is the normal boiling point of ___?

78

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Use Method C!

79

80 81

82


Equal numbers of chemistry students, occupying equal volumes of classrooms do not possess equal numbers

of ques;ons....You?

Things To Do Now:

83

11/9/10

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10/22 Objective: Test Do Now: Fill out Blue side of scantron HW – MOLE DUE MONDAY – CLASS

VOTE 84

10/25 Objective: SWBAT describe how the pressures of individual gases in a mixture are determined. Do Now: Have your moles ready to present. HW – Pg. 25 and 26 Questions

85

Mole Vobng •  Each student will present their mole to the class

•  Explain the motivation behind your mole,

•  Leave the mole up front, once each student has presented ballots will be collected

86

Unit 3: Phases of Matter Lesson 4: Partial Pressure and Effusion

87

Passing Gases

Dalton’s Law of Parbal Pressures

NOT in your Reference Tables (memorize!)

88

Ptotal = PgasA + PgasB + PgasC + ...

John Dalton (1766 – 1844)

The total pressure exerted by a mixture of gasses is equal to the sum of the pressures exerted by each gas in the mixture.

Pracbce Helps Us Learn! 1) What is the total pressure of a mixture of O2 (g), N2 (g) and

NH3 (g) if the pressure of the O2 (g) is 20. kPa, N2 (g) is 60. kPa and the NH3 (g) is 15 kPa?

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2) A mixture of 1 mole of O2 and 2 moles of N2 exerts a pressure of 150. kPa. What is the partial pressure of each gas?

90

3) A mixture of 30.0% He and 70.0% Ar exerts a pressure of 150. kPa at 25oC. What is the partial pressure of each gas?

91

4) A sample of NH3 (g) is decomposed into its component elements. If the pressure of the nitrogen gas produced equals 40.0 kPa, what would the pressure of the hydrogen gas?

92

Graham’s Law of Effusion

The heavier the gas molecules,

The greater the gas density. Table S – Densities (and boiling

points) for most elements.

93

Thomas Graham (1805 – 1869)

Lighter gas molecules will spread out (effuse) faster than heavier gas molecules.

Mathemabcal Form of Graham’s Law

ALSO NOT in your Reference Tables! (ALSO MEMORIZE IT!)

94

The Kind of Thing You Need To Do: A closed container of a mixture of chlorine,

fluorine, neon and helium gases is opened so the gases can escape. Place the gases in order of increasing rate of effusion.

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What now?

John Dalton (1766 – 1844)

The total ques;ons asked by a class of chemistry students equals the sum of the ques;ons asked by each student in the class. Any Ques;ons?

10/26 Objective: SWBAT describe the relationships

that exist between volume, temperature, and pressure when studying gases.

Do Now: Take a stick…. (PTV) HW – Pg. 27 Questions

97

HW Quesbons pgs 25 & 26

98 99

100 101

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Unit 3: Phases of Matter Lesson 5: The Gas Laws

102

Imagine a Piston... Gases Obey Physical Laws This should not surprise you. The behavior of gases can be predicted and

expressed according to mathematical relationships.

We will look at relationships of Pressure, Volume,

Temperature and the # of molecules (aka moles) of a gas.

103

A Brief Note on Units We will use the following units: Pressure-

Atmospheres(atm) & KiloPascals(kPa) Volume-

Liters(L) and milliliters(ml) Temperature-

Kelvin(K) # of molecules-

Moles(mol) 104

The Beginning: Avogadro’s Hypothesis All of the gas laws stem from Avogadro’s

Hypothesis:

105


Equal numbers of gas par;cles occupy equal volumes of space under the same condi;ons of temperature and pressure.

2 Illustrabve Problems to Consider 1.  Consider two 4.00 L containers, each at 298 K

and 1.00 atm. Container A holds nitrogen gas, Container B holds carbon dioxide gas. If container A holds 2.00 moles of nitrogen gas, how many moles of carbon dioxide must be present in container B?

2.  Do equal volumes of gases under the same conditions of temperature and pressure have the same MASS? Why or why not?

106

How To Solve Any Gas Law Problem 1.  Get rid of the words!

Read the problem and pick out the variables. Make a list of them.

Make sure your units are acceptable and agree.

2.  Write down the particular Gas Law you need. 3.  Rearrange to isolate the variable you’re solving. 4.  Plug in your numbers. 5.  Solve and Round to sig. figs. 6.  Rejoice.

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Boyle’s Law: Pressure & Volume

Temperature must be constant

108

Robert Boyle (1627 -‐ 1691)

As Pressure Increases, Volume Decreases P x V = k (a constant) P1V1 = P2V2

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A sample of gas occupies a volume of 2.00 L at STP. If the pressure is increased to 2.00 atm at constant temperature, what is the new volume of the gas?

109

libretto - unit 3 phasesofmatter - libretto regents …3+phasesofmatter+... · 11/9/10 1 54 10/18...

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