CHEMISTRY 30S GASES & THE ATMOSPHERE SMART BOARD PRESENTATION

ASSIGNMENT DESCRIPTION

You and a partner will generate and present an attractive and informative SMART boardpresentation based on a topic of your choice having to do with gases and the atmosphere.

Your dynamic presentation should involve the other members of the class and will be nolonger_ than five minutes. The following information must be contained in a minimumof five slides as part of a SMART Notebook file:

3 A clear and concise description of your selected topic worded using language thatall of your classmates may understand

3 A creative and. eye catching presentation that includes a minimum of 3 ways ofpresenting information (text, pictures, diagrams. sou d, graphs,videos/animations) in a stylish format

3 An explanation of how your topic relates to the Gas Laws (Boyle's Law, Charles'Law, Gay-Lussac's Law, andior the combined Gas Laws)

3 A specific explanation of particle behaviour as it relates to your topic3 A stylish and concise handout summarizing the content of your presentation using

three different ways to communicate the information3 A complete references cited list of all resources used with active hyperlinks,

including references to photographs, sounds and videos, presented as a separateslide at the end of the presentation

Some suggestions for involving members of the class:o demonstration

o very short game

o quiz

Topic LIST

Research may be done on any of the following topics. No two groups may research thesame topic. All students must write their names on a sign up sheet BEFORE researchinga topic.

• SCUBA diving

• Hot air balloons

• Gas collection and storage

• Salvage divers• Blimps (airships)• Weather balloons• Submarines• Or a topic of your choice (confirm topic choice with

instructor before researching)

TIMELINE

Full Library Da #1 E Thursday, October 16, 2008

• Anaesthetics & medicalapplications

• Airbags• Acetylene welding• Propane appliances• Hyperbaric chambers• Formation of Earth's

atmosphere• Remote controlled divers

Library Day #2Presentations

Thursday, October 23, 2008Friday, Oct. 24 & Monday Oct. 28, 2008

CHEMISTRY 30S GASES & THE ATMOSPHERE SMART BOARD PRESENTATION

Student 1: Student 2:

SMART NOTEBOOK DOCUMENT RUBRICCRITERIA NOVICE

- INTERMEDIATE 2 EKI'ERTInformation is too Information is

Information isWordy and uses Only one of the concise and worded

understandableterms that most required criteria is using language thatstudents do not met all students may

understand understandExplanations Document includes

pertaining to theOnly one of the

explanations of howDocument contains Gas Laws and

required criteria isthe topic relates to

relevant particle behaviour one or more of theinformation of gases are missing

met or containsGas Laws & particle

or containminor errors

behaviour as itsignificant errors relates to topic

Minimum of 3 waysInformation

ways ofTwoof presenting

contained in poster information areDocument has is presented in only

prengprepresent (text, colour,

aesthetic appeal one way and/orinformation are

pictures, diagrams,lacks an aesthetic

present in a stylishsound, graphs,

formatformat

videos/animations)in a stylish format

All references used,including videos

An incomplete list and graphics, are

References citedReferences used are of references used is cited using thenot submitted with part of the document proper format withpage

the poster or is submitted in active hyperlinks onanother format a separate slide at

the end of thepresentation

/12

CHEMISTRY 30S GASES & THE ATMOSPHERE SMART BOARD PRESENTATION

Student 1: Student 2:

PRESENTATION RUBRICCRITERIA NOVICE 1 INTERMEDIATE 2 EXPERT

Group does notincorporate the Presentation is

Presentation is members of the Only one criteria practiced anddynamic audience and the met engages members of

presentation is not the audience.

Ismooth

Timeline adequately

No consideration of reflects the content

Students stick to time limitation or of the poster, the

the five minute rate at which Only two criteria rate at which

time limitation information is met information is

delivered presented, and doesnot exceed five

minutesEach group

memberOne partner Evidence that one All grow membersp

participates in an conducts the entireI

student presented share the role of

equitable waypresentation more than the other presenting equitably

New information ispresented in Handout uses

Information in handout that is not minimum of 2

handout does not contained in the different ways to

match with the presentation or communicateSummary Handout

content of the relevant information information and is a

presentation or no is missing or concise summary of

handout is presented handout only usesI

all of the mainone way of aspects of theconveying presentation

information

/12

/24

A COOL CANTwo companies developing theself-chilling can have overcomethe obstacles. They haveperfected a way to Inject thegas quickly and to vent It slowlyso the gas does not simply chillthe air outside the can.

The can works on theprinciple that when acompressed gas expands, Itstemperature falls. Inside eachcan is a metal capsule filledwith carbon dioxide under highpressure. A valve reieases thegas, cooling the outside of thecapsule and thus the beverage.in volume production theprocess could add 2 to 5 centsto the 8-cent cost of making aconventional can. The carbondioxide chills a beverage byabout 150C. within a minute anda half. Both companies say theywill market the process instandard 280 mL cane.Consumers will pay more forless beverage because thecapsule takes up 40-50 mL ofspace.

This model Eels so" 'is

rpCG . It is based on fourpostulates. Eachp

OWWW faa;ts.

P sudaw1The tiny molecules rils,. tstgr g a d so for span from each other thatspowthe actual volume Ofd*

i

aat wltem compared to the space be-tween them.

Fae : Under no mal^

and pressure about 99.96% of

the total vet el l ?

tqty Spam Gases, therefore:, canbe easily

No intermolecular f

4xW*tjjVM molecules In a perfect (ideal) gas.

Fact: Gases freely a

the entire space available to them.Under condlticas of i

and low temperature, however,be significant. Nevertheless, the factintermolecular faeces find"to

is still observed. -

Molecules of a gas are ca

moving in rapid, straight-line motion. They col-

lide constantly with each9*ad with the sides of the container. Energy is ex-

changed in these coMsioni hono anew Is lost. The collisions are said to becompletely elastic.

Fact: A Brownian motiiem apparatus can be used to show that gas molecules arein continuous motion. Particles of dust or smoke are added to thegas (air) In the apperatt Even though the gas molecules are too

small to be seven, the particles of smoke can be observed through amicroscope. These particles move continuously as if they werebeing bit by the invisible gas molecules. Since the dust particlesdo not settle out, we can assume that these collisions are strongenough to oven the pull of gravity on the dust particles.

At any given time, not all molecules of the gas have the same speed and, therefore,their individual kinetic energies also vary . However, on the average the kineticenergies of different gasses are the same and the average kinetic energy of themolecules varies directly (Le. the average kinetic energy of the gas molecules in-creases as temperature increases) with the absolute temperature of the gas.

Fact: Collisions between molecules of gas will continually cause their speed tochange. However, the collisions are elastic and thus, no kinetic ener-gy is kW during these collisions. The total kinetic energy of the sys-tem is the sum of the kinetic energies of all the molecules, If thetemperature of the gas is in reased by adding heat; the averagekinetic energy of the particles will increase proportionately.

T

t

Use the particle theory of matter to answer thefollowing questions:

1. Why is it easier to compress a gas than a liquid?

2. Why must heat be removed to change liquidwater to ice?

3. How does air inside a balloon hold the rubberout? That is, what causes pressure?

4. The air pressure inside an automobile tireincreases when the tire becomes warm. Why isthis so?

1 www.pemblnatrails.caishaftesbury/mrdeakin 'r adeakin!E pembinatraiis_ca(204) 888-5898 ''.

Shaftesbury High School, 2240 Grant Ave, Wpg, MB, R3P OP7

n collisions

the speed,

is in a gas..e particles

with the.;;molecule

ainer. It isNails of a'measured::.

15:3 MEASURING PRESSUREIn measuring gas pressure, an instrument called a manometer (mah

NAH'11 uh tuhr) is used. Two types of manometers are shown in Figure15-3. In the "open" type, air exerts pressure on the column of liquid inone arm of the U-tube. The gas being studied exerts pressure on the otherarm. The difference in liquid level between the two arms is a measure of

the as pressure relative to the air pressure. If you know the density of theliquid in the manometer, you can calculate the pressure difference

between the gas and the air.

15:3 Measuring Pressure

287

FIGURE 15-3. Closed (a) andopen arm (b) manometers areused to measure gas pressure.

'onstantly

you andfrom the

indard of.air at sea':nd uponns at seatern that:'a). One.We will

The "closed" type of manometer has a vacuum above the liquid inone arm. The operation of a closed-arm manometer is independent of airpressure. A closed-arm manometer used to measure atmospheric pressure

is called a barometer. Most barometers are manufactured with a scalecalibrated to read the height of a column of mercury in millimetres. Aver-age air pressure will support a column of mercury 760 mm high. Sinceaverage air pressure is defined as 101.325 kPa, then 101.325 kPa = 760

FIGURE 15-4. This barometer (a)is used to measure air pressurein the laboratory. This gauge (b)

measures air pressure in tires.A sphygmomanometer (c) isused to measure blood pres-sure.

288

Kinetic Theory

mm. By dividing both sides of the equation by 101 .325 we find that 1 kPa= 7.50 mm Hg.

Closed-arm manometers can be used to measure actual or "abso..lute" gas pressure. It is also possible to calculate the absolute pressure of agas using an open manometer. However, a barometer must be available

to measure the atmospheric pressure on the outside arm of the opetimanometer. The following examples show some typical calculationsinvolving gas pressure.

EXAMPLE.:, PressureThe open manometer in Figure 15-3 is filled with mercury. The differencebetween mercury levels in the two arms is 6 mm. What is the total presssure, in kilopascals, of the gas in the container? The air pressure is 101.3kPa.Solving Process:The mercury is higher in the arm connected to the gas. Thus, the pressure

exerted by the gas must be less than that of the air. As a result, we mustsubtract the pressure of the mercury from the air pressure to get the gas:pressure. Before subtracting, however, we must convert the 6 mm difference in height to kilopascals.

I kPa= 0.8 kPa

7.50 i rr

Now we can subtract the two pressures.

101.3 - 0.8 = 100.5 kPa

EXAMPLE: PressureSuppose the difference in height of the two mercury levels in the closedmanometer in Figure 15-3 is 238 mm. What is the pressure in kilopascals:of the gas in the container?Solving Process:

Since the column of mercury is 238 mm high and 7.50 mm of mercury;equals 1 kPa, the pressure is

Air pressure is 97kilopascals?A closed manorneand connected toof mercury in thenitrogen in kilopaAn open manometamer of oxygen.the tube connecte,kPa. What is the l

4. An open manomet38 mm higher in96.3 kPa, what is

5. A closed manometamer of helium.two arms is 86.0helium?

15:4 KINETICThe average spee

temperature and the mititle mass related?

Kinetic energy ismotion. Temperature iskinetic energy of molecoa particular tem.peraturtemperature, the averagkinetic energy of a parti.velocity. Therefore, at a

6 p+rr

2.

3.

238 sornl kPa7.50

err = 31.7 kPa

1. An open manometer, such as the one in Figure 15-3, is filled with

mercury and connected to a container of hydrogen. The mercury...level is 62 mm higher in the arm of the tube connected to the gasz;

15:4 Kinetic Energy and Temperature

d that 1 kPa Air pressure is 97.7 kPa. What is the pressure of the hydrogen inkilopascals?

2. A closed manometer like the one in Figure 15-3 is filled with mercuryand connected to a container of nitrogen. The difference in the heightof mercury in the two arms is 691 mm. What is the pressure of thenitrogen in kilopascals?

3. An open manometer is filled with mercury and connected to a con -

tainer of oxygen. The level of mercury is 6 mm higher in the arm of

the tube connected to the container of oxygen. Air pressure is 100.0kPa. What is the pressure, in kilopascals, of the oxygen?

4. An open manometer connected to a tank of argon has a mercury level38 mm higher in the atmospheric arm. If atmospheric pressure is96.3 kPa, what is the pressure of the argon?

5. A closed manometer is filled with mercury and connected to a con-tainer of helium. The difference in the height of mercury in thetwo arms is 86.0 mm. What is the pressure, in kilopascals, of thehelium?

15:4 KINETIC ENERGY AND TEMPERATUREThe average speed of the particles in a gas depends only on the

temperature and the mass of the particles. How are temperature and par-ticle mass related?

or "abso -ressure of ae availablef the openalculations

difference

total pres.e is 101.3

pressure

we must

et the gasim differ-

WAX

Kinetic energy is the energy an object possesses because of itsmotion. Temperature is a measure of that kinetic energy. The averagekinetic energy of molecules or atoms in a gas is the same for all particles ata particular temperature. In other words, if two gases are at the sametemperature, the average kinetic energies of their particles are equal. Thekinetic energy of a particle is equal to mv212, where m is its mass and v itsvelocity. Therefore, at a given temperature, a particle with small mass will

e closed

)pascals

nercuryParticles of samples of gases atthe same temperature have thegame average kinetic energy.

FIGURE 15-5. The cotton on oneend of the tube Is saturated withconcentrated HCI. The cotton atthe other end is saturated withNH3(aq). The formation ofNH4Ct Is shown by the whitering in the tube. By noting theposition of the ring, can you de-termine which end of the tubecontains HCI?

FIGURE 15-8. The first twographs show the relationshipsamong mass, velocity, and ki-netic energy. The third graphshows that In any given samplesome particles will have moreor less energy than the averageparticle.

•

290

Kinetic Theory

sere. 9s -273'C

FIGURE 15-7. Theoretically, thepoint at which molecular mo-tion ceases (KE = 0) is absolutezero (--273°C).

Cold

Hot

FIGURE 15-8. Heat flows fromhot objects to cooler onesthrough a transfer of kinetic en-ergy when particles collide.

move faster than a particle with large mass. A decrease in the temperatureof a substance means the particles of the substance are moving moreslowly. An increase in temperature means the particles are movingfaster.

In theory, it should be possible to lower the temperature to a pointwhere all molecular motion ceases, The temperature at which all molec-ular motion should cease is known as absolute zero. It is -273.15°C. Thisvalue is usually rounded to -273°C.

To make a temperature scale based on absolute zero, scientists haveagreed on a system known as the absolute, or kelvin scale. The zero pointof the kelvin scale is absolute zero. The divisions, or degrees, are thesame size as those of the Celsius scale. Therefore,

K=°C+273

The kelvin is the SI unit of temperature.

MMOW

Temperature can be used to determine the direction of flow ofenergy. Energy always flows from a warmer object to a cooler one. Ki -netic theory explains the flow of energy in terms of particle collisions. Theparticles of the warmer object and the cooler object have unequal kineticenergy. The excess kinetic energy of the particles in the warmer object ispassed on to the particles of the cooler object as they collide, Figure 15-8.The particles of the cooler object gradually receive more kinetic energyuntil the average kinetic energy of both objects is the same. For example,you can feel the air warm near a bowl of hot soup. If left undisturbed thesoup and bowl will eventually reach room temperature. Heat is theamount of energy transferred. Heat, like energy, is measured in joules.

6. Convert the folio,a. 65°

b. 1(7. Convert the folloF

a.86

b.1=8. Convert the folio'

a. 23°

b. 5f

9. Convert the folio'

a. 872

b. 6=

10. At 25°C, which ca. N 2

b. F

15:5 STATESMatter exists in ft

our discussion of the

kinetic theory can alliquids. Plasmas are t

Gas particles areline. Change of direcanother, or when a p:particles, then, traveluntil they collide witgases assume the sha

The particles of amotion. Actually, theywith near neighbors.often shifts as one piamount of space betrelative positions coalvolume, assume the t

In solids, a partic

the surrounding parti(

fixed point. Again, ttbetween collisions wioxygen gas at 25°C try

diameter before collieparticles are closely pof their diameters beftitles arranged in a doshape and, a definite

The )hysical statatmospheric pressure

15:5 States of Matte 291

ve

nt

fe

6. Convert the following temperatures from Celsius to kelvin,

a. 65°

b. 16° .

c. 48°

d. ---36`

e. -7 3°

7. Convert the following temperatures from kelvin to Celsius.

a. 86

b. 191

c. 533

d. 321

e. 894

8, Convert the following temperatures from Celsius to kelvin.

a. 23°

b. 58°

c. -90°

d. 18°

e. 25°

9. Convert the following#emperatures from kelvin to Celsius.

a. 872

b. 690

c. 384

d. 20

e. 60

10. At 25°C, which of the following gas molecules move fastest?

a. N2

b. F2

C. CO

d. 02

15:5 STATES OF MATTERMatter exists in four states----solid, liquid, gas, and plasma. Thus far,

our discussion of the kinetic theory has been limited to gases. However,kinetic theory can also be used to explain the behavior of solids andliquids. Plasmas are treated as a special case.

Gas particles are independent of each other and move in a straightline. Change of direction occurs only when one particle collides withanother, or when a particle collides with the walls of the container. Gasparticles, then, travel in a completely random manner. Since they traveluntil they collide with a neighbor or with the walls of their container,gases assume the shape and volume of their container.

The particles of a liquid have what appears to be a vibratory type ofmotion. Actually, they are traveling a straight-line path between collisionswith near neighbors. The point about which the seeming vibration occursoften shifts as one particle slips past another. These differences in theamount of space between particles allow the particles to change theirrelative positions continually. Thus, liquids, although they have a definitevolume, assume the shape of their container.

In solids, a particle occupies a relatively fixed position in relation tothe surrounding particles. A particle of a solid appears to vibrate about afixed point. Agi.in, the particle is actually traveling a straight-line pathbetween collisions with very near neighbors. For example, a molecule ofoxygen gas at 25°C travels an average distance equal to 314 times its owndiameter before colliding with another molecule. In a solid, however, theparticles are closely packed and travel a distance equal to only a fractionof their diameters before colliding. Unlike liquids, solids have their par-ticles arranged in a definite pattern. Solids, therefore, have both a definiteshape and, a definite volume.

The physical state of a substance at room temperature and standardatmospheric pressure depends mostly on the bonding in the substance.

6 a.

i. .

8s

d. 48'C

b. _ $2`C

e. 621.,

E,. 26U1

M

is m

ftand

0

rr

1 4

NAME

OAT C

..e ins .

-t -f? v" Y" icy

c HE 30 15

def-eyv`nt"a +Ae Preecu

of

1 4 50 VK v" Hc^

(.

tq1

^2.

Far '4-(,, ) 8,c w -fke rr+evcur(j in 41e movmme- er c&v c' (abed ±,e dif-Cevevia

be 4weeu 4- t le ,+-e i s -ko cQ r resQUAc'. 4o

&'4ere ce "vi Prrss vas .

'If

UU

'4 3 m m 9 5

753 aAm I51 a

VWM

755 M W!

or-^C 1+

r

t° ` e Y Vial I IA

Ocl V Y

kI SSi i.iVV („34

^L

\ C{ L. i

b^ ,vL C3L^•L .

^

61i

ICes (L?Ye o ^ e

v

b t,+c-^ aa?+1e i r `P +

[ ^ C + t t

u;as acd

f 3o,, 5W.. 45

PASCO scientificScience Workshop

Chemistry Lab Manual: C07 -1Boyle 's Law (P & V)

Experiment C07: Boyle's Law (P & V)(Pressure Sensor - Absolute)

Concept

Time SW Interface Macintosh® file

Windows® file

gas laws

l m 300 700

C07 Boyle's Law

1C0 _BOYL.S S

Adapted from materials provided by Terri Case, J.L Case High School, Racine, WL

©UIPMENT NEEDEDScience Works

rm Interface•

ressure sensor - absolute•

printer (optional)

PURPOSE

The purposr of this laboratory activity is to experimentally determine the relationship between

the pressure and volume of a sample of air at a constant temperature.

THEOAY

Boyle's Law states that for a given amount of a gas at a fixed temperature the pressure of the gas

is inversely proportional to the volume.

SAEETY PROCEDURES

Follow all safety directives given by your teacher.

PROCEDURE

For this activity, the pressure sensor will measure the change in pressure of a gas inside a

cylinder as the volume of gas changes. The Science Workshop program records and displays the

data. The plot of pressure and volume shows the relationship between them.

PART lz Computer Setup

I. Connect the Science Workshop interface to thecomputer, turn on the interface, and turn on thecomputer.

2. Connect the DIN plug of the pressure sensor toAnalog Channel A on the interface.

3. Open the Science Workshop file titled as shown:

Macintosh

C07 Boyle's Law (pressure)WindowsC07 BOYL.SWS

to

0 1996, PASCO scientific

c©7 -1

PASCO scientificScience Workshop

Chemistry Lab Manual: C07 - 3Boyle's Law (P & V)

Put the barb end of a quick releaseconnector into one end of a short piece ofplastic tubing that comes with the PressureSensor.

2.

Put the end of the piston of the syringe atthe 20 mL, line. Connect the end of thesyringe to the other end of the small piece(about 2.5 cm) of plastic tubing (includedwith the pressure sensor).

3.

Align the quick-release connectoron one end of the plastic tubingwith the connector on thePRESSURE PORT of the PressureSensor. Push the connector ontothe port, and then turn theconnector clockwise until it clicks(about one-eighth turn).

4. Check that the syringe and pressure sensor have a secure seal by adjusting the volumebetween 20 ml, and 10 mL. It should get harder to push as the volume decreases.

PART III: Data Recording

1. When you are ready to begin the experiment, click the "REC" buttonrecording data.

The Keyboard Sampling dialog box opens.

2. Adjust the volume of air in the syringe to 20.0 nL.

3. When the pressure reading stabilizes, type in 20.0 in theKeyboard Sampling dialog box and click on "Enter"

4. Reduce the volume to 18.0 mL. Type in 18.0 in theKeyboard Sampling dialog box and click on "Enter".

5. Continue reducing the volume by 2.0 mL, checking the pressure, and entering the newvolume until your last entered volume is 10.0 mL.

After you enter 10.0, press the "Stop Sampling" button (L

Stop Sampl ing

) to enddata recording.

tc 01996, PASCO scientific

C07 - 3

quick-releaseconnector

plastictubing

barb

PressurePlastictubing

Sensor To

Interface

Syringe

Boyle 's Law: Pressure and Volume

) to begin

Kegboard sampling

Volume (ml)

at I

Stop Sampling

C07 - 4: Chemistry Lab ManualBoyle's Law (P & V)

PASCO scientificScience Workshop

ANALYZING THE DATA

Click on the Graph window tobring it to the front. Click on

the "Autoscale" button (to rescale the Graph to fit thedata. Notice that one plotshows Volume versus Pressureand that the second plot showsInverse Volume versusPressure.

2. Select "Print Active Display"from the File menu to print acopy of the Graph.

Pk0 II 11t

ON=

(1

60 70 80 90 100 110 120 130 140!N®

yt

,('^,

^r►

Pressure (kPa)C3

V

A osede

3. Click on the Table to select it. Select"Print Active Display" from the Filemenu to print a copy of the datatable.

4. If time permits, repeat the procedure.For both the Table and the Graphwindows, you can choose which runis displayed by clicking on the

"DATA" buttons (

). Be surethat you are consistent about whichrun is specified for all the columnson the Table or both plots on theGraph.

GIUEST1ONS

Table

El -i LEE

QQ o.oo ...

©.oa ...

o.oo ...

In4.x Pressure (...

Volume NO

Invcl (1 !mi)

2- ---- --------

--_............- _......_._....._..._.......... ..

._._,.._......

-

_........_........ _..._.

5........... ... _.._.........._.__._..._.._...,..__.._.._..-°--....._........___......._..._._._.

8_9

10

E

Charles' Law Activity

Objective1. Develop the relationship between volume and temperature at constant pressure.2. Calculate absolute zero using experimental data.

Procedure and Calculations1. Given the following data, graph volume in millilitres on the y-axis versus

temperature on the x-axis. Set up your graph so that you can extrapolate the lineto where it intersects the x-axis (the x-intercept).

Temperature (°C) ` Volume mL)91.9 26775 256

50 238

20 217

_L8 202- 10 196- 15 193

2. Use a ruler to sketch the line of best fit, extrapolating the line to where itintersects the x-axis.

3. Calculate the slope of the graph and determine the y-intercept.

4. Determine the actual value of the x-intercept.

Conclusion1. State the relationship between volume and temperature at constant pressure.

2. According to the experimental data, what is the value of absolute zero? Why doesthis value differ from absolute zero?

Date:

Assignment:

From: To:

Form 4A-BW. a 2000 Mathematics Help Central

http:/fwww.mathematicshelpcentr'al.com

4 Boy es'' Law

Use Boyles' Law to answer the following questions:

1) 1.00 L of a gas at standard temperature and pressure is compressed to

473 mL. What is the new pressure of the gas?

2) In a thermonuclear device, the pressure of 0.050 liters of gas within the

bomb casing reaches 4.0 x 10$ atm. When the bomb casing is destroyed

by the explosion, the gas is released into the atmosphere where it

reaches a pressure of 1.00 atm. What is the volume of the gas after the

explosion?

3)Synthetic diamonds can be manufactured at pressures of 6.00 x 104 atm.

If we took 2.00 liters of gas at 1.00 atm and compressed it to a pressure

of 6.00 x 104 atm, what would the volume of that gas be?

4)The highest pressure ever produced in a laboratory setting was about 2.0

x 100 atm. If we have a 1.0 x 10'6 liter sample of a gas at that pressure,

then release the pressure until it is equal to 0.275 atm, what would the

new volume of that gas be?

a 2O Cavalcade Pubishrp - Al Rights Reserved

5)

Atmospheric pressure on the peak of Mt. Everest can be as low as 150mm Hg, which is why climbers need to bring oxygen tanks for the last part of theclimb. If the climbers carry 10.0 liter tanks with an internal gas pressure of 3.04x 10^ mm Hg, what will be the volume of the gas when it is released from thetanks?

6)

Part of the reason that conventional explosives cause so much damage

isthat their detonation produces a strong shock wave that can knock thingsdown. While using explosives to knock down a building, the shock wavecan be so strong that 12 liters of gas will reach a pressure of 3.8 x 10"' mmHg. When the shock wave passes and the gas returns to a pressure of780 mm Hg, what will the volume of that gas be?

7)

Submarines need to be extremely strong to withstand the extremely highpressure of water pushing down on them. An experimental researchsubmarine with a volume of 15,000 liters has an internal pressure of 1.2atm. If the pressure of the ocean breaks the submarine forming a bubblewith a pressure of 250 atm pushing on it, how big will that bubble be?

8) Divers get "the bends" if they come up too fast because gas in their bloodexpands, forming bubbles in their blood. If a diver has 0.05 L of gas in hisblood under a pressure of 250 atm, then rises instantaneously to a depthwhere his blood has a pressure of 50. 0 atm, what will the volume of gas inhis blood be? Do you think this will harm the diver?

0 2000 eavatcads Pubishl ig - A/ Rughts Reserved

Charles' Law Worksheetrwn.^^nu w i i^r.rnminow^rimr^^ +rr^inni iw

1) The temperature inside my refrigerator is about 40 Celsius. If I place a

balloon in my fridge that initially has a temperature of 22° C and a volume

of 0.5 liters, what will be the volume of the balloon when it is fully cooled

by my refrigerator?

2) A man heats a balloon in the oven. If the balloon initially has a volume of

0.4 liters and a temperature of 20 °C, what will the volume of the balloon

be after he heats it to a temperature of 250 °C?

3)

On hot days, you may have noticed that potato chip bags seem to

"inflate", even though they have not been opened. If I have a 250 mL bag

at a temperature of 19 °C, and I leave it in my car which has a

temperature of 60° C, what will the new volume of the bag be?

4)A soda bottle is flexible enough that the volume of the bottle can change

even without opening it. If you have an empty soda bottle (volume of 2 L)

at room temperature (25 °C), what will the new volume be if you put it in

your freezer (4 °C)?

5)

Some students believe that teachers are full of hot air. If I inhale 2.2 liters

of gas at a temperature of 18 ° C and it heats to a temperature of 38° C in

my lungs, what is the new volume of the gas?

8)

How hot will a 2.3 L balloon have to get to expand to a volume of 400 L?

Assume that the initial temperature of the balloon is 25 °C.

7)

1 have made a thermometer which measures temperature by the

compressing and expanding of gas in a piston. I have measured that at

100 C the volume of the piston is 20 L. What is the temperature outside

if the piston has a volume of 15 L? What would be appropriate clothing

for the weather?

Chemistry 30S- Gay-Lussac Questions

Name:_

1) Determine the pressure change when a constant volume of gas at 1.00 atm is heatedfrom 20.0 °C to 30.0 °C.

2) A gas has a pressure of 0.370 atm at 50.0 °C. What is the pressure at standardtemperature?

3) A gas has a pressure of 699.0 mm Hg at 40.0 °C. What is the temperature at standardpressure?

4) If a gas is cooled from 323.0 K to 273.15 K and the volume is kept constant what finalpressure would result if the original pressure was 750.0 mm Hg?

5) If a gas in a closed container is pressurized from 15.0 atmospheres to 16.0atmospheres and its original temperature was 25.0 °C, what would the final temperatureof the gas be?

6) A 30. 0 L sample of nitrogen inside a rigid, metal container at 20.0 °C is placed insidean oven whose temperature is 50.0 °C. The pressure inside the container at 20.0 °C wasat 3.00 atm. What is the pressure of the nitrogen after its temperature is increased?

7) A sample of gas at 3.00 x 103 mm Hg inside a steel tank is cooled from 500.0 °C to0.00 °C. What is the final pressure of the gas in the steel tank?

8) The temperature of a sample of gas in a steel container at 30.0 kPa is increased from-100.0 °C to 1.00 x 103 °C. What is the final pressure inside the tank?

9) Calculate the final pressure inside a scuba tank after it cools from 1.00 x 103 °C to25.0 C. The initial pressure in the tank is 130.0 atm.

Combined Gas Law Problems

Use the combined gas law to solve the following problems:

1) If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and atemperature of 200 K, and then I raise the pressure to 14 atm andincrease the temperature to 300 K, what is the new volume of the gas?

2) A gas takes up a volume of 17 liters, has a pressure of 2.3 atm, and atemperature of 299 K. If I raise the temperature to 350 K and lower thepressure to 1.5 atm, what is the new volume of the gas?

3)A gas that has a volume of 28 liters, a temperature of 45 °C, and anunknown pressure has its volume increased to 34 liters and itstemperature decreased to 35 °C. If I measure the pressure after thechange to be 2.0 atm, what was the original pressure of the gas?

4)A gas has a temperature of 14 °C, and a volume of 4.5 liters. If thetemperature is raised to 29 °C and the pressure is not changed, what isthe new volume of the gas?

WKS001x007 0 2000 Cavalcade Publishing

All Rights Reserved

5)

If I have 17 liters of gas at a temperature of 67 °C and a pressure of 88.89atm, what will be the pressure of the gas if I raise the temperature to 94°C and decrease the volume to 12 liters?

6)1 have an unknown volume of gas at a pressure of 0.5 atm and atemperature of 325 K. If I raise the pressure to 1.2 atm, decrease thetemperature to 320 K, and measure the final volume to be 48 liters, whatwas the initial volume of the gas?

7)If I have 21 liters of gas held at a pressure of 78 atm and a temperature of

900 K, what will be the volume of the gas if I decrease the pressure to 45atm and decrease the temperature to 750 K?

8)If I have 2.9 L of gas at a pressure of 5 atm and a temperature of 50 °C,what will be the temperature of the gas if I decrease the volume of the gasto 2.4 L and decrease the pressure to 3 atm?

9)1 have an unknown volume of gas held at a temperature of 115 K in acontainer with a pressure of 60 atm. If by increasing the temperature to225 K and decreasing the pressure to 30 atm causes the volume of thegas to be 29 liters, how many liters of gas did I start with?

WKS001x007 0 2000 Cavalcade Publishing ,

All Rights Reserved

GRADE 11 CHEMISTRY • Topic 3 Appendices

Appendix 3.9: Determining the Molar Mass of a Gas (Student Experiment)

PurposeThe molar mass of a compound is an important constant that, in some cases, canhelp identify a substance. In this lab, you will calculate the molar mass of butaneusing calculations involving the combined gas law and the constant 22.4 L/mole.

Materials

• goggles• butane lighter (with flint removed)

• plastic bucket• water

• graduated cylinder (1000 mL)

• funnel• balance• thermometer• barometer

Procedure

1. Determine the initial mass of the butane lighter.

2. Pour water into the bucket until it is about three-quarters full. Then fill thegraduated cylinder with water and invert it into the bucket so that the waterlevel is within the calibrated region. Record the volume reading.

3. Place the funnel in the mouth of the graduated cylinder while it is under thewater to ensure all butane gas bubbles are collected.

4. Hold the butane lighter in the water under the graduated cylinder and funnelapparatus. Release the butane gas from the lighter into the mouth of thegraduated cylinder until you have displaced from half to three-quarters of thewater within the cylinder.

5. Equalize the pressures inside and outside the cylinder by adjusting the positionof the cylinder until the water levels inside and outside the cylinder are the same.

6. Read the measurement on the cylinder and record the volume of gas collected.

7. Record the ambient (room) temperature and pressure.

8. Thoroughly dry the butane lighter and determine its final mass.

Topic 3 Appendices - 31

GRADE 11 CHEMISTRY • Topic 3 Appendices

Appendix 3.9: Determining the Molar Mass of a Gas (Student Experiment) (continued)

Observations

Data Chart

Initial mass of lighter

Final mass of lighter

Mass of gas released

Initial volume reading on graduated cylinder

Final volume reading on graduated cylinder

Volume of gas released

Room temperature

Room air pressure

Calculations

1. Using the combined gas law, convert the volume of gas released in the lab to thevolume it would occupy at standard temperature and pressure (STP).

2. Use the volume of gas at STP (recorded above) and the gas constant of22.4 L/mole to determine the number of moles of gas collected at STP.

3. Use the mass of gas released (from the data chart) and divide it by the moles ofgas at STP to find the molar mass of the gas.

Conclusions

1. What is the molar mass of the butane according to your lab results?2. What is the known molar mass of butane according to the periodic table?3. What is your experimental percent error?4. Every experiment has some experimental error or uncertainties. State some

possible flaws, limitations, experimental errors, or uncertainties that may affectthe accuracy of your results. Make a list and rank them from most to leastsignificant.

5. It is always possible to omit a source of experimental error. In the experiment,you may not have realized that butane in a lighter is not pure butane butcontains a small quantity of water vapour. For a typical room temperature, thiswould correspond to about 2.6 kPa of the pressure you recorded. Subtract thisvalue from the pressure you used, and use the new pressure to recalculate themolar mass and the experimental percent error. Is your answer significantlymore accurate? Explain.

32 - Topic 3 Appendices

GRADE 11 CurMISTRY • Topic 3 Appendices

9: Determining the Molar Mass of a Gas (Teacher Notes)

Safety Precautions

• Butane is highly flammable.

• Do not conduct this experiment near an open flame.• Good ventilation in the laboratory is essential.• Eye protection is required.

• Flints must be removed from the butane lighters. You can pry off the metalcasing (hood) and the spark wheel of the typical disposable commercial lighterwithout much effort, and the flint and a long spring will just pop out.

Important Notes

• You will need one butane lighter per group.• An ice cream pail (4 L) works fine for this experiment, but because it is small it is

a little clumsy to use. The funnel could be removed so that you have more handroom, but then students have to be more careful not to lose the bubbles. A sinkfilled with water works well also.

• If you don't have a barometer, you can find the air pressure for your town or cityon a weather website on. the Internet.

• After thoroughly drying the lighter, you may also want to let it air dry for awhile so that the interior parts can dry as well. A more accurate mass can berecorded after this is done.

Observations

Sample Data Chart

Initial mass of lighter 18.17 g

Final mass of lighter 18.01 g

Mass of gas released 0.16 g

Initial volume reading on graduated cylinder 21.0 mL

Final volume reading on graduated cylinder 89.8 mL

Volume of gas released 68.8 mL

Room temperature 22'C = 295 K

Room air pressure 102.14 kPa

Topic 3 Appendices - 33

GRADE 11 CHEMISTRY • Topic 3 Appendices

Gas Density Table (Student Resource Material)

Density of Gases at 25°C and 101.3 kPa (760 mmHg or 1.0 atm) Pressure

Name

Formula

Ammonia

NH3

Argon

Ar

Butane C4H19

Carbon dioxide

CO2

Carbon monoxide

CO

Dichiorine

Cl2Ethane

C2H6

Ethene

C2H4

Ethyne (acetylene)

C2H2

Helium

He

Dihydrogen

H2

Hydrogen chloride

HCI

Hydrogen iodide

HI

Krypton

Kr

Methane CH4

Neon

No

Nitrogen monoxide

NO

Dinitrogen

N2

Dinitrogen monoxide

Nitrogen dioxide

Dioxygen

02

Ozone

03

Propane

C3H8

Sulphur dioxide

SO2

Xenon

Xe

Molar Mass (g/mol)

17.03

39,944

58.12

44.01

28.01

70.91

30.07

28.05

26.04

4.003

2.016

36.47

127.93

83.70

16.04

20.18

30.01

28.02

44.02

46.01

32.00

48.00

44.09

64.07

131.30

Density (gIL)

0.696

1.633

2.376

1.799

1.145

2.898

1.229

1.147

1.064

0.164

0.082

1.490

5.228

3.425

0.656

0.825

1.226

1.145

1.799

1.880

1.308

1.962

1.802

2,618

5.367

N20

NO2

Topic 3 Appendices - 35