bell work january 31 st , 2014

Bell workBell workJanuary 31January 31stst, 2014, 2014

You will have to do stoichiometry again You will have to do stoichiometry again towards the end of this unit towards the end of this unit

So, given the following equation, So, given the following equation, CC33HH88 + O + O22 CO CO22 + H + H22O if you start with 10 O if you start with 10

grams of tricarbon octahydride, how many grams of tricarbon octahydride, how many grams of water will you end up with?grams of water will you end up with?

AgendaAgendaPressure Conversion FactorsPressure Conversion Factors

Review of the characteristics of gasesReview of the characteristics of gases

Objective:Objective:

You will be able to convert between You will be able to convert between different units of pressure on your own.different units of pressure on your own.

Pressure VideosPressure VideosBasketball:Basketball:

http://www.youtube.com/watch?v=t-Iz414g-ro

Egg:Egg:

http://www.youtube.com/watch?v=28TIyWdfxxc&list=PLCA9B7D3D7031D919

http://www.youtube.com/watch?v=t-Iz414g-ro



For example:

1 pascal (Pa) = 1 N/m2

Barometer

Pressure = ForceArea

Pressure

Write down the following conversion Write down the following conversion factors:factors:

1 atm = 760 torr1 atm = 760 torr

1 atm = 101.3 kPa1 atm = 101.3 kPa

1 atm = 760 mmHg1 atm = 760 mmHg

1 atm = 14.7 psi1 atm = 14.7 psi

1 kPa = 7.50 mmHg1 kPa = 7.50 mmHg

As a class…As a class…Convert: Convert: 1)1) 727 mmHg into kPa727 mmHg into kPa

727mmHg x727mmHg x _ _1 kPa____1 kPa____ 7.50mmHg7.50mmHg

2) 52.5 kPa into atm2) 52.5 kPa into atm

3)3) 0.729 atm into mmHg0.729 atm into mmHg

= 96.9 kPa

Solutions…Solutions…Convert: Convert: 1) 1) 727mmHg x _727mmHg x _1 kPa____1 kPa____

7.50mmHg7.50mmHg

2) 2) 52.5 kPa x _52.5 kPa x _1 atm___1 atm___ 101.3 kPa101.3 kPa

3) 3) 0.729 atm x _0.729 atm x _760 mmHg760 mmHg 1 atm1 atm

= 96.9 kPa

= 0.52 atm

= 554.0 mmHg

On your own…On your own…Convert: Convert:

4) 522 torr into kPa4) 522 torr into kPa

5) 800.0 mmHg into atm5) 800.0 mmHg into atm

6) 495 kPa into mmHg6) 495 kPa into mmHg

Solutions…Solutions…Convert: Convert: 4. 4. 522 torr x _522 torr x _1 atm_1 atm_ x x 101.3 kPa101.3 kPa

760 torr 1 atm760 torr 1 atm

5. 5. 800.0 mmHg x _800.0 mmHg x _1 atm___1 atm___ 760 mmHg760 mmHg

6. 6. 495 kPa x _495 kPa x _7.50 mmHg_7.50 mmHg_ 1 kPa1 kPa

= 69.58 kPa

= 1.05 atm

= 3712.5 mmHg

PracticePracticeIf a paint ball COIf a paint ball CO22 tank tank

is at a is at a pressure of pressure of 2000psi2000psi and you know and you know that that 1psi1psi equalsequals 51.7mmHg51.7mmHg, how many , how many atmatm of pressure are in of pressure are in the tank?the tank?

SolutionSolutionKnown quantity: 2000 psiKnown quantity: 2000 psi

Conversion factors: 51.7 mmHg/1 psiConversion factors: 51.7 mmHg/1 psi

1 atm/760 mmHg1 atm/760 mmHg

Elements that exist as gases at 250C and 1 atm

Gases assume the volume and shape of their containers.

Gases are the most compressible state of matter.

Gases will mix evenly and completely when confined to the same container.

Gases have much lower densities than liquids and solids.

Physical Characteristics of Gases

Standard Temperature and Pressure

Standard temperature and pressure, (STP), refers to conditions in the atmosphere at sea level.

Temperature = 0°C or 273KPressure = 1atm

This is essentially the freezing point of pure water at sea level, in air, at standard pressure

KelvinKelvin

When doing gas law problems, all When doing gas law problems, all temperatures must be in Kelvin, not temperatures must be in Kelvin, not Celsius!Celsius!

To convert from Celsius to Kelvin, just add To convert from Celsius to Kelvin, just add 273.273.

So, -10°C would be: So, -10°C would be:

-10°C + 273= 263K-10°C + 273= 263K

Pressure Conversion Pressure Conversion HW…HW…

Convert: Convert: 1.1. 258 mmHg into kPa258 mmHg into kPa2.2. 30.5 kPa into atm30.5 kPa into atm

3.3. .259 atm into mmHg.259 atm into mmHg

4.4. 752 torr into kPa752 torr into kPa

5.5. 526 mmHg into atm526 mmHg into atm

6.6. 125 kPa into mmHg125 kPa into mmHg

Bell WorkFeb. 2nd, 2014

How about volume of a cylinder? Pi*r2h What would be the volume of a sausage link if its diameter was 4 cm and it is 10.2 cm height?

Remember density? D = g/mlWhat is the density of a 5.6 gram substance that takes up 9.8 mL of space.

As a class…As a class…

What is the mass in grams of a textbook What is the mass in grams of a textbook that is 10 inches long, 8 inches wide, and that is 10 inches long, 8 inches wide, and 3 inches thick, if it has a density of 0.382 3 inches thick, if it has a density of 0.382 g/cmg/cm33??

Remember…Remember…

Density=mass/volumeDensity=mass/volume

Volume of a cylinder=pi*rVolume of a cylinder=pi*r22hh

PracticePractice1. Solve for T1. Solve for T22: : PP11VV11 = = PP22VV22

T1 T2

2. What would be the 2. What would be the volumevolume of a 50 gram sphere of of a 50 gram sphere of platinum (density of platinum = 21.50 g\cmplatinum (density of platinum = 21.50 g\cm33))

3. What would be the mass of 15.2 cm3. What would be the mass of 15.2 cm3 3 of water? d=1 g/cmof water? d=1 g/cm33

4. The density of the core of the sun is = 150 g\cm4. The density of the core of the sun is = 150 g\cm33 how how many cubic centimeters would 10 g be? many cubic centimeters would 10 g be?

5. PV = nRT; solve for n!5. PV = nRT; solve for n!

6. PV = nRT; P=3 atm; V= 1L; T= 273 K; R= .0821atm6. PV = nRT; P=3 atm; V= 1L; T= 273 K; R= .0821atm..L/ L/

molmol..KK

PracticePractice1. What would be the 1. What would be the volumevolume of a 50 gram sphere of platinum of a 50 gram sphere of platinum

(density of platinum = 21.50 g\cm(density of platinum = 21.50 g\cm33) ) {ec find the diameter} {ec find the diameter}

2. What would be the mass of 15.2 cm2. What would be the mass of 15.2 cm3 3 of water? of water?

3. What would be the 3. What would be the mass in gramsmass in grams, of a solid steel flagpole if its , of a solid steel flagpole if its circumference was 20cm? (density of steel = 7.3 g\cmcircumference was 20cm? (density of steel = 7.3 g\cm33) *height ) *height of 5 meters of 5 meters

4. The density of the core of the sun is = 150 g\cm4. The density of the core of the sun is = 150 g\cm33 how many how many cubic centimeters would 10 g be? cubic centimeters would 10 g be?

5. What would be the mass 5. What would be the mass in grams in grams of the trunk of a tree that of the trunk of a tree that had a circumference of 1 meter and was 3 meters tall (density of had a circumference of 1 meter and was 3 meters tall (density of pine = 600 g\mpine = 600 g\m33))

6.6. Solve for TSolve for T11: : PP11VV11 = = PP22VV22

T1 T2

Bell WorkFeb. 3rd, 2014

Tough one?: What would be the pressure in atm if the pressure gauge read 4500psi and 14.7psi is equals 1 atm?

Not so tough one:What is the pressure of a tank of He in atm if the pressure gauge reads 5700mmHg.

Extra CreditFrom test!

Using the following equation…HCl + NaOH H2O + NaCl1) How many grams of NaCl are produced if you start with 5.5 grams of NaOH?

2) Calculate the percent yield of NaCl if you ended up with 6.5 grams in lab.

AgendaAgendaBoyle’s Law Practice ProblemsBoyle’s Law Practice Problems

Objective:Objective:

You will know how to carry out basic Boyle’s You will know how to carry out basic Boyle’s Gas Law Calculations and visually see the Gas Law Calculations and visually see the out come on volume when varying pressure.out come on volume when varying pressure.

VideosVideos

http://www.youtube.com/watch?v=q6-oyxnkZC0

http://www.youtube.com/watch?v=3yvSQuTP4T4





Sea level 1 atm

4 miles 0.5 atm

10 miles 0.2 atm

ClosedOpen

As P (h) increases V decreases

P 1/V

P x V = constant

P1 x V1 = P2 x V2

Boyle’s Law

Constant temp. Const. amount of gas

Boyle’s Law

What is Boyles Law…What is Boyles Law…

PP11VV11= P= P22VV22

So pressure is inversely proportional to So pressure is inversely proportional to volume:volume:

As Pressure goes up… volume goes___As Pressure goes up… volume goes___

As pressure goes down… volume goes____As pressure goes down… volume goes____

Examples of Boyle Law at Examples of Boyle Law at workwork

A syringe being used A syringe being used to draw bloodto draw blood

Popping a balloonPopping a balloon

Popping ears during Popping ears during elevation changeelevation change

Solve for …Solve for …

VV22


PP11


A sample of chlorine gas occupies a volume of 946mL at a pressure of 726mmHg. What is the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 154 mL?

Try this…

A sample of chlorine gas occupies a volume of 946mL at a pressure of 726mmHg. What is the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 154 mL?

P1 x V1 = P2 x V2

P1 = 726 mmHg

V1 = 946 mL

P2 = ?

V2 = 154 mL

P2 = P1 x V1

V2

= 726 mmHg x 946 mL154 mL

= 4460 mmHg

From the data in the following table From the data in the following table calculate the missing quantity calculate the missing quantity

(assuming constant temperature).(assuming constant temperature).

a) Va) V11 = 22.4 L; P = 22.4 L; P11= 1 atm; = 1 atm; PP22 =? atm =? atm; V; V22 = 2.8L = 2.8L

b) Vb) V11 = 60mL; = 60mL; PP11 =? kPa =? kPa; P; P22 = 101.3kPa; V = 101.3kPa; V22= 16 mL = 16 mL

c) c) VV11 = ? L = ? L ; P; P11 = 40 kPa; P = 40 kPa; P22 = 100 = 100 kPa; V; V22 = 1.0 L = 1.0 L

d) Vd) V11 = 2.50 L; P = 2.50 L; P11 = 7.5 atm; = 7.5 atm; PP22 = ?atm = ?atm; V; V22 = 0.100L = 0.100L

Practice makes perfect Practice makes perfect A sample of hydrogen at 1.50 atm had its A sample of hydrogen at 1.50 atm had its

pressure decreased to 0.50 atm producing pressure decreased to 0.50 atm producing a new volume of 750 mL. What was the a new volume of 750 mL. What was the sample’s original volume? sample’s original volume? 250ml

Boyle’s ppt. HWBoyle’s ppt. HW

1)1) If the initial volume is 3.7 L and the initial If the initial volume is 3.7 L and the initial pressure is 180.0 KPa, what is the final volume pressure is 180.0 KPa, what is the final volume if the final pressure is 160 KPa? if the final pressure is 160 KPa?

2)2) If volume doubles, what happens to pressure?If volume doubles, what happens to pressure?

3)3) A pressure of 950.0 Kpa is required to initially A pressure of 950.0 Kpa is required to initially inflate a balloon 300.0 mL. What is the final inflate a balloon 300.0 mL. What is the final pressure when the balloon has reached its pressure when the balloon has reached its capacity of 1.5 L?capacity of 1.5 L?

Bellwork 2-4-14Bellwork 2-4-14

1) What happens to volume as pressure 1) What happens to volume as pressure increases?increases?

2) Convert 2.5 atm to kpa.2) Convert 2.5 atm to kpa. 3) Now convert that number to mmHg.3) Now convert that number to mmHg. 4) What does STP stand for??4) What does STP stand for??

Check your grades—mid quarter is Friday!Check your grades—mid quarter is Friday! Test back to look at—not 5Test back to look at—not 5 thth!!

BELL WORKBELL WORK2-5-20142-5-2014

A sample of mustard gas is in a sealed vessel A sample of mustard gas is in a sealed vessel that can change volume based on internal gas that can change volume based on internal gas pressure. If the sample of gas started at a pressure. If the sample of gas started at a volume of volume of 500mL 500mL and an unknown pressure and an unknown pressure and then the pressure changed to and then the pressure changed to 540mmHg 540mmHg and a new volume of and a new volume of 0.75L0.75L was established, was established, what was the original pressure of the vessel?what was the original pressure of the vessel?

(write out all the parts first…)(write out all the parts first…)

Bell WorkBell Work6-Feb-20146-Feb-2014

1)1) Fluorine gas exerts a pressure of 900 Fluorine gas exerts a pressure of 900 torr. When the pressure is changed to torr. When the pressure is changed to 1.50 atm, its volume is 250 mL. What 1.50 atm, its volume is 250 mL. What was the original volume? was the original volume?

2)2) What is 50 degrees C in Kelvin?What is 50 degrees C in Kelvin?

3)3) 78 kpa is equal to how many torr?78 kpa is equal to how many torr?

Boyle’s Law LabBoyle’s Law Lab

Please do not damage the plunger/ syringePlease do not damage the plunger/ syringe

Practice makes perfect Practice makes perfect 1.00L of a gas at standard temperature and 1.00L of a gas at standard temperature and

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

In a thermonuclear device, the pressure of In a thermonuclear device, the pressure of 0.050L of gas within the bomb casing 0.050L of gas within the bomb casing reaches 4.0 x 10reaches 4.0 x 1066 atm. When the bomb atm. When the bomb casing is destroyed by the explosion, the casing is destroyed by the explosion, the gas is released into the atmosphere where gas is released into the atmosphere where it reaches a pressure of 1.00 atm. What is it reaches a pressure of 1.00 atm. What is the volume of the gas after the explosion?the volume of the gas after the explosion?

2.11atm

2.0x105L

AgendaAgenda

Boyles Law Practice ProblemsBoyles Law Practice Problems

Finish Boyle’s law labFinish Boyle’s law lab

ObjectiveObjective

You will know how to recognize a Pressure You will know how to recognize a Pressure volume problem and understand the volume problem and understand the concept of Boyle’s lawconcept of Boyle’s law

Bell WorkBell Work7-Feb-20147-Feb-2014

1)1) Neon gas exerts a pressure of 2.3 atm. Neon gas exerts a pressure of 2.3 atm. When the pressure is changed to 1.50 When the pressure is changed to 1.50 atm, its volume is 125 mL. What was atm, its volume is 125 mL. What was the original volume in liters? the original volume in liters?

2)2) How do you go from Kelvin to Celsius?How do you go from Kelvin to Celsius?

3)3) One more time, what are the values at One more time, what are the values at STP?STP?

4)4) Solve Boyle’s Law for PSolve Boyle’s Law for P22..

AgendaAgendaVolume vs. Temp.Volume vs. Temp.

Charles lawCharles law

Objective:Objective:You will understand the relationship between You will understand the relationship between

volume and temperature and how it relates to volume and temperature and how it relates to gas molecules. By the end of the period you gas molecules. By the end of the period you will be able to compute basic volume will be able to compute basic volume temperature calculationstemperature calculations..

Recall…Recall…

With your partner convert 23,015 Kpa to With your partner convert 23,015 Kpa to atm.atm.

According to Boyle’s Law what happens to According to Boyle’s Law what happens to Pressure as volume increases?Pressure as volume increases?

As T increases… V increases

Variation of gas volume with temp.at constant pressure.

V T

V = constant x T

V1 = V2

T1 T2

Charles’ & Gay-Lussac’s

Law

Why is the Kelvin scale used exclusively in gas law calculations?

To convert 0C KT (K) = t (0C) + 273

All temperature must be converted to Kelvin

Because there are no negative temperatures

To convert K 0CT (0C) = t (K) - 273

A sample of carbon monoxide gas occupies 3.20 L at 125 0C. At what temperature will the gas occupy a volume of 1.54 L if the pressure remains constant?

Try this…

A sample of carbon monoxide gas occupies 3.20 L at 125 0C. At what temperature will the gas occupy a volume of 1.54 L if the pressure remains constant?

V1 = 3.20 L

T1 = 398 KV2 = 1.54 LT2 = ?

T2 = V2 x T1

V1

1.54 L x 398 K3.20 L

=

= 192 K

V1/T1 = V2/T2

A sample of nitrogen occupies a volume of A sample of nitrogen occupies a volume of 250mL250mL at at 25 25 CC. What volume will it occupy . What volume will it occupy at at 95 95 CC??

Helium occupies a volume of 3.80L at -45 Helium occupies a volume of 3.80L at -45 C. C. What volume will it occupy at 45 What volume will it occupy at 45 C?C?

A 175 A 175 mLmL sample of neon had its pressure sample of neon had its pressure changed from 75.0 changed from 75.0 kPakPa to 150 to 150 kPakPa. What is . What is its new volume (it’s not Charles Law)? its new volume (it’s not Charles Law)?

Practice makes perfect Practice makes perfect

308.7ml

5.3L

87.5ml

Bell Work 2-10-14Bell Work 2-10-14When the boom can, a volume of 500ml, When the boom can, a volume of 500ml,

was filled with gas the temperature was was filled with gas the temperature was 25°C. During the back draft the 25°C. During the back draft the temperature reached 257°C, what temperature reached 257°C, what volume did the gas expand to?volume did the gas expand to?

**P. slips**P. slips

Practice makes perfect Practice makes perfect A sample of Ne has a volume of A sample of Ne has a volume of 1.83L1.83L at at 23.523.5ooCC. .

At what temperature would the gas occupy At what temperature would the gas occupy 5.00 L5.00 L? Assume pressure is constant? Assume pressure is constant. .

A sample of Ar is collected in a A sample of Ar is collected in a 5.00 x 105.00 x 1022ml ml bottle at a temp. of bottle at a temp. of 12.012.0ooCC. Assuming the . Assuming the pressure remains the same, what volume pressure remains the same, what volume would the gas occupy at would the gas occupy at 2.0 2.0 ooCC? ?

810K

482ml

BELL WORK 2-11-14bBELL WORK 2-11-14b

1. A sample of gas at a volume of 840mL 1. A sample of gas at a volume of 840mL is in a test tube covered by a is in a test tube covered by a centimeter of mercury. If the test tube centimeter of mercury. If the test tube is put in a water bath at a temperature is put in a water bath at a temperature of 55of 55°°C and a new volume of 1.1L is C and a new volume of 1.1L is measured, what was the original measured, what was the original temperature (K)?temperature (K)?

2. What are Standard Temp. & Pressure2. What are Standard Temp. & Pressure

**P. slips**P. slips

Charles Law and Water

100 – (Actual/ Theoretical x100) = % error

Charles video clipsCharles video clips

http://www.youtube.com/watch?v=j2k40Hw3GI0

http://www.youtube.com/watch?v=0aqH1JgmZ_4





RecallRecallSynthetic diamonds can be manufactured at Synthetic diamonds can be manufactured at

pressures of 6.00 x 10pressures of 6.00 x 1044atm. If we took atm. If we took 2.00 L2.00 L of of gas at gas at 1.00atm 1.00atm and compressed it to a pressure and compressed it to a pressure of of 6.00 x 106.00 x 1044atmatm, what would the volume of that , what would the volume of that gas be in mL?gas be in mL?

The highest pressure ever produced in a laboratory The highest pressure ever produced in a laboratory setting was about setting was about 2.0 x 102.0 x 1066atmatm. If we have a . If we have a 1.0 1.0 x 10x 10-5-5 L L sample of a gas at that pressure, then sample of a gas at that pressure, then release the pressure until it is equal to release the pressure until it is equal to 275mmHg275mmHg, , what would the new volume of that gas be?what would the new volume of that gas be?

Answer w/ your partnerAnswer w/ your partnerConsider the following changes imposed upon a Consider the following changes imposed upon a

sample of gas, assuming the variables not sample of gas, assuming the variables not mentioned remain constant:mentioned remain constant:

a.a. What happens to the pressure if the What happens to the pressure if the temperature in K is doubled?temperature in K is doubled?

b.b. What happens to the volume if the What happens to the volume if the pressure is tripled?pressure is tripled?

c.c. What happens to the volume if the What happens to the volume if the temperature decreases from 300K to 200K?temperature decreases from 300K to 200K?

d.d. What happens to the temperature if one-What happens to the temperature if one-half of the gas is removed? half of the gas is removed?

Kinetic Molecular Theory Kinetic Molecular Theory VideoVideo

http://www.youtube.com/watch?v=o2viSF0PjlY



AgendaAgendaKinetic molecular theory (short)Kinetic molecular theory (short)

Combine Gas LawCombine Gas Law

Objective:Objective:You will SEE how volume, pressure You will SEE how volume, pressure

and temperature are related.and temperature are related.

Kinetic Molecular Theory of Gases

1. Gas molecules have far greater distances between them than their own dimensions. They possess mass but have negligible volume.

2. Gas molecules are in constant random motion. No Energy is lost during collisions.

Kinetic Molecular Theory of Gases3. Gases exert neither attractive nor

repulsive forces on one another.

4.The average kinetic energy of the molecules is proportional to the temperature of the gas in Kelvin. Any two gases at the same temperature will have the same average kinetic energy.

Bell Work 2-12-14Bell Work 2-12-141. Solve for x: (4x)17 + 3 = 291. Solve for x: (4x)17 + 3 = 29

2. Solve Charles’s Law for V2. Solve Charles’s Law for V1.1.

3. A sample of neon gas at 503. A sample of neon gas at 50C and a volume of C and a volume of 2.50 Liters is cooled to 252.50 Liters is cooled to 25C. What is the new C. What is the new volume in mL?volume in mL?

***Math Moves U!***Math Moves U!

Hydrogen gas was cooled from 150C to 50C. Its new volume is 75.0 mL. What was its original volume?

Chlorine gas occupies a volume of 25.0 mL at 300 K. What volume will it occupy at 600 K?

Quick Review

COMBINED GAS LAWCOMBINED GAS LAW

Boyles law: Boyles law: PP11 x x VV11 = = PP22 x x VV22

Charles law: Charles law: VV11//TT11 = = VV22//TT22

PP11VV11 = =PP22VV22

TT11 TT22


Solve for VSolve for V11


TT11 TT22


Solve for TSolve for T11


TT11 TT22

A balloon is filled with hydrogen gas to a volume of 0.5L , and a pressure of 2.0atm at a temperature of 25°C. If the balloon is then left out in the sun at a temperature of 35°C and reaches a new volume of 2.0L, what is the new pressure?


A balloon is filled with hydrogen gas to a volume of 0.5L , and a pressure of 2.0atm at a temperature of 25°C. If the balloon is then left out in the sun at a temperature of 35°C and reaches a new volume of 2.0L, what is the new pressure?

V1 = 0.5LP1 = 2.0atm

V2 = 2.0L

T2 = 308K

P2 = P1 V1T2

T1V2

2.0atm x0.5L x 308K

298K x2.0L=

= 0.52atm

P1V1/T1 = P2V2/T2

T1 = 298K

P2 = ?

PracticePracticeA 350 cmA 350 cm33 sample of helium gas is sample of helium gas is

collected at 25.0 collected at 25.0 ooC and 119.3 kPa. C and 119.3 kPa. What volume would this gas occupy at What volume would this gas occupy at STP?STP?

PracticePracticeA weather balloon is filled with helium to a A weather balloon is filled with helium to a

volume of 31.5 L at 20volume of 31.5 L at 20ooC and 1.3 atm. In the C and 1.3 atm. In the stratosphere the temperature and pressure are stratosphere the temperature and pressure are -23-23ooC and 3.00 x 10C and 3.00 x 10-3-3atm respectively. What atm respectively. What will be the volume (in L) in the stratosphere?will be the volume (in L) in the stratosphere?

BELL WORK BELL WORK 2-14-142-14-14

A certain gas is in an elastic vessel at a A certain gas is in an elastic vessel at a pressure of 820 torr, a volume of 0.75L and a pressure of 820 torr, a volume of 0.75L and a temperature of 27temperature of 27ººC. If the volume of the C. If the volume of the vessel is doubled and the pressure becomes vessel is doubled and the pressure becomes 101.325kPa, what is the new Temp (K)101.325kPa, what is the new Temp (K)

A balloon has a volume of 1.0 L at 21.0A balloon has a volume of 1.0 L at 21.0C and C and 750 mmHg. What is the balloon’s volume at 750 mmHg. What is the balloon’s volume at STP?STP?

BELL WORK BELL WORK 2-17-142-17-14 A gas is in an elastic vessel at a pressure of A gas is in an elastic vessel at a pressure of

670mmHg, a volume of 0.5L and a 670mmHg, a volume of 0.5L and a temperature of 30temperature of 30ººC. If the volume of the C. If the volume of the vessel increases by 200 mL and the pressure vessel increases by 200 mL and the pressure decreases by 45 mmHg, what is the new decreases by 45 mmHg, what is the new temperature in Celsius?temperature in Celsius?

BELL WORK BELL WORK 2-26-132-26-131. How many moles is 123 g of H1. How many moles is 123 g of H22SOSO44??

2. If the original temperature is 25C and volume 2. If the original temperature is 25C and volume stays constant, but pressure increases from stays constant, but pressure increases from 760 torr to 775 torr, what is the new 760 torr to 775 torr, what is the new temperature?temperature?

BELL WORK BELL WORK 2-27-132-27-131. How many grams is 3 moles of HNO1. How many grams is 3 moles of HNO33??

2. If the original temperature is 22C and 2. If the original temperature is 22C and pressure stays constant, but volume pressure stays constant, but volume decreases from 10 L to 8.3 L, what is the new decreases from 10 L to 8.3 L, what is the new temperature?temperature?

Baby Goats!Baby Goats!

http://www.youtube.com/watch?v=5IuRzJRrRpQhttp://www.youtube.com/watch?v=5IuRzJRrRpQ

BELL WORK BELL WORK 2-28-132-28-131. Balance the following equation:1. Balance the following equation:

Fe + ClFe + Cl22 FeCl FeCl33

2. How many moles of FeCl2. How many moles of FeCl33 will there be if you will there be if you

start with 3 moles of Clstart with 3 moles of Cl22??

3. How many grams of FeCl3. How many grams of FeCl33 would that be? would that be?

Agenda:Agenda:Ideal Gas lawIdeal Gas law

Objective:Objective:You will be able to solve problems using You will be able to solve problems using

the Ideal Gas Law.the Ideal Gas Law.

ReviewReview1.1. If the volume of a container starts out as 3 L with a pressure of If the volume of a container starts out as 3 L with a pressure of

1 atm, what is the new pressure if the volume is compressed 1 atm, what is the new pressure if the volume is compressed to 2.7 L?to 2.7 L?

2.2. If initial pressure is 0.9 atm with a volume of 8 L at a If initial pressure is 0.9 atm with a volume of 8 L at a temperature of 25C, what is the new volume if the temperature temperature of 25C, what is the new volume if the temperature increases to 27C and pressure increases to 1.1 atm?increases to 27C and pressure increases to 1.1 atm?

3.3. If the volume starts at 7 L and temperature is 28C, what is the If the volume starts at 7 L and temperature is 28C, what is the new volume if the temperature increases to 31C?new volume if the temperature increases to 31C?

Ideal Gas LawIdeal Gas Law

http://www.youtube.com/watch?v=Mytvt0wlZK8http://www.youtube.com/watch?v=Mytvt0wlZK8

Ideal Gas EquationIdeal Gas Equation

Charles’ law: V T(at const. n and P)

Avogadro’s law: V n(at const. P and T)

Boyle’s law: V (at const. n and T)1

R is the gas constantPV = nRT

Must have these units…Must have these units…n = molesV = litersT = KelvinP = atmR = .0821 L(atm)/mol(K)

Why? Look at the units for R

PV = nRT

R = PVnT

=(1 atm)(22.4L)

(1mol)(273 K)

R = 0.082057 L • atm / (mol • K)

At STP, 1 mol of an ideal gas occupies 22.4 L. Experimentally proven to give us the value of R.

What is the volume (in liters) occupied by 1.37moles of HCl at STP?

PV = nRT

V = nRT

P

T = 0 0C = 273 K

P = 1 atm

V =1 atm

1.37molx 0.0821 x 273 KL•atmmol•K

V = 30.7 L

n = 1.37 moles

Practice… Ideal GasPractice… Ideal Gas

0.02 moles of oxygen gas are at 0.5 L at 0.02 moles of oxygen gas are at 0.5 L at 0.25 atm. At what temperature is the gas? 0.25 atm. At what temperature is the gas?

A 0.334L gas cylinder contains 2.12 moles A 0.334L gas cylinder contains 2.12 moles of helium at 23of helium at 23ooC. What is the pressure C. What is the pressure (atm) assuming ideal gas behavior?(atm) assuming ideal gas behavior?

154 atm

76K

HomeworkHomeworkA 26.9 mole sample of neon is introduced into a 4.5 L A 26.9 mole sample of neon is introduced into a 4.5 L

cylinder, and the cylinder is heated until the gas pressure is cylinder, and the cylinder is heated until the gas pressure is 375 atm. What is the gas temperature (in K) at this point?375 atm. What is the gas temperature (in K) at this point?

The pressure in a 2.0 L container is 1.5 x 10The pressure in a 2.0 L container is 1.5 x 10-4-4 torr at 1115K. torr at 1115K. How many moles are in the container?How many moles are in the container?

Turn-In:Turn-In:

Boyle’s Law Lab (Textbooks Lab)Boyle’s Law Lab (Textbooks Lab)

Can Crushn’ LabCan Crushn’ Lab

Ideal Gas Law Lab (Lighter Lab)Ideal Gas Law Lab (Lighter Lab)

Lab Turn InLab Turn InGas Law LabGas Law Lab

Can Crushn’ LabCan Crushn’ Lab

R constant Lab (Lighter Lab)R constant Lab (Lighter Lab)

Bell Work 3-1-13Bell Work 3-1-131. A 500 mL metal cylinder holding 8 1. A 500 mL metal cylinder holding 8

grams of chlroine gas is known to grams of chlroine gas is known to rupture at a pressure of 7.6 x 10rupture at a pressure of 7.6 x 1033 torr. torr. At what temperature, At what temperature, in °Cin °C, will the , will the container fail? container fail?

Bell WorkBell WorkA 500 mL metal cylinder holding 0.100 moles of helium gas is known to rupture at a A 500 mL metal cylinder holding 0.100 moles of helium gas is known to rupture at a

pressure of 10 atmospheres. At what temperature, pressure of 10 atmospheres. At what temperature, in °Cin °C, will the container fail? , will the container fail? (when will it busrt – volume be over 500ml) (when will it busrt – volume be over 500ml)

T = ?T = ?

V = 0.500LV = 0.500L

n = 0.100 moln = 0.100 mol

P = 10atmP = 10atm

R = R = 0.0821 0.0821 LL∙∙atmatm

molmol∙∙KK

PV = nRT

T = PV/nR

T = ___(10atm)(0.500L)__________

(0.100mol)(0.0821 L∙atm/ mol∙K)0.0821 L∙atm/ mol∙K)

T(T(ººC) = 609K – 273C) = 609K – 273

= = 336 ºC336 ºC

Algebra Practice Algebra Practice Due by End of ClassDue by End of Class

Solve for x in the following problems (show Solve for x in the following problems (show allall work):work):

1)1)3x3x22 – 14 = 21 – 14 = 21

2)2)2x + 11x + 17 = 242x + 11x + 17 = 24

3)3)7x7x22 + 70y = 140 + 70y = 140

4)4)2(4x2(4x22 – 16) + 32 = 44 – 16) + 32 = 44

5)5)3(6x3(6x22 – 18) + 6x – 18) + 6x22 – 15 = 45 – 15 = 45

Turn in to Ms. Barrow and do Ideal Gas Law Turn in to Ms. Barrow and do Ideal Gas Law Worksheet (1-19 odds) when done.Worksheet (1-19 odds) when done.

Bell Work 3-4-13Bell Work 3-4-13

1. How many moles is 15 g of oxygen gas?1. How many moles is 15 g of oxygen gas?

2. The Goodyear blimp has 5.12 x 102. The Goodyear blimp has 5.12 x 1066 liters liters of helium at 25of helium at 25ooC and 1.00 atm. How many C and 1.00 atm. How many moles of helium are in the blimp?moles of helium are in the blimp?

Sodium and Chlorine Sodium and Chlorine VideoVideo

http://www.youtube.com/watch?http://www.youtube.com/watch?v=Mx5JJWI2aawv=Mx5JJWI2aaw

Agenda:Agenda:Gas Laws Practice ProblemsGas Laws Practice ProblemsGas laws using stoichiometryGas laws using stoichiometry

Objective:Objective:You will continue to UNDERSTAND how to You will continue to UNDERSTAND how to

use the ideal gas law.use the ideal gas law.

Gas Law ReviewGas Law ReviewWhat pressure will be exerted by 0.450 What pressure will be exerted by 0.450

moles of a gas at 25moles of a gas at 25ooC if it is C if it is contained in a vessel whose volume is contained in a vessel whose volume is 650 cm650 cm33??

What volume will 12.0 grams of neon What volume will 12.0 grams of neon gas occupy at 25gas occupy at 25ooC and a pressure of C and a pressure of 0.520 atm?0.520 atm?

STOICHIOMETRY: RECAPSTOICHIOMETRY: RECAPBalance the equation first!Balance the equation first!

NHNH33 + O + O22 NO + H NO + H22OO

How many grams of How many grams of HH22OO do I have if do I have if

I started with 4 grams of I started with 4 grams of OO22??

More ReviewMore ReviewAccording the equation below (balance first)–According the equation below (balance first)–

_H_H22SOSO44(aq)(aq)+_NaOH+_NaOH(aq)(aq)_H_H22OO(g)(g)+_Na+_Na22SOSO44(aq) (aq)

What would the moles of water be if 5.0 grams What would the moles of water be if 5.0 grams of Hof H22SOSO44 was reacted with NaOH? was reacted with NaOH?

What would the volume of gas be in the same What would the volume of gas be in the same reaction at 300K and 2.5atm?reaction at 300K and 2.5atm?

STOICHIOMETRY: RECAPSTOICHIOMETRY: RECAP 4NH4NH33 + 5O + 5O22 4NO + 6H 4NO + 6H22OO

How many grams of How many grams of HH22OO do I have if I do I have if I

reacted 4 grams of reacted 4 grams of OO2 2 w/ excess w/ excess NHNH33??

Gas Stoichiometry

What is the volume of CO2 produced at 37 ºC and 1.00 atm when 5.60 g of glucose are used up in the rxn:C6H12O6(s)+6O2(g) 6CO2(g)+6H2O(l)

PracticePracticeWhat volume of nitrogen can be produced by the What volume of nitrogen can be produced by the

decomposition of 50.0 g of NHdecomposition of 50.0 g of NH44NONO22 at 25 at 25C and C and

1.20 atm? 1.20 atm?

(HINT: You must write a balanced equation. (HINT: You must write a balanced equation. NHNH44NONO22 N N22 + H + H22OO ))

More Stoichiometry …More Stoichiometry …

4NH4NH33 + 5O + 5O22 4NO + 6H 4NO + 6H22OO

Using the above equation tell me how many Using the above equation tell me how many grams of grams of NONO do I have if I reacted 15 grams do I have if I reacted 15 grams of of OO2 2 w/ excess w/ excess NHNH33??

Check your grade!Check your grade!BELL WORK 3-5-13BELL WORK 3-5-13

How many moles of OHow many moles of O22 are in 20L are in 20L

of oxygen at 2.1 atm and 0of oxygen at 2.1 atm and 0°°CCWhat mass of Mg will burn in the below What mass of Mg will burn in the below

reaction? reaction?

Hint: write the balanced equation and you have Hint: write the balanced equation and you have moles of oxygen so now use a mole bridge to moles of oxygen so now use a mole bridge to

get there!!get there!!

Mg + OMg + O22 MgO MgO

Crushin’ Cans LabCrushin’ Cans Lab

#3 Could you have made the air inside the #3 Could you have made the air inside the can push outward? If so how?can push outward? If so how?

#4 why do you feel the wind when it blows, #4 why do you feel the wind when it blows, and what do you think causes it?and what do you think causes it?

More PracticeMore Practice

Many gases are available for use in Many gases are available for use in the laboratory in compressed gas the laboratory in compressed gas cylinders, in which they are cylinders, in which they are stored at high pressures. Let's stored at high pressures. Let's calculate the mass of Ocalculate the mass of O22 that can that can

be stored at 21ºC and 170 atm in a be stored at 21ºC and 170 atm in a cylinder with a volume of 60.0 L.cylinder with a volume of 60.0 L.

BELL WORKBELL WORKOn a new Bell Work Sheet labeled Bell On a new Bell Work Sheet labeled Bell

Work 2-28-11Work 2-28-11

In three sentences or more explain In three sentences or more explain how you could use your knowledge how you could use your knowledge of stoichiometry to find the volume of of stoichiometry to find the volume of HH22 gas produce at STP from 20.0g of gas produce at STP from 20.0g of

Mg given the following rxnMg given the following rxn..

MgMg(s) (s) + HCl+ HCl(aq) (aq) MgCl MgCl22(aq) (aq) + H+ H22(g)(g)

STOICHIOMETRY: RECAPSTOICHIOMETRY: RECAP

Grams AGrams A ( (÷÷ mol mass) mol mass)

moles Amoles A (mol B/ mol A) (mol B/ mol A)

moles Bmoles B ( (xx mol mol mass)mass)

Grams of BGrams of B

BELL WORK 2-21-12BELL WORK 2-21-12

What mass (think “moles What mass (think “moles first”) of carbon dioxide first”) of carbon dioxide will occupy 12.5 L at 10will occupy 12.5 L at 10C C and 1.75 atm?and 1.75 atm?

Standard Molar Volume: Standard Molar Volume: 1 mol = 22.4 L1 mol = 22.4 L

At STP an ideal gas occupies a At STP an ideal gas occupies a volume of 22.4 L/ mol.volume of 22.4 L/ mol.

So, what volume would 1.25 mole So, what volume would 1.25 mole of Hof H22 gas occupy at STP gas occupy at STP

1.25mol H1.25mol H22 x 22.4L/mol = x 22.4L/mol = 28 L

Review PracticeReview Practice3-7-133-7-13

1. How many grams is 2.1 mol of HCl?

2. How many moles is 3.1 grams of CH4?

3. Starting from an unbalanced equation, write down the steps to go from grams of A to grams of B .

Review PracticeReview Practice

If I have 5.6 liters of gas in a piston at a If I have 5.6 liters of gas in a piston at a pressure of 1.5 atm and compress the gas pressure of 1.5 atm and compress the gas until its volume is 4.8 L, what will the new until its volume is 4.8 L, what will the new pressure inside the piston be?pressure inside the piston be?

I have added 15 L of air to a balloon at sea I have added 15 L of air to a balloon at sea level (1.0 atm). If I take the balloon with level (1.0 atm). If I take the balloon with me to Denver, where the air pressure is me to Denver, where the air pressure is 0.85 atm, what will the new volume of the 0.85 atm, what will the new volume of the balloon be? balloon be?

Turn in the following:Turn in the following:

Determining the value of “R” LabDetermining the value of “R” Lab Ideal and Combined (white sheet) 1-20.Ideal and Combined (white sheet) 1-20. Chapter 18 review pg. 43 a & b, 44-47 Chapter 18 review pg. 43 a & b, 44-47

and page 481 1-5.and page 481 1-5. Gas Stoichiometry (white sheet) 1-10.Gas Stoichiometry (white sheet) 1-10. Chapter 19 review page 494-95 36a, Chapter 19 review page 494-95 36a,

37a, 38, 40, 46, 47, 52.37a, 38, 40, 46, 47, 52.

Can Crushn’!

bell work january 31 st , 2014

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