date% lesson% ngss% sol% activity/hw% assessment%...

Date% Lesson% NGSS% SOL% Activity/HW% Assessment%3/19/14% Boyle’s%Law%

%Charles’%Law%%GayBLussac’s%Law%

HSBPS3B2% CH.5%a% Engage:%%Shaving%Cream%in%Vacuum%Peeps%in%Vacuum%%Explore:%Lab%Activities%%

Formative:%Lab%techniques%and%experimental%design%

3/20/14% Continued% HSBPS3B2% CH.5%a% Explore:%Continued%%Explain:%Butcher%Paper%Discussion%%Elaborate:%Avogadro%Lab%brainstorm%%Evaluate:%Lab%Reports%%Engage:%Potato%Cannon%%

Lab%Reports%

3/21/14% Avogadro’s%Law%%Dalton’s%Law%%

HSBPS3B2% CH.5%a,%b% %Explore:%Lab%Activities%%Explain:%ThinkBPairBShare%with%other%groups%discussing%data%and%associated%gas%law%constants.%%Elaborate:%Gas%Law%RAFT%%

Lab%Reports%

Evaluate:%Lab%Reports%%

3/24/14% Ideal%Gas%Law% HSBPS3B2% CH.5%a,%b% Engage:%Variable%sort%%Explore:%Equation%manipulation%and%rearrangement%%Explain:%Class%discussion%of%gas%laws%and%mathematical%relationships%between%variables%%Elaborate:%Density,%molar%mass,%and%mole%fraction%rearrangements%miniBlecture%%Evaluate:%Gas%Law%HW%Problems%

Gas%Law%HW%Problems%

3/26/14% Graham’s%Law% HSBPS3B2% CH.5%b% Engage:%Comparison%of%golf%ball%and%bowling%ball%%Explore:%Student%run%diffusion%demos%%Explain:%miniBlecture%on%KE,%diffusion,%effusion%%

Molecular%Text%Messages%

Elaborate:%Molecular%Text%Messages%%Evaluate:%MTMs%%

3/27/14% Kinetic%Molecular%Theory%%Van%der%Waals%

HSBPS3B2% CH.5%a,%b% Engage:%Predraw%Talking%Drawing%%Explore:%Balloon%Pressure%scenarios%%Explain:%Particles%on%a%Stick%and%Talking%Drawing%%Elaborate:%ExchangeBCompare%Writing%%Evaluate:%Exchange%compare%samples%

Formative:%Their%knowledge/performance%during%particles%on%a%stick%

3/28/14% Test%Review% HSBPS3B2% CH.5%a,%b% Jigsaw:%Released%Free%Response%Questions%

%

3/31/14% Unit%Test%%

HSBPS3B2% CH.5%a,%b% % Unit%Test%

%%

Boyle’s,)Charles’,)and)Gay1Lussac’s)Laws)!Purpose! Students!will!develop!a!fundamental!understanding!of!the!

relationships!between!macroscopic!properties!of!a!gas!including!pressure!and!volume,!temperature!and!volume,!and!pressure!and!temperature.!!

SOL!!

!

CH.5!The!student!will!investigate!and!understand!that!!the!phases!of!matter!are!explained!by!kinetic!theory!!and!forces!of!attraction!between!particles.!Key!concepts!include:!!a)!!pressure,!temperature,!and!volume;!

!Materials!&!!Resources!

• Materials:!(per!group)!- Vernier!LabPro!- Gas!Pressure!Sensor!- 20!mL!syringe!- Logger!Pro!Software!- Student!chosen!supplies!(i.e.!glassware,!tubing,!etc.)!

!Safety!&!Management!

• Hotplates!and!gases!under!pressure!mean!students!should!wear!goggles!at!all!times.!Gloves,!or!hot!mitts!may!also!be!useful!to!some!groups.!

• !Engage!(10!min)!

Shaving!Cream!and!Peeps!in!Vacuum!• Engage!student!prior!knowledge!by!asking!probing!questions!

about!what!they!think!will!happen!and!why!!

Explore!(80!+!60!min)!

Lab!Activities!• See!student!activity!sheets!for!lab!instructions!• Student!groups!start!with!different!labs!and!rotate!making!

their!contribution!to!the!Butcher!Paper!Discussion!after!finishing!each!lab.!

• Concluding!paragraphs!are!to!be!done!as!homework.!!

Explain!(15!min)!

Butcher!Paper!Discussion!• After!each!lab!students!will!write!one!thoughtful!

contribution!on!the!piece!of!butcher!paper!labeled!with!the!corresponding!law.!

• At!the!end!of!lab!each!law!will!be!assigned!to!two!student!pairs.!They!will!be!given!three!minutes!to!discuss!the!conclusions!and!decide!what!to!share!out.!

• Each!group!has!two!minutes!to!share!out.!!

Elaborate! Avogadro’s!Lab!Brainstorm!

(15!min)! • Groups!begin!thinking!through!apparatus!and!approach!to!analyze!Avogadro’s!and!Dalton’s!Laws!!

Evaluate! Lab!conclusion!paragraphs!• Students!will!address!the!leading!questions!provided!in!the!

student!handouts!in!a!thoughtful!paragraph!that!demonstrates!their!understanding!of!the!gas!law.!

!

Name:&_______________________&

Boyle’s Law

Task: Investigate the relationship between the volume of a gas and the pressure it exerts. Required Outcomes:

1. Quantitative relationship between P and V. a. Based on at least 10 data points. b. Plot of P vs. V and P vs. 1/V c. Proportionality constant based on regression line or

plotted curve (use excel for data analysis). 2. Thoughtful paragraph demonstrating your understanding of

Boyle’s Law. a. Use the guiding questions to focus your thoughts b. Discussion of the sources of error or equipment

inadequacies in your experimental setup (excluding human error)

Potential Sample Data Table

Volume (mL) Pressure (kPa) P*V P/V

Questions to Consider 1. What do the two curves look like? What does the shape of each

curve tell you about the relationship between P and V (i.e. is it direct, inverse, exponential, etc.)?

2. Is the product or the quotient of P and V constant? Does this fact agree with your determination of the relationship between the two?

3. Use your computed constant (or it’s average) to add a line to the graph of P vs. V. How closely does it match your data?

4. Are there regions of the graph (your data points) that seem to buck the trend? What’s up with those points?

5. According to your P vs. V curve what happens to P at zero V? Does that make sense, does it agree with your intuition?

6. What happens to P at infinite V? Does that make sense, does it agree with your intuition?

Name:&_______________________&

Gay-Lussac’s Law

Task: Investigate the relationship between the temperature of a gas and the pressure it exerts. Required Outcomes:

1. Quantitative relationship between P and T. a. Based on at least 3 data points b. Plot of P vs. T and P vs. 1/T c. Proportionality constant based on regression line or


Gay-Lussac’s Law. a. Use the guiding questions to focus your thoughts b. Discussion of the sources of error or equipment


Potential Sample Data Table Temperature (K) Pressure (kPa) P*T P/T

Questions to Consider 1. What do the two curves look like? What does the shape of each

curve tell you about the relationship between P and T (i.e. is it direct, inverse, exponential, etc.)?

2. Is the product or the quotient of P and T constant? Does this fact agree with your determination of the relationship between the two?

3. Use your computed constant (or it’s average) to add a line to the graph of P vs. T. How closely does it match your data?


5. According to your P vs. T curve what happens to P at zero T? Does that make sense, does it agree with your intuition?

6. What happens to P at infinite T? Does that make sense, does it agree with your intuition?

Name:&_______________________&

Charles’ Law

Task: Investigate the relationship between the temperature of a gas and its volume. Required Outcomes:

1. Quantitative relationship between T and V. a. Based on at least 3 data points b. Plot of T vs. V and T vs. 1/V c. Proportionality constant based on regression line or


Charles’ Law. a. Use the guiding questions to focus your thoughts b. Discussion of the sources of error or equipment


Potential Sample Data Table

Temperature (K) Volume (mL) T*V T/V

Guiding Questions 1. What do your two curves look like? What does the shape of each

curve tell you about the relationship between T and V (i.e. is it direct, inverse, exponential, etc.)?

2. Is the product or the quotient of T and V constant? Does this fact agree with your determination of the relationship between the two?

3. Use your computed constant (or it’s average) to add a line to the graph of T vs. V. How closely does it match your data?


5. According to your T vs. V curve what happens to V at zero T? Does that make sense, does it agree with your intuition?

6. What happens to V at infinite T? Does that make sense, does it agree with your intuition?

Avogadro’s*and*Dalton’s*Laws*!

Purpose! Students!will!develop!a!fundamental!understanding!of!the!

relationships!between!macroscopic!properties!of!a!gas!and!the!amount!of!a!gas!including!how!the!number!of!moles!relates!to!

pressure!or!volume!and!whether!the!identity!of!a!gas!changes!this.!

Students!will!also!determine!whether!volumes/pressures!of!gases!are!perfectly!additive!when!two!gases!are!combined.!

!

SOL!!

!

CH.5!The!student!will!investigate!and!understand!that!!the!phases!of!matter!are!explained!by!kinetic!theory!!and!forces!of!attraction!

between!particles.!Key!concepts!include:!!

b)!partial!pressure!and!gas!laws;!

!

Materials!

&!!

Resources!

• Materials:!(per!group)!

- Vernier!LabPro!

- Gas!Pressure!Sensor!- 20!mL!syringe!

- Logger!Pro!Software!

- Student!chosen!supplies!(i.e.!glassware,!tubing,!etc.)!- Zn,!Mg,!CaCO3,!NaHCO3,!and!3M!HCl!

!

Safety!

&!

Management!

• Acid!=!Goggles.!!

• If!students!choose!to!study!pressure!they!must!understand!

that!it!is!especially!important!to!estimate!the!amount!of!gas!produced!and!the!resulting!pressure!to!avoid!an!explosion.!

!

Engage!(10!min)!

Potato!Cannon!• Engage!student!prior!knowledge!by!asking!probing!questions!

about!what!they!think!will!happen!and!why.!• Relate!their!reasons!back!to!previously!studied!gas!laws.!

• Show!the!chemical!reaction!that!occurs,!do!they!think!we!

have!accounted!for!the!dominant!effects?!!

Explore!

(70!min)!

Lab!Activities!

• See!student!activity!sheets!for!lab!instructions!• Student!procedures!must!be!teacher!approved!before!

beginning.!

• Concluding!paragraphs!are!to!be!done!as!homework.!!

Explain!(15!min)!

Think[Pair[Share!• How!proportionality!constants!compare!to!other!groups.!

• Compare!data!and!discoveries!with!another!group.!

• Each!group!share!out!one!discovery.!

!

Evaluate! Lab!conclusion!paragraphs!• Students!will!address!the!leading!questions!provided!in!the!

student!handouts!in!a!thoughtful!paragraph!that!

demonstrates!their!understanding!of!the!gas!law.!

!

Name:&_______________&&

Avogadro’s&&&Dalton’s&Laws&&

Task%1:&Investigate&the&relationship&between&the&amount&of&a&gas&(moles)&and&the&gases&pressure&(or&volume)&for&two&gases&of&your&choice.&& Required&Outcomes:&

1. Quantitative&relationship&between&moles&and&volume&&a. Based&on&at&least&two&trials&per&gas.&b. Proportionality&constant&&

2. Experimental&molar&mass&for&each&gas.&3. Discussion&of&the&sources&of&error&in&your&experimental&setup&(excluding&

human&error)&&

Gas&A:&_____________________&& Trial&1& Trial&2&Mass&& & &Pressure&(or&Volume&)& & &Moles&& & &&&

Gas&B:&_____________________&& Trial&1& Trial&2&Mass& & &Pressure&(or&Volume)& & &Moles& & &&&Task%2:&Determine&the&effect&mixing&your&two&gases&has&on&the&total&pressure&(or&volume)&of&the&system.&

1. Quantitative&relationship&describing&the&combination&of&gases.&a. Produce&a&data&table&(including&predictions)&

2. Discussion&of&the&sources&of&error&in&your&experimental&setup&(excluding&human&error)&

&& Trial&1& Trial&2&Pressure&(or&Volume)&of&gas&A& && &Pressure&(or&Volume)&of&gas&B& & &Predicted&Mixed&Pressure&(or&Volume)& & &Actual&Mixed&Pressure&(or&Volume)& & &&&Key%Points:%

1. Mr.&Mach&must&sign&off&on&your&proposal&before&you&begin&lab&work.&&Teacher&Initial:&___________&

2. Be&sure&to&include&both&tasks&in&your&procedures!&&

Name:&_______________&&

&&Safety:%

1. Goggles&should&be&worn&at&all&times&while&in&the&lab,&as&gases&generated&will&be&under&pressure&and&acids&and&bases&are&being&used!&

2. Care&should&be&taken&with&the&amount&of&reactants&used&to&be&sure&safe&amounts&of&gas&and&heat&are&produced.&

&&&&Relevant%Reactions:%

&&

&&

&

&

&&&Concluding%Paragraph:%Thoughtful&paragraph&demonstrating&your&understanding&of&Avogadro’s&and&Dalton’s&Law.&Use&the&guiding&questions&from&the&other&three&labs&(Boyle’s,&Charles’,&and&GayVLussac’s&Law)&to&focus&your&thoughts.&

1 Mg(s) + 2 HCl(aq) ��! 1 MgCl2(aq) + 1 H2 "

1 CaCO3(s) + 2 HCl(aq) ��! 1 CaCl2(aq) + 1 H2O(l) + 1 CO2 "

1 NaHCO3(s) + 1 HCl(aq) ��! 1 NaCl(aq) + 1 H2O(l) + 1 CO2 "

Gas$Law$RAFT$!

I!hereby!declare!that!this!weekend!all!members!of!AP!Chemistrydom!(even!those!peasants!traveling!vast!distances!via!chemically!powered!group!horses)!shall!write!a!decree!that!outlines!their!governance!as!a!Gas!Law!to!your!loyal!gas!particle!subjects.!This!decree!should!outline!your!style!of!governance!and!the!expectations!of!each!particle!individually!and!as!a!part!of!the!collective!whole.!This!document!created!using!your!electronic!book!from!the!future!(computer)!shall!be!presented!(due)!on!Monday.!!!

Summary$of$Assignment$(in$plain$English)$$

Role:$$ $ Gas!Law!Audience:$$ Gas!Particles!Everywhere!Format:! Decree!(scroll!style,!from!the!days!of!kings)$Topic:! Your!governance!and!expectations!of!each!

individual!and!the!community!as!a!whole.!!Vocabulary$(or$concepts)$to$be$included$in$your$RAFT:!

• CREATIVITY!!☺!• The!Variables!of!your!chosen!gas!law.!• Collisions!• Particle!Interactions!• Additional!concepts!as!desired!

!Your!RAFT!should!be!typed!and!is!due!on!Monday.!!

Ideal&Gas&Law&!Purpose! Students!will!understand!the!relationship!between!the!macroscopic!

observable!behavior!of!gases!and!mathematical!representations!commonly!utilized!in!calculations.!They!will!be!able!to!“derive”!uncommon!forms!of!the!ideal!gas!law!involving!variables!that!seem!obscure!and!unrelated!at!first!glance.!!

SOL!!

!

CH.5!The!student!will!investigate!and!understand!that!the!phases!of!matter!are!explained!by!kinetic!theory!!and!forces!of!attraction!between!particles.!Key!concepts!include:!!b)!partial!pressure!and!gas!laws;!


• Materials:!(per!student)!- Set!of!Variable!cards!- Equation!Mat!


• None.!!

Engage!(10!min)!

Variable!Sort!• Hand!out!decks!of!variable!cards!and!equation!mats!to!each!

student.!• Students!should!manipulate!the!variables!to!form!

mathematical!relationships!for!those!gas!laws!studied!previously.!!

Explore!(10!min)!

Equation!Manipulations!• Students!will!explore!differences!between!proportional!to!

and!equal!to.!• Students!will!recognize!the!links!between!the!simple!forms!of!

equations!based!on!their!experimental!experience!and!those!commonly!found!on!equation!sheets!or!textbooks.!!

Explain!(10!min)!

Class!Discussion!• Student!contributions!of!possible!equation!rearrangements.!• Questions!about!why!these!equations!work,!or!which!order!

the!variables!need!to!be!in.!!

Elaborate!(15!min)!

Advanced!Ideal!Gas!Law!Rearrangements!• Density!• Molar!Mass!• Mole!Fraction!• Dalton’s!Law!

Evaluate!(50)!

Gas!Law!HW!Problems!• Student!practice!using!the!equations!from!class!discussion.!

!

V (volume)

= n (amount of substance)

R (gas constant)

P (pressure)

T (temperature)

k (Boyle)

k (Gay-Lussac)

k (Avogadro)

P (pressure) = P

(pressure) = V

(volume) V (volume)

Name:

Gas Laws Homework Section 7.2: Pressure Measuring Devices

(7.17*) A jet educator is a piece of equipment used to draw gases from other equipment items. When operating on a condenser in a steam plant, the closed leg of a mercury manometer attached to the condenser is 692 mm above the open leg. What pressure is being maintained by the jet educator if atmospheric pressure is 743mm Hg?

Section 7.3: Boyle’s Law

(7.3) A gas is confined in a cylinder with a moveable piston at one end. When the volume of the cylinder is 682 ml the pressure of the gas is 1.33 atmospheres. What will the pressure be if the volume is reduced to 419 ml?

Section 7.6: Gay-Lussac’s Law

(7.5) A gas in a steel cylinder shows a gauge pressure of 355 pounds per square inch while sitting on a loading dock during a cold winter day when the temperature is -18°C. What pressure will the gauge show when the tank is brought inside and its contents warm up to 23°C?

(7.21*) A gas storage tank is designed to hold a fixed volume and quantity of gas at 1.74 atmospheres and 35°C. To prevent excessive pressure build-up by overheating, the tank is fitted with a relief valve that opens at 2.00 atmospheres. To what temperature must the gas rise in order to open the valve?

Name:

Section 7.7 & 7.8: Combined Gas Laws & Standard Temperature and Pressure

(7.6*) An industrial process yields 8.42 liters of NO at 35°C and 725 torr. What would be its volume if adjusted to STP?

(7.9) Superheated steam at 371°C and 51 atmospheres is delivered from the boilers of an ocean liner to its turbines, where it expands and propels the ship. At one point, one liter of starting steam will have expanded to 153 liters, and its pressure will have been reduced to 131 torr. Assuming compliance with the ideal gas laws, calculate the Celsius temperature at that point in the system.

(7.22*) A quantity of potassium chlorate is selected to yield, on complete thermal decomposition, 75.0 ml of oxygen, measured at STP. If the actual temperature is 28°C, and the actual pressure is 0.894 atmosphere, what volume of oxygen will result?

(7.24) A collapsible balloon for carrying meteorological testing apparatus aloft is partly filled with 282 liters of helium, measured at 25°C and 756 torr. Assuming the volume of the balloon is free to expand or contract according to changes in pressure and temperature, what volume will it have on reaching an altitude at which the temperature is -58°C and pressure is 0.641 atmosphere?

(7.25) In chemical processing plants hot exhaust gases are commonly sent through heat exchangers where they preheat an incoming reactant. In one such system 5.0 liters of exhaust gas at 274°C and 2.60 atmospheres expands to 74.9 liters at 1.12 atmospheres in passing though the heat exchanger. At what temperatures is the gas finally exhausted to the atmosphere?

Name:

Section 7.9: Ideal Gas Law

(7.10) A 9.81 liter cylinder contains 23.5 moles of nitrogen at 23°C. What pressure is exerted by the gas? Answer in atmospheres.

(7.11) A pressure 850 torr is exerted by 28.6 grams of sulfur dioxide at a temperature of 40°C. Calculate the volume of the vessel holding the gas.

(7.13*) At what Celsius temperature will argon have a density of 10.3 grams/liter and a pressure of 6.43 atmospheres?

(7.14*) Calculate the mass of ammonia in a 6.64 liter cylinder if the pressure is 4.76 atmospheres at a temperature of 25°C.

(7.15*) The density of an unknown gas at 20°C and 749 torr is 1.31 grams/liter. Estimate the molar weight of the gas.

Name:

(7.28) A 721 milliliter hydrogen lecture bottle is left with the valve slightly open. Assuming no air has mixed with the hydrogen, how many moles of hydrogen are left in the bottle after the pressure has become equal to an atmospheric pressure of 752 torr and a temperature of 22°C?

Section 8.2 : Molar Volume

(8.2) How many gams of nitrogen will be in a 1.50 liter flask at STP?

(8.3*) Find the STP density of neon.

(8.5*) When filled with an unknown gas at STP, a 2.10 liter vessel weights 2.63 grams more than it does when evacuated. Find the molar weight of the gas.

(8.25) Calculate the mass of 162 liters of chlorine, measured at STP.

(8.28*) A student evacuates a gas-weighing bottle and finds its mass to be 135.821 grams. She then fills the bottle with an unknown gas, adjusts the temperature to 0°C and the pressure to 1.00 atmosphere and weights it again at 136.201 grams. She then fills the bottle with water and finds is mass to be 385.42 grams. Find the molar weight of the gas.

Name:

Section 8.3: Molecular Formulas

(8.6*) Just above its boiling point at 445°C, sulfur appears to be a mixture of polyatomic molecules. Above 1000°C, however, there is but one structure. Determine the formula of molecular sulfur if its vapor density is 0.625 gram per liter at 1.10 atmospheres and 1100°C.

(8.7*) An organic compound has the following percentage composition: 55.8% carbon, 7.0% hydrogen, and 37.2% oxygen. 3.26 grams of the compound occupies 1.47 liters at 160°C and 0.914 atmosphere. Find the molecular formula of the compound.

(8.8*) Two compounds both contain 7.69% hydrogen and 92.31% carbon by weight. 4.35 grams of one, a gas at room conditions, occupies 4.16 liters at 22°C and 738 torr. The other, a liquid at room conditions, has a vapor density of 1.88 grams per liter at 195°C and 702 torr. Determine the molecular formula of each compound.

(8.30*) If 0.271 gram of the liquid rocket propellant hydrazine is vaporized at 748 torr and 180°C it occupies 320 milliliters. Analysis of the sample shows that it contains 0.0334 gram of hydrogen, and the balance is nitrogen. Calculate the molecular formula of hydrazine.

Section 8.4: Gas Stoichiometry

(8.33) The reaction chamber in a modified Haber process for making ammonia by direct combination of is elements is operated at 550°C and 250 atmospheres. How many grams of ammonia will be produced by the reaction of 75.0 liters of nitrogen if introduced at the temperature and pressure of the chamber?

Name:

(8.36) A major cause of smoke pollution is the incomplete combustion of coal and some of the complex ingredients in coal tar. The burning of naphthalene vapor (moth balls), C10H8, is an example. Shown with inert nitrogen to get a more accurate picture of air volume required the equation is C10H8 (g) + 12 O2 (g) + 48 N2 (g) 10 CO2 (g) + 4 H2O (g) + 48 N2 (g). How many liters of air at 764 torr and 16°C are required to burn one liter of naphthalene vapor, measured at 815 torr and 243°C? “Air” volume includes both oxygen and nitrogen.

Graham’s(Law(!Purpose! Students!will!understand!the!relationship!molecular!mass!and!

diffusion/effusion!rates.!!

SOL!!

!

CH.5!The!student!will!investigate!and!understand!that!the!phases!of!matter!are!explained!by!kinetic!theory!!and!forces!of!attraction!between!particles.!Key!concepts!include:!!b)!gas!laws;!


• Materials:!(per!student)!- Conc.!NH4OH,!Conc.!HCl,!phenolphthalein,!AgNO3!- QQtips!- Glass!tubes!


• Conc.!Acids!and!Bases!=!Goggles,!and!extreme!care.!!

Engage!(10!min)!

Golfing!with!Golf!balls!vs.!Bowling!balls!• Tell!students!that!I!brought!my!lucky!golf!club!and!ball.!

(show!them!the!putter!and!bowling!ball)!• Ask!them!why!this!is!ridiculous?!• What!about!the!bowling!ball!makes!using!it!for!golf!

impractical.!• Show!them!a!golf!ball.!• FollowQup,!why!is!a!putter!not!used!for!driving?!• Finish!with!the!expression!for!kinetic!energy.!

!Explore!(15!min)!

Diffusion!Demos!(student!run)!• Student!groups!receive!supplies!and!two!chemicals.!• Student!groups!set!up!and!perform!demos!for!the!rest!of!the!

class!and!explain!what!happens!and!why.!!

Explain!(15!min)!

MiniQLecture!• Equate!Temperature!to!Kinetic!Energy.!• Constant!temperature!leads!directly!to!comparison!of!masses!

and!velocities!• Introduce!Graham’s!Law!equation.!

!Elaborate!(50!min)!

Molecular!Text!Messages!• Students!will!formulate!a!message!to!send!their!friends!via!

diffusion.!They!must!correctly!account!for!the!differences!in!transmission!speed!among!the!characters!(elements)!in!their!message!and!utilize!a!delay!between!characters!to!send!an!

interpretable!message.!• See!Rubric!for!grading!criteria.!• Reminder:!Python!script!for!grading!takes!txt!input!and!

returns!messages,!speeds,!and!times.!Evaluate!!

MTMs!.!

!

Graham’s(Law(Using&the&chemicals&listed&below&and&the&apparatus&shown&in&class&setup&a&demo&of&Graham’s&Law&(diffusion).&Be&sure&to&make&a&prediction&and&discuss&plausible&explanations.&&

Conc.&NH4OH&Conc.&HCl&

&&&&&


Dilute&NaOH&Phenolphthalein&

Conc.&HCl&&&&&&


Conc.&NH4OH&Water&

Phenolphthalein&&&&&&


AgNO3&Conc.&HCl&

Name:______________'

Molecular)Text)Messages)Today'you’ll'be'sending'a'“molecular'text'message”'using'the'principle'of'diffusion.'You'may'use'text'slang'or'even'create'your'own'molecular'slang!'Messages'may'be'created'using'all'letters'in'the'atomic'symbol,'only'the'first'letter,'or'other'complicated'schemes.'''Assumptions:'

(1) All'species'are'gases'at'room'temperature.'(2) Your'fastest'diffuser'travels'from'you'to'the'recipient'in'1'second.'

'Example:'

I'HeArTc'CHEsMnInSTaRnY''H'is'the'fastest'diffuser'in'this'example;'we’ll'base'all'speeds'relative'to'this.'Consider'just'the'C,'H,'and'Es'of'“Chemistry”.'If'H'is'standardized'to'1'second'then'according'to'Graham’s'Law'C'diffuses'3.45'times'slower'(i.e.'it'takes'3.45'seconds)'and'Es'diffuses'15.88'times'slower'(i.e.'it'takes'15.88'seconds).'If'we'want'them'to'all'reach'our'recipient'simultaneously'we'should'release'the'Es'and'C'14.88'and'2.45'seconds'before'the'H'respectively.'However,'this'will'result'in'the'species'all'reaching'the'reader'simultaneously,'so'to'make'the'message'understandable'we’ll'delay'each'“letter”'by'0.1'seconds'for'its'desired'position.'So'Es'will'be'released'at'0.2'(0'+'0.2)'seconds,'we’ll'wait'12.23'(14.88'–'2.45)'seconds'to'release'C,'then'we’ll'wait'2.55'(2.45'+'0.1)'seconds'to'release'H'so'the'letters'arrive'in'the'order'C,'H,'Es.''Practice)Work)for)above)example:)'''''''''''''Hints:'

(1) Calculate'all'relative'speeds'first'(relative'to'your'fastest'diffuser)'(2) Figure'out'the'release'times'for'simultaneous'arrival'(negative'times'are'

useful'here)'(3) Adjust'the'timing'to'start'at'zero'(4) Adjust'the'timing'to'ensure'message'readability'(5) Create'a'scramble'(include'species'and'release'times)'on'separate'page'

'

Name:______________'

Molecular'Text'Messages'Rubric'Criteria' Evidence' Scoring'

Message'Encoding' 0]1'errors'='3'pts'2]3'errors'='2'pts'''''4'errors'='1'pts'''5+'errors'='0'pts'

'

Message'Length' 10'characters'='3'pts'''8'characters'='2'pts'''6'characters'='1'pts'''2'characters'='0'pts'

'

Work'' All'work'shown'='3'pts'All'work,'but'unclear'='2'pts'Partial'work'='1'pt'No'work'='0'pts'

'

Timeliness' Turned'in'on'or'before'deadline'1'pt'

'

'

Kinetic'Molecular'Theory'&'van'der'Waals'Equation'!Purpose! Students!will!understand!the!relationship!between!the!macroscopic!

observable!behavior!of!gases!and!events!occurring!at!the!molecular/particulate!level.!They!will!know!the!assumptions!that!underlie!the!ideal!gas!law!and!how!those!assumptions!can!be!used!to!build!a!more!realistic!representation!of!gas!behavior!(van!der!Waals!Eqn).!!

SOL!!

!

CH.5!The!student!will!investigate!and!understand!that!the!phases!of!matter!are!explained!by!kinetic!theory!!and!forces!of!attraction!between!particles.!Key!concepts!include:!!b)!partial!pressure!and!gas!laws;!


• Materials:!(per!student)!- Talking!Drawing!Form!- ExchangePCompare!Form!- Particles!on!a!stick!


• None.!!

Engage!(5!min)!

Talking!Drawing!(prePdraw)!• Students!will!draw!in!the!“prePReading”!box!a!picture!of!their!

current!understanding!of!gas!particle!behavior.!!

Explore!(20!min)!

Balloon!Pressure!Scenarios!• Students!will!be!shown!several!images!of!balloons!with!

molecules!arranged!in!different!ways!and!must!critique!these!representations!explaining!what!is!wrong!with!them,!why,!and!how!they!know.!

• Students!have!the!tendency!to!use!their!prior!school!knowledge!as!justification!rather!than!critically!thinking!about!what!they!actually!know!from!experience!and!logic!to!disprove!the!improper!representations.!You!must!demand!that!they!provide!justification!based!on!logical!reasoning!or!experience.!!

Explain!(10!min)!

Particles!on!a!stick!• Each!student!receives!a!particle!on!a!stick.!• In!their!groups!(tables!are!fine)!they!should!model!the!

behavior!of!solids,!liquids,!and!gases.!!• With!care!about!temperature!increases!this!can!also!show!

phase!changes,!and!the!idea!that!speed!is!directly!

Before Reading After Reading

Tell what has changed about your before reading and after reading pictures. Describe one way this new information will be helpful to you.

Talking Drawings

Exchange Compare Writing Form!

Group Members:

Part 1: Predict how the terms below might be used in Chapter 5.8 & 5.9 Real Gases.

van der Waals

interparticle interactions

high temperature particle volume

ideal gas real gas deviate/deviation low pressure

Part 2: Write your predicted passage in the space below.

! ! ! ! ! !

! ! ! ! ! ! ! ! ! ! ! ! !

! ! ! ! ! ! ! ! ! ! ! ! !

! ! ! ! ! ! ! ! ! ! ! ! !

! ! ! ! ! ! ! ! ! ! ! ! !

! ! ! ! ! ! ! ! ! ! ! ! !

! ! ! ! ! ! ! ! ! ! ! ! !

! ! ! ! ! ! ! ! ! ! ! ! ! !

Part 3: After reading, write your newly synthesized passage below.

! ! ! ! ! ! ! ! ! ! ! ! !

! ! ! ! ! ! ! ! ! ! ! ! !

! ! ! ! ! ! ! ! ! ! ! ! !

! ! ! ! ! ! ! ! ! ! ! ! !

! ! ! ! ! ! ! ! ! ! ! ! !

! ! ! ! ! ! ! ! ! ! ! ! !

! ! ! ! ! ! ! ! ! ! ! ! !

! ! ! ! ! ! ! ! ! ! ! ! ! !

Test%Review%!Purpose! Students!will!synthesize!their!understanding!of!individual!gas!laws!

and!incorporate!this!new!knowledge!into!their!previously!developed!chemical!understanding.!!

SOL!!

!

CH.5!The!student!will!investigate!and!understand!that!the!phases!of!matter!are!explained!by!kinetic!theory!!and!forces!of!attraction!between!particles.!Key!concepts!include:!!a)!pressure,!temperature,!and!volume;!b)!partial!pressure!and!gas!laws;!


• Materials:!(per!student)!- Released!AP!Free!Response!Questions!- Jigsaw!Flash!Cards!


• None.!!

Test!Review!(95!min)!

Jigsaw!• Students!will!be!given!challenging!free!response!questions!to!

solve!in!their!expert!groups.!Each!member!of!the!expert!group!must!fully!understand!the!solution!as!they!will!then!return!to!their!home!groups!and!explain!the!problem!and!solution!so!that!all!members!of!the!home!group!understand.!!

!

AP* Chemistry Name: ____________________________ Gas Law Quiz II Period:______________

AP® is a registered trademark of the College Board. The College Board was not involved in the production of and does not endorse this product. Test Questions are Copyright © 1962-2008 by College Entrance Examination Board, Princeton, NJ. All rights reserved. For face-to-face teaching purposes, classroom teachers are permitted to reproduce the questions. Web or Mass distribution prohibited.

Consider two containers of volume 1.0 L at 298 K, as shown above. One container holds 0.10 mol N2(g) and the other holds 0.10 mol H2(g). The average kinetic energy of the N2(g) molecules is 6.2 × 10í21 J. Assume that the N2(g) and the H2(g) exhibit ideal behavior. (a) Is the pressure in the container holding the H2(g) less than, greater than, or equal to the pressure in the

container holding the N2(g)? Justify your answer. (b) What is the average kinetic energy of the H2(g) molecules? (c) The molecules of which gas, N2 or H2, have the greater average speed? Justify your answer. (d) What change could be made that would decrease the average kinetic energy of the N2(g) molecules in

the container? (e) If the volume of the container holding the H2(g) was decreased to 0.50 L at 298 K, what would be the

change in each of the following variables? In each case, justify your answer.

(i) The pressure within the container

(ii) The average speed of the H2(g) molecules

____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________

____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________

AP* Chemistry Name: ____________________________ Gas Law Quiz I Period:______________

AP® is a registered trademark of the College Board. The College Board was not involved in the production of and does not endorse this product. Test Questions are Copyright © 1962-2008 by College Entrance Examination Board, Princeton, NJ. All rights reserved. For face-to-face teaching purposes, classroom teachers are permitted to reproduce the questions. Web or Mass distribution prohibited.

Answer the following questions related to hydrocarbons. (a) Determine the empirical formula of a hydrocarbon that contains 85.7 percent carbon by mass. (b) The density of the hydrocarbon in part (a) is 2.0 g L–1 at 50°C and 0.948 atm.

(i) Calculate the molar mass of the hydrocarbon.

(ii) Determine the molecular formula of the hydrocarbon.

(c) Two flasks are connected by a stopcock as shown below. The 5.0 L flask contains CH4 at a pressure of 3.0 atm, and the 1.0 L flask contains C2H6 at a pressure of 0.55 atm. Calculate the total pressure of the system after the stopcock is opened. Assume that the temperature remains constant.

(d) Octane, C8H18(l), has a density of 0.703 g mL–1 at 20°C. A 255 mL sample of C8H18(l) measured at 20°C reacts completely with excess oxygen as represented by the equation below.

2 C8H18(l) + 25 O2(g) ĺ 16 CO2(g) + 18 H2O(g)

Calculate the total number of moles of gaseous products formed.

Name: __________ ______________

Version A Period: ____________

(1) Test Questions are Copyright ¤ 1984-2002 by College Entrance Examination Board, Princeton, NJ. All rights reserved. For face-to-face teaching purposes, classroom teachers are permitted to reproduce the questions. Web or Mass distribution prohibited. (2) AP® is a registered trademark of the College Entrance Examination Board. The College Entrance Examination Board was not involved in the production of and does not endorse this product. Permission is granted for individual classroom teachers to reproduce the activity sheets and illustrations for their own classroom use. Any other type of reproduction of these materials is strictly prohibited.

1

AP* Chemistry: Gases

NO CALCULATORS MAY BE USED

Note: For all questions, assume that the temperature is 298 K, the pressure is 1.00 atmosphere, and solutions are aqueous unless otherwise specified.

Throughout the test the following symbols have the definitions specified unless otherwise noted.

Directions: Each set of lettered choices below refers to the numbered questions or statements immediately following it. Select the one lettered choice that best answers each question or best fits each statement and then fill in the corresponding oval on the answer sheet. A choice may be used once, more than once, or not at all in each set. Before turning in your answer sheet, count the number of questions that you have skipped and place that number next to your name ON YOUR ANSWER SHEET and circle it.

Questions 1 - 3 refer to the following gases at 0ºC and 1 atm.

(A) Ne (B) Xe (C) O2

(D) CO (E) NO

1. Has an average atomic or molecular speed closest to that of N2 molecules at 0ºC and 1 atm

2. Has the greatest density

3. Has the greatest rate of effusion through a pinhole

Question 4 refers to the following elements.

A) Lithium B) Nickel C) Bromine D) Uranium E) Fluorine

4. Is a gas in its standard state at 298 K

Version A

2

Directions: Each of the questions or incomplete statements below is followed by five suggested answers or completions. Select the one that is best in each case and then fill in the corresponding oval on the answer sheet.

5. When a sample of oxygen gas in a closed container of constant volume is heated until its absolute temperature is doubled, which of the following is also doubled?

A) The density of the gasB) The pressure of the gasC) The average velocity of the gas moleculesD) The number of molecules per cm3

E) The potential energy of the molecules

6. The density of an unknown gas is 2.00 grams per liter at 3.00 atmospheres pressure and 127°C. What is the molecular weight of this gas?

A) 254/3 RB) 188 RC) 800/3 RD) 600 RE) 800 R

7. Equal masses of three different ideal gases, X, Y, and Z, are mixed in a sealed rigid container. If the temperature of the system remains constant, which of the following statements about the partial pressure of gas X is correct?

A) It is equal to 1/3 the total pressure.B) It depends on the intermolecular forces of

attraction between molecules of X, Y, and Z.C) It depends on the relative molecular masses of

X, Y, and Z.D) It depends on the average distance traveled

between molecular collisions.E) It can be calculated with knowledge only of the

volume of the container.

8. Two flexible containers for gases are at the same temperature and pressure. One holds 0.50 gram of hydrogen and the other holds 8.0 grams of oxygen. Which of the following statements regarding these gas samples is FALSE?

A) The volume of the hydrogen container is the same as the volume of the oxygen container.

B) The number of molecules in the hydrogen container is the same as the number of molecules in the oxygen container.

C) The density of the hydrogen sample is less than that of the oxygen sample.

D) The average kinetic energy of the hydrogen molecules is the same as the average kinetic energy of the oxygen molecules.

E) The average speed of the hydrogen molecules is the same as the average speed of the oxygen molecules.

9. When the actual gas volume is greater than the volume predicted by the ideal gas law, the explanation lies in the fact that the ideal gas law does NOT include a factor for molecular

A) volumeB) massC) velocityD) attractionsE) shape

10. A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.50 mole of helium exerts a total pressure of 0.90 atmosphere. What is the partial pressure of the nitrogen?

A) 0.13 atm

B) 0.27 atm

C) 0.63 atm

D) 0.90 atm

E) 6.3 atm

Version A

3

11. A 2.00-liter sample of nitrogen gas at 27° C and 600. millimeters of mercury is heated until it occupies a volume of 5.00 liters. If the pressure remains unchanged, the final temperature of the gas is

A) 68° C

B) 120° C

C) 477° C

D) 677° C

E) 950.° C

12. A sample of 0.010 mole of oxygen gas is confined at 127°C and 0.80 atmosphere. What would be the pressure of this sample at 27°C and the same volume?

A) 0.10 atm

B) 0.20 atm

C) 0.60 atm

D) 0.80 atm

E) 1.1 atm

13. A sample of 3.0 grams of an ideal gas at 127°C and 1.0 atmosphere pressure has a volume of 1.5 liters. Which of the following expressions is correct for the molar mass of the gas? The ideal gas constant, R, is 0.08 (L � atm)/(mole �K).

A)[(0.08)(400)]

[(3.0)(1.0)(1.5)]

B)[(1.0)(1.5)]

[(3.0)(0.08)(400)]

C)[(0.08)(1.0)(1.5)]

[(3.0)(400)]

D)[(3.0)(0.08)(400)]

[(1.0)(1.5)]

E)[(3.0)(0.08)(1.5)]

[(1.0)(400)]

14. Samples of F2 gas and Xe gas are mixed in a container of fixed volume. The initial partial pressure of the F2 gas is 8.0 atmospheres and that of the Xe gas is 1.7 atmospheres. When all of the Xe gas reacted, forming a solid compound, the pressure of the unreacted F2 gas was 4.6 atmospheres. The temperature remained constant. What is the formula of the compound?

A) XeF

B) XeF3

C) XeF4

D) XeF6

E) XeF8

Version A

4

15.

The system shown above is at equilibrium at 28 °C. At this temperature, the vapor pressure of water is 28 millimeters of mercury. The partial pressure of O2(g) in the system is

A) 28 mm Hg

B) 56 mm Hg

C) 133 mm Hg

D) 161 mm Hg

E) 189 mm Hg

16. A sample of an ideal gas is cooled from 50.0°C to 25.0°C in a sealed container of constant volume. Which of the following values for the gas will decrease?

I. The average molecular mass of the gas

II. The average distance between the molecules

III. The average speed of the molecules

A) I only

B) II only

C) III only

D) I and III

E) II and III

17. At 25°C, a sample of NH3 (molar mass 17 grams) effuses at the rate of 0.050 mole per minute. Under the same conditions, which of the following gases effuses at approximately one-half that rate?

A) O2 (molar mass 32 grams)

B) He2 (molar mass 4.0 grams)

C) CO2 (molar mass 44 grams)

D) Cl2 (molar mass 71 grams)

E) CH4 (molar mass 16 grams)

18.

A hot-air balloon, shown above, rises. Which of the following is the best explanation for this observation?

A) The pressure on the walls of the balloon increases with increasing temperature.

B) The difference in temperature between the air inside and outside the balloon produces convection currents.

C) The cooler air outside the balloon pushes in on the walls of the balloon.

D) The rate of diffusion of cooler air is less than that of warmer air.

E) The air density inside the balloon is less than that of the surrounding air.

Version A

5

19. A rigid metal tank contains oxygen gas. Which of the following applies to the gas in the tank when additional oxygen is added at constant temperature?

A) The volume of the gas increase.B) The pressure of the gas decreases.C) The average speed of the gas molecules

remains the same.D) The total number of gas molecules remains the

same.E) The average distance between the gas

molecules increases.

20. NH4NO3(s) l N2O(g) + 2 H2O(g)

A 0.03 mol sample of NH4NO3(s) is placed in a 1 L evacuated flask, which is then sealed and heated. The NH4NO3(s) decomposes completely according to the balanced equation above. The total pressure in the flask measured at 400 K is closest to which of the following? ( The value of the gas constant, R, is 0.082 L atm mol–1 K–1)

A) 3 atmB) 1 atmC) 0.5 atmD) 0.1 atmE) 0.03 atm

21. Equal numbers of moles of He(g), Ar(g), and Ne(g) are placed in a glass vessel at room temperature. If the vessel has a pinhole-sized leak, which of the following will be true regarding the relative values of the partial pressures of the gases remaining in the vessel after some of the gas mixture has effused?

A) PHe < PNe < PAr

B) PHe < PAr < PNe

C) PNe < PAr < PHe

D) PAr < PHe < PNe

E) PHe = PAr = PNe

22. Which of the following gases deviates most from ideal behavior?

A) SO2

B) NeC) CH4

D) N2

E) H2

23. A flask contains 0.25 mole of SO2(g), 0.50 mole of CH4(g), and 0.50 mole of O2(g). The total pressure of the gases in the flask is 800 mm Hg. What is the partial pressure of the SO2(g) in the flask?

A) 800 mm HgB) 600 mm HgC) 250 mm HgD) 200 mm HgE) 160 mm Hg

24. In which of the following systems would the number of moles of the substances present at equilibrium NOT be shifted by a change in the volume of the system at constant temperature?

A) CO(g) + NO(g) p� CO2(g) + 12 N2(g)

B) N2(g) + 3 H2(g) p 2 NH3(g)

C) N2(g) + 2 O2(g) p 2 NO2(g)

D) N2O4(g) p 2 NO2(g)

E) NO(g) + O3(g) p NO2(g) + O2(g)

Version A

6

25. A hydrocarbon gas with an empirical formula CH2 has a density of 1.88 grams per liter at 0°C and 1.00 atmosphere. A possible formula for the hydrocarbon is

A) CH2

B) C2H4

C) C3H6

D) C4H8

E) C5H10

26. Under which of the following sets of conditions could the most O2(g) be dissolved in H2O(l)?

Pressure of O2(g) Temperature Above H2O(l) of H2O(l) (atm) (°C) A) 5.0 80B) 5.0 20C) 1.0 80D) 1.0 20E) 0.5 20

27. A compound is heated to produce a gas whose molecular weight is to be determined. The gas is collected by displacing water in a water-filled flask inverted in a trough of water. Which of the following is necessary to calculate the molecular weight of the gas, but does NOT need to be measured during the experiment?

A) Mass of the compound used in the experimentB) Temperature of the water in the troughC) Vapor pressure of the waterD) Barometric pressureE) Volume of water displaced from the flask

28. Hydrogen gas is collected over water at 24° C. The total pressure of the sample is 755 millimeters of mercury. At 24° C, the vapor pressure of water is 22 millimeters of mercury. What is the partial pressure of the hydrogen gas?

A) 22 mm Hg

B) 733 mm Hg

C) 755 mm Hg

D) 760 mm Hg

E) 777 mm Hg

29. In the laboratory, H2(g) can be produced by adding which of the following to 1 M HC1(aq)?

I. 1 M NH3(aq) II. Zn(s) III. NaHCO3(s)

A) I onlyB) II onlyC) III onlyD) I and II onlyE) I, II, and III

30. A sample of 9.00 grams of aluminum metal is added to an excess of hydrochloric acid. The volume of hydrogen gas produced at standard temperature and pressure is

A) 22.4 litersB) 11.2 litersC) 7.46 litersD) 5.60 litersE) 3.74 liters

Version A

7

31. An excess of Mg(s) is added to 100. mL of 0.400 M HCl. At 0ºC and 1 atm pressure, what volume of H2 gas can be obtained? A) 22.4 mLB) 44.8 mLC) 224 mLD) 448 mLE) 896 mL

32. The boiling points of the elements helium, neon, argon, krypton, and xenon increase in that order. Which of the following statements accounts for this increase? A) The London (dispersion) forces increase.B) The hydrogen bonding increases.C) The dipole-dipole forces increase.D) The chemical reactivity increases.E) The number of nearest neighbors increases.

33. A 2-L container will hold about 4 g of which of the following gases of 0ºC and 1 atm?

A) SO2

B) N2

C) CO2

D) C4H8

E) NH3

34. W(g) + X(g) l Y(g) + Z(g)

Gases W and X react in a closed, rigid vessel to form gases Y and Z according to the equation above. The initial pressure of W(g) is 1.20 atm and that of X(g) is 1.60 atm. No Y(g) or Z(g) is initially present. The experiment is carried out at constant temperature. What is the partial pressure of Z(g) when the partial pressure of W(g) has decreased to 1.0 atm?

A) 0.20 atmB) 0.40 atmC) 1.0 atmD) 1.2 atmE) 1.4 atm

35.

What volume of O2(g) is required to react with excess CS2(l) to produce 4.0 L of CO2(g) ? (Assume all gases are measured at 0ºC and 1 atm.)

A) 12 L

B) 22.4 L

C) 13 × 22.4 L

D) 2 × 22.4 L

E) 3 × 22.4 L

Name: __________ ______________

Version B Period: ____________


1








(D) CO (E) NO







Version B

2



A) SO2

B) NeC) CH4

D) N2

E) H2


A)[(0.08)(400)]

[(3.0)(1.0)(1.5)]

B)[(1.0)(1.5)]

[(3.0)(0.08)(400)]

C)[(0.08)(1.0)(1.5)]

[(3.0)(400)]

D)[(3.0)(0.08)(400)]

[(1.0)(1.5)]

E)[(3.0)(0.08)(1.5)]

[(1.0)(400)]

7. W(g) + X(g) l Y(g) + Z(g)




A) 22 mm Hg

B) 733 mm Hg

C) 755 mm Hg

D) 760 mm Hg

E) 777 mm Hg

Version B

3


A) PHe < PNe < PAr

B) PHe < PAr < PNe

C) PNe < PAr < PHe

D) PAr < PHe < PNe

E) PHe = PAr = PNe

10. NH4NO3(s) l N2O(g) + 2 H2O(g)



















Version B

4

15.


A) 12 L

B) 22.4 L

C) 13 × 22.4 L

D) 2 × 22.4 L

E) 3 × 22.4 L


A) 0.13 atm

B) 0.27 atm

C) 0.63 atm

D) 0.90 atm

E) 6.3 atm


A) CO(g) + NO(g) p� CO2(g) + 12 N2(g)

B) N2(g) + 3 H2(g) p 2 NH3(g)

C) N2(g) + 2 O2(g) p 2 NO2(g)

D) N2O4(g) p 2 NO2(g)

E) NO(g) + O3(g) p NO2(g) + O2(g)


A) SO2

B) N2

C) CO2

D) C4H8

E) NH3


A) 68° C

B) 120° C

C) 477° C

D) 677° C

E) 950.° C


A) CH2

B) C2H4

C) C3H6

D) C4H8

E) C5H10

Version B

5

21.


A) 28 mm Hg

B) 56 mm Hg

C) 133 mm Hg

D) 161 mm Hg

E) 189 mm Hg

22.








Version B

6





A) I only

B) II only

C) III only

D) I and III

E) II and III




A) 254/3 RB) 188 RC) 800/3 RD) 600 RE) 800 R








A) 0.10 atm

B) 0.20 atm

C) 0.60 atm

D) 0.80 atm

E) 1.1 atm




Version B

7












A) XeF

B) XeF3

C) XeF4

D) XeF6

E) XeF8




Name: __________ ______________

Version C Period: ____________


1








(D) CO (E) NO







Version C

2










A) I only

B) II only

C) III only

D) I and III

E) II and III


A) 22 mm Hg

B) 733 mm Hg

C) 755 mm Hg

D) 760 mm Hg

E) 777 mm Hg


A) 254/3 RB) 188 RC) 800/3 RD) 600 RE) 800 R


A) PHe < PNe < PAr

B) PHe < PAr < PNe

C) PNe < PAr < PHe

D) PAr < PHe < PNe

E) PHe = PAr = PNe

Version C

3


A) 0.10 atm

B) 0.20 atm

C) 0.60 atm

D) 0.80 atm

E) 1.1 atm


A) SO2

B) N2

C) CO2

D) C4H8

E) NH3


A)[(0.08)(400)]

[(3.0)(1.0)(1.5)]

B)[(1.0)(1.5)]

[(3.0)(0.08)(400)]

C)[(0.08)(1.0)(1.5)]

[(3.0)(400)]

D)[(3.0)(0.08)(400)]

[(1.0)(1.5)]

E)[(3.0)(0.08)(1.5)]

[(1.0)(400)]

14.













Version C

4

16.


A) 12 L

B) 22.4 L

C) 13 × 22.4 L

D) 2 × 22.4 L

E) 3 × 22.4 L


A) 68° C

B) 120° C

C) 477° C

D) 677° C

E) 950.° C









A) CH2

B) C2H4

C) C3H6

D) C4H8

E) C5H10


A) XeF

B) XeF3

C) XeF4

D) XeF6

E) XeF8

Version C

5




A) SO2

B) NeC) CH4

D) N2

E) H2


A) CO(g) + NO(g) p� CO2(g) + 12 N2(g)

B) N2(g) + 3 H2(g) p 2 NH3(g)

C) N2(g) + 2 O2(g) p 2 NO2(g)

D) N2O4(g) p 2 NO2(g)

E) NO(g) + O3(g) p NO2(g) + O2(g)



26.


A) 28 mm Hg

B) 56 mm Hg

C) 133 mm Hg

D) 161 mm Hg

E) 189 mm Hg


A) 0.13 atm

B) 0.27 atm

C) 0.63 atm

D) 0.90 atm

E) 6.3 atm

Version C

6







29. W(g) + X(g) l Y(g) + Z(g)















Version C

7



35. NH4NO3(s) l N2O(g) + 2 H2O(g)



Name: __________ ______________

Version D Period: ____________


1











(D) CO (E) NO




Version D

2



A) CO(g) + NO(g) p� CO2(g) + 12 N2(g)

B) N2(g) + 3 H2(g) p 2 NH3(g)

C) N2(g) + 2 O2(g) p 2 NO2(g)

D) N2O4(g) p 2 NO2(g)

E) NO(g) + O3(g) p NO2(g) + O2(g)





A) 0.13 atm

B) 0.27 atm

C) 0.63 atm

D) 0.90 atm

E) 6.3 atm


A) CH2

B) C2H4

C) C3H6

D) C4H8

E) C5H10


A) PHe < PNe < PAr

B) PHe < PAr < PNe

C) PNe < PAr < PHe

D) PAr < PHe < PNe

E) PHe = PAr = PNe


A) SO2

B) N2

C) CO2

D) C4H8

E) NH3

Version D

3

11.


A) 12 L

B) 22.4 L

C) 13 × 22.4 L

D) 2 × 22.4 L

E) 3 × 22.4 L





14.


A) 28 mm Hg

B) 56 mm Hg

C) 133 mm Hg

D) 161 mm Hg

E) 189 mm Hg







Version D

4




A) 254/3 RB) 188 RC) 800/3 RD) 600 RE) 800 R


A) XeF

B) XeF3

C) XeF4

D) XeF6

E) XeF8





A)[(0.08)(400)]

[(3.0)(1.0)(1.5)]

B)[(1.0)(1.5)]

[(3.0)(0.08)(400)]

C)[(0.08)(1.0)(1.5)]

[(3.0)(400)]

D)[(3.0)(0.08)(400)]

[(1.0)(1.5)]

E)[(3.0)(0.08)(1.5)]

[(1.0)(400)]

Version D

5




23.








A) SO2

B) NeC) CH4

D) N2

E) H2


A) 0.10 atm

B) 0.20 atm

C) 0.60 atm

D) 0.80 atm

E) 1.1 atm


A) 68° C

B) 120° C

C) 477° C

D) 677° C

E) 950.° C

Version D

6







A) 22 mm Hg

B) 733 mm Hg

C) 755 mm Hg

D) 760 mm Hg

E) 777 mm Hg

29. W(g) + X(g) l Y(g) + Z(g)







A) I only

B) II only

C) III only

D) I and III

E) II and III







Version D

7

32. NH4NO3(s) l N2O(g) + 2 H2O(g)












Name: ______________________________ AP* Chemistry: Gas Laws Period:_____________

(1) Test Questions are Copyright © 1984-2002 by College Entrance Examination Board, Princeton, NJ. All rights reserved. For face-to-face teaching purposes, classroom teachers are permitted to reproduce the questions. Web or Mass distribution prohibited. (2) AP® is a registered trademark of the College Entrance Examination Board. The College Entrance Examination Board was not involved in the production of and does not endorse this product. Permission is granted for individual classroom teachers to reproduce the activity sheets and illustrations for their own classroom use. Any other type of reproduction of these materials is strictly prohibited.

YOU MAY USE YOUR CALCULATOR

CLEARLY SHOW THE METHOD YOU USED AND STEPS INVOLVED IN ARRIVING AT YOUR ANSWERS. It is to your advantage to do this, because you may earn partial credit if you do and you will receive little or no credit if you do not. Attention should be paid to significant figures. Be sure to write all your answers to the questions on the lined pages following the question set.

1. Consider the hydrocarbon pentane, C5H12 (molar mass 72.15 g). (a) Write the balanced equation for the combustion of pentane to yield carbon dioxide and water.

(b) What volume of dry carbon dioxide, measured at 25°C and 785 mm Hg, will result from the

complete combustion of 2.50 g of pentane?

(c) The complete combustion of 5.00 g of pentane releases 243 kJ of heat. On the basis of this information, calculate the value of ǻH for the complete combustion of one mole of pentane.

(d) Under identical conditions, a sample of an unknown gas effuses into a vacuum at twice the rate

that a sample of pentane gas effuses. Calculate the molar mass of the unknown gas.

(e) The structural formula of one isomer of pentane is shown below. Draw the structural formulas for the other two isomers of pentane. Be sure to include all atoms of hydrogen and carbon in your structures.

2. A rigid 5.00 L cylinder contains 24.5 g of N2(g) and 28.0 g of O2(g).

(a) Calculate the total pressure, in atm, of the gas mixture in the cylinder at 298 K. (b) The temperature of the gas mixture in the cylinder is decreased to 280 K. Calculate each of the

following. (i) The mole fraction of N2(g) in the cylinder (ii) The partial pressure, in atm, of N2(g) in the cylinder


(c) If the cylinder develops a pinhole-sized leak and some of the gaseous mixture escapes, would the ୫୭୪ୣୱ�୭��మሺሻ୫୭୪ୣୱ�୭��మሺሻ

in the cylinder increase, decrease, or remain the same? Justify your answer. A different rigid 5.00 L cylinder contains 0.176 mol of NO(g) at 298 K. A 0.176 mol sample of O2(g) is added to the cylinder, where a reaction occurs to produce NO2(g).

(d) Write the balanced equation for the reaction.

(e) Calculate the total pressure, in atm, in the cylinder at 298 K after the reaction is complete.



Your responses to the rest of the questions in this part of the examination will be graded on the basis of the accuracy and relevance of the information cited. Explanations should be clear and well organized. Examples and equations may be included in your responses where appropriate. Specific answers are preferable to broad, diffuse responses.

3. Answer the following questions about carbon monoxide, CO(g), and carbon dioxide, CO2(g). Assume that both gases exhibit ideal behavior.

(a) Draw the complete Lewis structure (electron-dot diagram) for the CO molecule and for the CO2

molecule. (b) Identify the shape of the CO2 molecule. (c) One of the two gases dissolves readily in water to form a solution with a pH below 7. Identify the gas

and account for this observation by writing a chemical equation. (d) A 1.0 mole sample of CO(g) is heated at constant pressure. On the graph repeated below, sketch the

expected plot of volume versus temperature as the gas is heated.

(e) Samples of CO(g) and CO2(g) are placed in 1 L containers at the conditions indicated in the diagram below.

(i) Indicate whether the average kinetic energy of the CO2(g) molecules is greater than, equal to, or less than the average kinetic energy of the CO(g) molecules. Justify your answer.

(ii) Indicate whether the root-mean-square speed of the CO2(g) molecules is greater than, equal to,

or less than the root-mean-square speed of the CO(g) molecules. Justify your answer.

(iii) Indicate whether the number of CO2(g) molecules is greater than, equal to, or less than the number of CO(g) molecules. Justify your answer.

T (kelvins)

V (l

iters

)

Name: ______________________________ AP* Chemistry: Gas Laws Period:_____________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________

Name: ______________________________ AP* Chemistry: Gas Laws Period:_____________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________

Name: ______________________________ AP* Chemistry: Gas Laws Period:_____________ Question 3, part (d): ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________

T (kelvins)

V (l

iters

)

Name: ______________________________ AP* Chemistry: Gas Laws Period:_____________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________

GO ON TO THE NEXT PAGE. 2

INFORMATION IN THE TABLE BELOW AND IN THE TABLES ON PAGES 3-5 MAY BE USEFUL IN ANSWERING THE QUESTIONS IN THIS SECTION OF THE EXAMINATION.

D

O N

OT

DE

TA

CH

FR

OM

BO

OK

.

PE

RIO

DIC

TA

BL

E O

F T

HE

EL

EM

EN

TS

1 3 11 19 37

85.4

755

132.

9187 (223

)

4 12 20 38

87.6

256

137.

3388

226.

02

21 39

88.9

157

138.

9189

227.

03

22 40

91.2

272

178.

49

23 41

92.9

173

180.

95

24 42

95.9

474

183.

85

25 43 (98) 75

186.

21

26 44

101.

176

190.

2

27 45

102.

9177

192.

2

28 46

106.

4278

195.

08

29 47

107.

8779

196.

97

30 48

112.

4180

200.

59

5 13 31 49

114.

8281

204.

38

6 14 32 50

118.

7182

207.

2

7 15 33 51

121.

7583

208.

98

8 16 34 52

127.

6084 (209

)

9 17 35 53

126.

9185 (210

)

10 18 36 54

131.

2986 (222

)

H Li

Na K Rb

Cs

Fr

Be

Mg

Ca

Sr Ba

Ra

Sc Y *La

Ac

Ti

Zr

Hf

V Nb

Ta

Cr

Mo

W

Mn

Tc

Re

Fe

Ru

Os

Co

Rh Ir

Ni

Pd Pt

Cu

Ag

Au

Zn

Cd

Hg

110

(269

)

111

(272

)

112

(277

)

§§

§

B Al

Ga

In Tl

C Si Ge

Sn Pb

N P As

Sb Bi

O S Se Te

Po

F Cl

Br I At

Ne

Ar

Kr

Xe

Rn

He

104

(261

)

105

(262

)

106

(263

)

107

(262

)

108

(265

)

109

(266

)

Rf

Db

SgB

hH

sM

t

2

1.00

79

6.94

1

22.9

9

39.1

0

9.01

2

24.3

0

40.0

844

.96

47.9

050

.94

52.0

054

.938

55.8

558

.93

58.6

963

.55

65.3

9

10.8

11

26.9

8

69.7

2

12.0

11

28.0

9

72.5

9

14.0

07

30.9

74

74.9

2

16.0

0

32.0

6

78.9

6

19.0

0

35.4

53

79.9

0

20.1

79

39.9

48

83.8

0

4.00

26

5859

6061

6263

6465

6667

6869

7071

9091

9293

9495

9697

9899

100

101

102

Ce

Pr

Nd

Pm

SmE

uG

dT

bD

yH

oE

rT

mY

bL

u

Th

Pa

UN

pP

uA

mC

mB

kC

fE

sF

mM

dN

oL

r10

314

0.12

140.

9114

4.24

(145

)15

0.4

151.

9715

7.25

158.

9316

2.50

164.

9316

7.26

168.

9317

3.04

174.

97

232.

0423

1.04

238.

0323

7.05

(244

)(2

43)

(247

)(2

47)

(251

)(2

52)

(257

)(2

58)

(259

)(2

60)

*Lan

than

ide

Seri

es

†Act

inid

e Se

ries†

§Not

yet

nam

ed

rmccormick

rmccormick

rmccormick


ADVANCED PLACEMENT CHEMISTRY EQUATIONS AND CONSTANTS

E

v n

m

p

energy velocityfrequency principal quantum numberwavelength massmomentum

u

l

Speed of light, 3.0 10 m s

Planck’s constant, 6.63 10 J s

Boltzmann’s constant, 1.38 10 J K

Avogadro’s number 6.022 10 mol

Electron charge, 1.602 10 coulomb

1 electron volt per atom 96.5 kJ mo

8 1

34

23 1

23 1

19

1

l

c

h

k

e

�

�

�

�

� �

�

�

� �

�

�

�

Equilibrium Constants

(weak acid)

(weak base)

(water)

(gas pressure)

(molar concentrations)

K

K

K

K

K

a

b

w

p

c

S

H

G

E

T

n

m

q

c

C

E

k

A

p

a

D

D

D

D

standard entropy

standard enthalpy

standard free energy

standard reduction potentialtemperaturemolesmassheatspecific heat capacitymolar heat capacity at constant pressure

activation energy

= rate constant= frequency factor

Faraday's constant, coulombs per mole

of electrons

Gas constant, J mol K

L atm mol K

volt coulomb mol K

!

� �

� �

� �

96 500

8 31

0 0821

8 31

1 1

1 1

1 1

,

.

.

.

R

ATOMIC STRUCTURE

E hv c v

p m

En

n

� � �

l

lu

u= hm

2 178 10 18

2. joule

EQUILIBRIUM

K

K

K

a

b

b

=

=

=

+ −

− +

− + −

+ −

−

+

= ×= ×

= − = −= +

= +

= +

= − = −

== −

[ ] [ ][ ]

[ ] [ ][ ]

[ ] [ ] .

log [ ], log [ ]

log [ ][ ]

log [ ][ ]

log , log

( ) ,

H AHA

OH HBB

OH H @ 25 C

pH H pOH OHpH pOH

pH p AHA

pOH p HBB

p p

where moles product gas moles reactant gas

K

K

K

K

K K K K

K K RT

n

w

a

a

b

a a b b

p cn

1 0 10

14

14 D

D

D

THERMOCHEMISTRY/KINETICS

D

D D D

D D D

D D D

D D D

D

DD

S S S

H H H

G G G

G H T S

RT K RT K

n E

G G RT Q G RT Q

q mc T

C HT

f f

f f

p

D D D

D D D

D D D

D D D

D D

D

�

�

�

� � �

�

� �

Ç ÇÇ ÇÇ Ç

products reactants

products reactants

products reactants

ln . log

ln . log

2 303

2 303

!

ln lnA A

A A

t

t

kt

kt

� �

�

0

0

1 1

ln lnkER T

Aa � �1e j

rmccormick

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GASES, LIQUIDS, AND SOLUTIONS

1 1 2 2

1 2

1 2

2 1

2

2

2

,

( )

moles Awheretotal moles

...

K C 273

3 3

1 per molecule23 per mole2

molarity, moles solu

u

È ØÉ ÙÊ Ú

�

� �

� � �

�

D

M

M

MM

A total A A

total A B C

rms

P P

PV nRT

n aP V nb nRTV

X X

P P P P

mn

PV P V

T T

mDV

kT RTum

KE m

KE RT

r

r

M te per liter solutionmolality moles solute per kilogram solvent

molality

molality

D

D

p

� �

f f

b b

T iK

T iK

iMRTA abc

OXIDATION-REDUCTION; ELECTROCHEMISTRY

Q a b c d

Iqt

E E RTn

Q En

Q

K nE

c d

� � �

� �

[ ] [ ]

[ ] [ ]

ln . log @

log.

,C D

A Bwhere A B C D

C

cell cell cell

a b

D D D

D

!0 0592 25

0 0592

P

V

T

n

D

m

pressurevolumetemperaturenumber of molesdensitymassvelocityu

u

KE

r

i

K

K

Q

I

q

t

E

K

rms

f

b

Aabc

root-mean-square speed

kinetic energyrate of effusionmolar massosmotic pressurevan't Hoff factormolal freezing-point depression constant

molal boiling-point elevation constant

reaction quotientcurrent (amperes)charge (coulombs)time (seconds)

standard reduction potentialequilibrium constant

absorbancemolar absorptivitypath lengthconcentration

Mp

D

Gas constant, J mol K

L atm mol K

volt coulomb mol K

Boltzmann's constant, J K

for H O K kg mol

for H O K kg mol

STP C and atm

Faraday's constant, coulombs per mole of electrons

atm mm Hg

torr

R

k

K

K

f

b

�

� �

� �

� �

� �

�

�

8 31

0 0821

8 31

1 38 10

1 86

0 512

0 000 1 000

96 500

1 1

1 1

1 1

23 1

21

21

1 760760

.

.

.

.

.

.

. .

,

D

!

rmccormick

rmccormick

Unit%Plan%Reflection%

I"was"unsure"how"my"planned"activities"would"go"over"with"my"students"

because"they"are"used"to"learning"using"notes"delivered"via"PowerPoint"and"doing"

lots"of"in"class"practice"problems"as"a"whole"group."They"typically"do"a"lab"as"part"of"

each"unit"and"while"these"activities"are"demonstrative"of"important"lab"techniques"

and"skills,"only"occasionally"do"the"students"end"up"thinking"critically"or"being"

creative"to"study"an"aspect"of"the"lab"thoroughly."We"began"our"study"of"gas"laws"by"

plunging"straight"into"the"lab,"after"taking"a"pretest"to"determine"what"they"

remembered"from"first"year"chemistry"and"which"alternative"conceptions"remained."

Students"were"tasked"with"designing"appropriate"lab"setups"to"enable"them"to"

collect"data"and"determine"a"quantitative"relationship"between"the"pressure"and"

volume,"temperature"and"volume,"and"temperature"and"pressure"of"a"gas."All"groups"

used"Vernier"LabPro’s"and"Logger"Pro"software"to"collect"data"and"excel"to"plot"and"

analyze"their"findings."These"activities"met"NSTA"Standard"3b.""Throughout"the"

remainder"of"the"gas"laws"unit"we"performed"other"labs,"had"a"variety"of"discrepant"

events,"and"utilized"many"other"modes"of"learning"including"a"Talking"Drawing"

showing"pressure"at"the"particulate"level,"ExchangeJCompare"textbook"reading"

about"real"gases,"a"RAFT"writing"assignment"as"a"“gas"law”,"and"PowerPoint"based"

miniJlectures."These"various"approaches"to"instruction"gave"students"of"different"

abilities"and"academic"persuasions"activities"that"appealed"more"to"them,"or"enabled"

them"to"learn"in"their"desired"mode"and"met"INTASC"Standard"7.""

" During"the"first"day"of"lab"work"I"noticed"that"many"of"the"groups"were"

making"complex"and"creative"lab"setups"for"studying"the"gas"laws,"however,"these"

date% lesson% ngss% sol% activity/hw% assessment%...

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