Gas Laws Formula Sheet Name - Whitwell High · Gas Laws Formula Sheet Name_____ CHEMISTRY ......

Gas Laws Formula Sheet Name______________

CHEMISTRY: A Study of Matter © 2004, GPB

9.1

P1V1 = P2V2 2

2

1

1

T

V

T

V=

2

22

1

11

T

VP

T

VP=

PV = nRT PT = P1 + P2 + P3…

1

2

2

1

d

d

v

v=

1

2

2

1

m

m

v

v=

R = 8. 314Kmol

kPaL

!

! R = 0.0821 Kmol

atmL

!

!

Water-Vapor Pressure Temp Pressure Pressure Temp Pressure Pressure

(°C) (mm Hg) (kPa) (°C) (mm Hg) (kPa)

0.0 4.6 0.61 24.0 22.4 2.98

5.0 6.2 0.87 25.0 23.8 3.17

10.0 9.2 1.23 26.0 25.2 3.36

15.0 12.8 1.71 27.0 26.7 3.57

16.0 13.6 1.82 28.0 28.3 3.78

17.0 14.5 1.94 29.0 30.0 4.01

18.0 15.5 2.06 30.0 31.8 4.25

19.0 16.5 2.19 35.0 42.2 5.63

20.0 17.5 2.34 40.0 55.3 7.39

21.0 18.5 2.49 50.0 92.5 12.23

22.0 19.8 2.64 60.0 149.4 19.93

23.0 21.1 2.81 70.0 233.7 31.18

Note Taking Guide: Episode 901 Name______________


9.2

Kinetic Theory

• Gases are composed of ____________, ____________ particles called ____________.

• Gas molecules are in ____________ ____________. • All ____________ between particles are ____________

____________. • The ____________ of a gas display no ____________ or

____________ for one another. • The ____________ ____________ ____________ of the molecules is

____________ _______________ to the ____________ temperature of the gas.

Ideal Gas

• Gas whose ____________ conforms to the ____________ ____________—it is ______________.

Gas Pressure:

Pressure = ____________

Atmospheric Pressure - the ____________ the earth’s

_______________ exerts due to its ____________.

Barometer: • Instrument used to measure ____________ ____________. • Invented by ____________


9.3

Normal Atmospheric Pressure • Also called ____________ ____________ • ____________ • ____________ • ____________ • ____________ STP: • ____________ ____________ and ____________ • ____________ • ____________ Manometer: • ____________ used to measure ____________ ____________ • U-shaped tube ____________ filled with ____________ • One end ____________ to ____________ ____________ • One end ____________ to ____________

The Chemistry Quiz

CR1. _____ CR2. _____ 1. _____ 2. _____

3. _____ 4. _____ 5. _____

Worksheet: Episode 901 Review Name______________


9.4

1. The theory that explains the behavior of gases at the molecular level is called the _______________ _______________ which is based on assumptions about a theoretical gas often referred to as an _______________ -_______________.

2. Gases deviate most from ideal gas behavior under conditions of very low

____________ and very high ____________. --The molecules of an ideal gas display no ____________ or ____________

for one another. --Under ordinary conditions, an ideal gas consists chiefly of ____________

space, which explains why gases are so easily compressed. -- Ideal gas particles travel in ____________ lines until they collide with each

other or with the walls of their container. --The collisions between the molecules of an ideal gas are completely

____________. --The average kinetic energy of the molecules of an ideal gas is ____________

proportional to the ____________ temperature of the gas. 3. A gas exerts pressure on the walls of its container because gas molecules

____________ with the walls of the container. So, the pressure exerted by a gas depends on two factors:

a) b) 4. To measure gas pressure an instrument called a _______________ is used. 5. The earth’s atmosphere has weight, which creates ____________

____________. 6. The instrument used to measure atmospheric pressure is the ____________.


9.5

7. Standard Temperature and Pressure (or _______________ ) is: ___________ K ___________ kPa ___________ atm ___________ °C ___________ mm Hg ___________ torr 8. At 1 atm, the height of the ____________ in a barometer is 760 mm. 9. A block of wood with a weight of 18 Newtons rests on a table top. How much

pressure is the block of wood exerting on the surface of the table directly beneath it if the block is 3 cm long and 2 cm wide?

10. Use the kinetic theory to explain why a helium filled balloon “shrinks” when it is

taken from a warm room to the outside on a cold day. 11. Use the kinetic theory to explain why bubble wrap pops when it is squeezed. 12. Use the kinetic theory to explain why tire pressure increases when more air is

added to a tire.



9.6

Boyle’s Law

• The ____________ of a fixed ____________ of gas varies ____________ with the ____________ at constant ____________.

• ____________ • ____________________ Kinetic Theory and Boyle’s Law

• ____________ of a gas is caused by the ____________ of the gas ____________ the walls of the ____________.

• If the gas is ________________ to _________ the volume it had, ____________ as many ____________ are present in any ____________ ____________. * ____________ as many ____________ per ____________ on the walls of the ____________ * ____________ of the gas will ____________

Ex 1: A balloon filled with Helium has a volume of 457 mL at standard atmospheric pressure. After the balloon is released, it reaches an altitude of 6.3 km where the pressure is only 65.5 kPa. What is the volume of the balloon at this altitude?

Ex 2: Under a pressure of _______ mm Hg, a confined gas has a volume of

_______mL. If the pressure is increased until the volume is ______ mL, what is the new pressure, assuming the temperature remains constant?


9.7

Charles’s Law

• For a ____________ ____________ of gas, as long as the ____________ is held ____________, the ___________ varies ____________ with the ____________ ____________. • ________________________ • ________________________

The Kelvin Temperature Scale

• ____________ zero * ____________ possible ____________ * ___________ been reached

• ____________ = absolute zero • ____________ = ____________ • K = ____________ Ex 1: A quantity of gas occupies a volume of 506 cm3 at a temperature of 147oC.

Assuming the pressure stays constant, at what temperature will the volume of the gas be 604 cm3?

Kinetic Molecular Theory and Charles’s Law

• ____________ the ____________ ____________ of a gas ____________ the average ____________ ____________ of its ____________.

• ____________ moving molecules * strike the walls of the ____________ ____________ ____________ * strike the walls of the ___________ with ____________ ____________

• From ____________ law we derive that the ____________ would have to ____________ if the ____________ ____________ is ____________ so that ____________ would remain ____________.

The Chemistry Quiz CR1. _____ CR2. _____ 1. _____ 2. _____ 3. _____ 4. _____ 5. ______

Rules for Scientific Graphing


9.8

1. Title the graph to indicate what relationship is represented.

2. Label each axis with units and the variable the axis represents.

Y-axis: dependent variable

X-axis: independent variable

3. Spread out data by using an appropriate scale.

4. Plot each point on the graph with a dot.

5. Connect plotted points using a best fit line or curve.

6. Use a key if plotting more than one set of data on one graph.

Lab: Boyle’s Law—Datasheet Name______________


9.9

Data: • Pressure is defined as force per unit area: P = Force/Area • When a book rests on top of the plunger, the pressure it exerts equals the

weight of the book divided by the area of the bottom of the plunger. Diameter of syringe =_______cm = _______m Weight (force) of 1 book =________N Calculate the area of the circle in m2 using the formula ∏r2:

Using the fact that pressure is defined as force ÷ area, what is the pressure exerted by 1 book in N/m2? If 1 N/m2 = 1 Pascal (Pa), what is the pressure exerted by 1 book in Pa? ________ Using conversion facts, convert Pa to kPa:

Exerting Pressure

Pressure (kPa)

Volume of Gas (cm3)

P/V (kPa/cm3)

P•V (kPa•cm3)

atmosphere

atmosphere + 1 book

atmosphere + 2 books





9.10

Use the graph paper below to make a graph of “pressure vs. volume”. Use proper technique for scientific graphing and be sure to draw a best-fit line. Conclusions: As the pressure exerted on the air inside the syringe increased, the volume (increased, decreased). Volume and pressure are (directly, inversely) proportional. Look at the last two columns of your data table. Within bounds of experimental error, the relationship between pressure and volume of a gas is (P/V = k , P•V = k). This relationship is known as __________________ ________________. (Look at the title of this lab!)

Lab: Charles’s Law—Datasheet Name______________


9.11

The following activity was performed in a classroom lab: • The plunger of a syringe, like the one used in the Boyle’s Law Lab, was pulled out

so that 5.0 cm3 of air was confined. • The syringe was then tightly capped so that the number of molecules of air

confined could not change. • Around the classroom, water baths at various temperatures were set up. • The capped syringe containing 5.0 cm3 of air was clamped into place in one of

the water baths so that the capped bottom of the syringe pressed against the bottom of the beaker containing the water bath.

• A thermometer was placed in the water bath beside the capped syringe. • Five minutes were allowed to pass so that the air in the syringe would equal the

temperature of the water bath. • The temperature of the water bath, and consequently the air inside the syringe,

was recorded as well as the volume of trapped air. • The process was repeated using the various water baths set up around the

laboratory. • Complete the chart below using the provided data. • Graphing:

Make a graph of temperature in degrees Celsius vs. volume on the graph paper provided.

Using a dotted line, extend the best-fit line to determine what temperature is required to theoretically reduce the volume of air to 0 cm3.

Temperature

( °C ) Volume ( cm3 )

Temperature ( K )

V/T ( cm3/°C )

V/T ( cm3/K )

0.0°C 4.6 20.0°C 5.0 40.0°C 5.3 80.0°C 6.0 100.0°C 6.3


9.12

Conclusions: 1. When a best-fit line is extended BEYOND plotted points, this is called

EXTRAPOLATION. According to your graph, at what temperature would the volume of your gas equal 0 cm3?

2. As the temperature of a gas increases, its volume (increases, decreases).

This means that the volume of a gas is (inversely, directly) proportional to its temperature when the _____________ is held constant.

3. The law describing the relationship between volume and temperature of a

gas is called _______________ law (look at the title of the lab). Mathematically, it can be stated V/T = k. Look at the last two columns of your data table. Which temperature scale must be used for this law?____________

4. Look at your graph. At 20°C the volume of your gas would be _____cm3. At

40°C the volume would be ______cm3. The temperature has doubled. Has the volume doubled?________ Explain this apparent contradiction to the law:

Worksheet: Boyle’s Law and Charles’s Law Name______________


9.13

1. Boyle’s Law: When ____________ is held constant, the pressure and volume of a gas are ____________ proportional.

2. Mathematically, Boyle’s law is stated PV = ____________ or P1V1 =

____________. 3. At a pressure of 405 kPa, the volume of a gas is 6.00 cm3. Assuming the

temperature remains constant, at what pressure will the new volume be 4.00 cm3?

4. A volume of gas at 1.10 atm was measured at 326 cm3. What will be the volume

if the pressure is adjusted to 1.90 atm? 5. If 36.5 m3 of a gas are collected at a pressure of 755 mm Hg, what volume will

the gas occupy if the pressure is changed to 632 mm Hg?


9.14

6. Charles’s Law: When ____________ is held constant, the volume and temperature of a gas are ____________ proportional.

7. Mathematically, Charles’s Law is stated: T

V = _____ or 1

1

T

V =______.

8. The ____________ temperature scale must be used in all gas law problems. 9. At 189 K, a sample of gas has a volume of 32.0 cm3. What volume does the gas

occupy at 242 K? 10. The gas in a balloon occupies 2.25 L at 298 K. At what temperature will the

balloon expand to 3.50 L? 11. A sample of gas has a volume of 852 mL at 25°C. What Celsius temperature is

necessary for the gas to have a volume of 945 mL?

Worksheet: More Boyle’s Law and Charles’s Law Name______________


9.15

Complete each of the following showing all work and circling your final answer on all problems. 1. To change a temperature expressed in degrees Celsius to a temperature on the

Kelvin scale, what must be done to the Celsius temperature?

Why must we use the Kelvin scale in gas law problems? 2. The volume of a sample of gas is 2.00 L when the temperature is 11.0 °C. While

the pressure remains constant, the temperature is changed to a new value, which causes the volume to become 3.00 L. What was the temperature changed to?

This is an example of ____________________’s Law. 3. The volume occupied by a sample of gas is 480 mL when the pressure is 115 kPa.

What pressure must be applied to the gas to make its volume become 650 mL?

This is an example of __________________’s Law. 4. The volume occupied by a sample of gas is 240.0 mL when the pressure is 1.20

atm. What volume, at constant temperature, will the gas occupy when the pressure is decreased to 0.860 atm?


9.16

5. The volume of a sample of gas is 25.0 mL when the temperature is 270 K. If the temperature is changed to 30.0 °C, what will be the new volume occupied by the gas assuming that the pressure remains constant?

6. When the volume of a sample of gas is divided by the temperature of the gas,

the result is 1.33 mL/K. The temperature of the gas is changed to a new value, which happens to be 411 K while the pressure is kept constant. What volume does the sample of gas occupy at 411 K?

7. When the pressure exerted by a sample of gas is multiplied by the volume

occupied by the sample, the result of this multiplication is 1.60 x 105 mm Hg·mL. The pressure exerted by the sample changes to a new value, which happens to be 750 mm Hg. What volume will the sample occupy at this pressure, assuming that temperature remains constant?



9.17

The Combined Gas Law

• Expresses the relationship between the ___________, ___________ and ___________ of a ___________ amount of ___________.

• ___________ or _______________________

Ex: A sample of gas has a volume of _____ L when its temperature is _____ K and its pressure is _____ mm Hg. What volume will the gas occupy at STP? V1 = ____________ V2 = ____________ T1 = ____________ T2 = ____________ P1 = ____________ P2 = ____________ Diffusion

• The ____________ spreading of a ____________

Graham’s Law of Diffusion

• Under the same conditions of ____________ and ____________, gases ____________ at a rate ____________ proportional to the ____________ ____________ of their ____________ (or ____________ ____________)

• ____________ or __________________


9.18

Ideal Gas Equation

• _______________ • New variables:

n = ____________ of gas in ____________ R = ____________ ____________ ____________ * ____________ constant * value depends on ________ used for ___________ and ____________ * value of R when using ____________ and ____________, R = ________________________

Ex: The average lung capacity for a female student is 3.9 L. At normal body temperature, 37oC, and 110 kPa, how many moles of air could her lungs hold?

P = __________ V = ____________ T = ____________ n = _____ R = ____________ Avogadro’s Law

• Equal ____________ of different ____________ under the ____________ conditions have the ____________ number of ____________.

• Conversely, if samples of ____________ ____________ at the same ____________ and ____________ contain the ____________ number of ____________, then the ____________ of all the ____________ must be ____________.

• At ____________, one ____________ of any gas occupies a ____________ of ____________.

• ____________ is the ____________ ____________ of a gas.


9.19

Ex. 3.2 moles of KNO3 are heated, producing O2 and KNO2. Calculate the volume of O2 in liters, that could be obtained at STP. Dalton’s Law of Partial Pressures

• The ____________ of a gas ____________ is the ____________ of the

____________ ____________ of each gas ____________.

• ________________________

Ex: Oxygen gas has been collected over water at a total pressure of 95.0 kPa and a temperature of 25oC. What is the pressure of the dry oxygen gas?

The Chemistry Quiz

CR1. _____ CR2. _____ 1. _____ 2. _____

3. _____ 4. _____ 5. _____

Lab: Graham’s Law of Diffusion—Datasheet Name______________


9.20

Introduction: The diffusion rates (velocities) of HCl and NH3 gases will be compared. Hydrogen chloride fumes will come from hydrochloric acid and ammonia fumes will come from aqueous ammonia. Both will be simultaneously introduced into opposite ends of a glass tube. When the gases meet, they will form a white precipitate, NH4Cl, which will form a ring in the tube. According to the _____________ theory, gas molecules are in constant motion, hitting each other and the sides of their container with perfectly ______________ collisions. The temperature of a gas is a measure of the average ______________ energy of the molecules. The equation for calculating this energy is: KE = ½ mv2 If two gases are at the same temperature, the molecules have the same average kinetic energy. This makes KE a (constant, variable). This means that m and v2 are ____________ proportional. Heavier molecules move (slower, faster) than light molecules at the same temperature. Mathematically, the relationship can be stated as:

m1v

1

2 = m2v

2

2 which equals v

1

2

v2

2 =

m2

m1

which equals v

1

v2

= m

2

m1

The last equation is known as Graham’s Law of Diffusion.


9.21

Procedure: 1. A drop of concentrated hydrochloric acid (a source of HCl fumes) was placed on

a cotton swab. A drop of concentrated aqueous ammonia was placed on another cotton swab.

2. The swabs were simultaneously inserted into opposite ends of a glass tube. 3. The glass tube was left undisturbed for two minutes. 4. After two minutes, a white ring was located and the center of the ring was

marked. 5. The distance from each end of the tube to the mark was measured.

HCl: d1 = __________ NH3: d2 = __________

6. Calculate the ratio d1/d2 = _________

This is also the ratio of the velocities of the molecules, v1/v2 .

v1

v2

= ______

7. Calculate the molar masses of the molecules:

HCl: m1 = __________ NH3: m2 = __________

8. Calculate the ratio:

m2

m1

=

9. Within bounds of experimental error, does

v1

v2

= m

2

m1

? ________

Worksheet: Combined Gas Law and Ideal Gas Law Name______________


9.22

1. A 952 cm3 container of gas is exerting a pressure of 108 kPa while at a temperature of 48 °C. Calculate the pressure of this same amount of gas in a 1236 cm3 container at a temperature of 64 °C.

2. At STP, a sample of gas occupies 24.5 mL. Calculate the volume of this gas at a

pressure of 2.3 atm and a temperature of 301 K. 3. A 3.25 L container of ammonia gas exerts a pressure of 652 mm Hg at a

temperature of 243 K. Calculate the pressure of this same amount of gas in a 2.50 L container at a temperature of 221 K.

4. A sample of gas has a volume of 5.23 cm3 at a pressure of 72.6 kPa and a

temperature of 25 °C. What will be the volume of the gas if the pressure is changed to 124 kPa and the temperature is changed to 0 °C?


9.23

5. Calculate the pressure (in kPa) of 0.421 mole of helium gas at 254 K when it occupies a volume of 3.32 L.

6. How many moles of argon are there in a 22.4 L sample of gas at 101.3 kPa and

0 °C? 7. What is the volume of 2.56 moles of gas at 0.634 atm and 65 °C? 8. A 500.0 g block of dry ice (solid CO2, molar mass = 44.0 g) vaporizes to a gas at

room temperature. Calculate the volume of gas produced at 25.0 oC and 1.50 atm.

Worksheet: Dalton’s Law, Avogadro’s Name______________ Hypothesis, Molar Volume


9.24

1. A) John ____________ was the first to form a hypothesis about partial ____________ of combined gases. After experimenting with gases, he concluded that each gas exerts the same pressure it would if it ____________ were present at the same temperature. If a gas is collected over water, the pressure in the container actually includes the sum of the vapor ____________ of the gas and the __________ vapor pressure. Consequently, we must ____________ the water vapor pressure from the total pressure to obtain the pressure of the ____________ alone.

B) A quantity of gas is collected over water at 20.°C. The manometer indicated a pressure of 34.6 kPa. What would be the pressure of the dry gas?

C) Determine the total pressure of a gas mixture that contains oxygen, nitrogen and helium if the partial pressures of the gases are: oxygen = 150 mm Hg, nitrogen = 350 mm Hg, and helium = 210 mm Hg.

2. A) Avogadro’s law states that equal volumes of different gases, at the same

____________ and ____________, contain the same ____________ of ____________.

B) According to Avogadro’s law, how will the number of molecules in 2 liters of hydrogen gas compare with the number of molecules in 2 liters of oxygen gas at the same temperature and pressure? ____________


9.25

C) Why is 22.4 liters called the molar volume of a gas?

D) In the following equation, what volume of hydrogen will produce 0.25 mole of NH3 at standard conditions of temperature and pressure?

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

E) When magnesium burns in the presence of oxygen, magnesium oxide is formed. How many moles of magnesium were burned if at STP, the magnesium was ignited in a 0.50 L container of oxygen gas?

Lab: Gas Laws Activity Day—Datasheet Name______________


9.26

1. Place a small amount of water (about 10 mL) in an empty soda can. Heat the can on your hot plate. After about one minute of VIGOROUS boiling, use the tongs to turn the can over (in one quick motion) and immediately place the mouth of the can in a bucket of cold water.

During boiling, the air originally in the can is replaced with __________ . Placing the can in the cold water causes the __________ to condense. (Decreasing the temperature of the gas causes its __________ and __________ to decrease.) A __________ results. The __________ pressure then crushes the can!

2. Be sure to do this over the sink!! Pour water into the glass container until it

overflows. Place the provided piece of paper over the mouth of the glass container. Hold the paper in place while you invert the glass. Remove your hand from the paper.

The water shouldn’t have spilled. WHY NOT? (What held the paper in place?)

3. Fill a 2-liter soft drink bottle to within 4 cm from the top. Half-fill a medicine

dropper with colored water. Drop the entire dropper into the bottle and screw the cap on tightly. Firmly squeeze the sides of the sealed bottle until the “diver” descends.

Look at the level of colored water in the medicine dropper. As the “diver” descends, the level of colored water (increases, decreases) as pressure increases. Thus, the volume of air in the dropper (increases, decreases) as pressure increases. The water rises in the dropper to take the place of the compressed __________. The dropper now has (more, less) mass and sinks. When the pressure is released, the volume of air in the dropper (increases, decreases), forcing the extra water from the dropper. The dropper now has (more, less) mass, and is buoyant again. This relationship between pressure and volume is an excellent example of __________ Law.


9.27

4. Over the sink, fill the film canister with water. A hole has been punched in the canister, so of course, water will exit the hole. Now place your hand firmly over the top of the canister. You may have to practice this a few times because you have to quickly place your hand over the top before all of the water runs out!

What happened when you placed your hand over the top of the can?

What was apparently “pushing” the water out of the hole? 5. When Joseph Kittinger rode a balloon to a height 18.5 miles in the sky, he ran

into trouble. At a height of 43,000 feet the pressure glove on his right hand failed to work. EXPLAIN what happened to his hand based on your knowledge of atmospheric pressure and the gas laws.

6. Calculate the pressure exerted by a 120 pound woman wearing high heels with a

surface area of 0.02 square inches as she walks across a wooden floor.

Review Sheet: Unit 9 Name______________


9.28

FILL IN THE BLANKS and SHORT ANSWER: 1. The theory that explains the behavior of gases at the molecular level is called

the _________ _____________ which is based on assumptions about a theoretical gas often referred to as an ___________ ____________.

2. Use the kinetic theory to explain why a helium filled balloon expands when it is

brought inside to a warm room from the cold outdoors.

3. Define “IDEAL GAS” 4. Gases deviate most from ideal behavior under conditions of very

___________temperature and very __________ pressure. 5. Pressure is defined as ___________ per unit ____________. The earth’s

atmosphere has weight, which creates ___________ ______________. 6. Standard temperature has been established as ____°C or______ K. Standard

pressure has been established as _________ atm, _______ torr, ________ mm Hg, or ________ kPa. The abbreviation for standard temperature and pressure is _______________.

7. A _______________ is used to measure atmospheric pressure, while a

_______________ is used to measure gas pressure. 8. When atmospheric pressure increases, how does the height of the column of

mercury change? 9. If pressure is constant, the volume of a sample of gas (increases, decreases) as

temperature increases. 10. At constant pressure, the volume of a sample of gas is ___________ proportional to temperature as measured on the_______________ temperature scale.


9.29

11. According to _______________ law, pressure and volume are _______________ proportional provided all other factors remain constant. Mathematically, this means that their _______________ is a constant.

12. The _______________ Gas Law permits calculation of any one term when

temperature, pressure, and volume change for a gas. 13. If A and B are directly proportional and the value of A becomes 1/3 as much,

what happens to the value of B? 14. State Avogadro’s law: 15. At STP, 22.4 L of N2 contain how many molecules? 16. Tire manufacturers recommend checking air pressure when tires are cold,

before driving. WHY? 17. Ammonia (NH3) and sulfur dioxide (SO2) are both gases with readily

distinguishable odors. If a cylinder of each were opened at the same time in a draftless room, which odor would you expect to smell first? EXPLAIN.

18. _______________Law of Partial _______________ states that in a mixture

of gases the total pressure of the mixture is equal to the _______________ of the pressures that each gas would exert by itself in the same volume.

19. Suppose you have 1 L of oxygen gas at a pressure of 1 atm, 1 L of nitrogen gas

at a pressure of 2 atm, and 1 L of hydrogen gas at a pressure of 3 atm. All 3 samples are at room temperature. If you transfer the oxygen and nitrogen to the container occupied by the hydrogen, the pressure exerted by the oxygen in the final mixture will be _______________. The pressure exerted by the mixture will be _______________ .

20. At STP, ___________ liters is the volume one mole of a gas occupies; this

quantity is consequently called the __________ volume of a gas.


9.30

PROBLEMS: SHOW SET-UP AND CIRCLE FINAL ANSWER. 1. What volume does 2.50 moles of carbon monoxide occupy at 50.5 kPa

pressure and 20.0 °C? 2. At 800 mm Hg, a gas has a volume of 380 L. What is its volume at standard

pressure? 3. A quantity of gas has a volume of 121 L when confined under a pressure of

2.50 atm at a temperature of 20.0 °C. At what pressure will its volume be 30.0 L at 25.0 °C?

4. At constant pressure, the volume of a gas is increased from 150.0 L to

300.0 L by heating it. If the original temperature of the gas was 20.0 °C, what will its final temperature (in Kelvins) be?

5. A quantity of gas is collected over water at 15 °C. The manometer indicated

a pressure of 24.0 kPa. What would be the pressure of the dry gas? 6. How many liters of pure oxygen at STP is consumed by a human being in 24

hours if the human body requires daily energy that comes from metabolizing 816 grams of sucrose (C12H22O11)?

C

12H

22O

11 (s) + 12 O

2 (g) ! "! 12 CO

2 (g) + 11 H

2O (l)

Gas Laws Formula Sheet Name - Whitwell High · Gas Laws Formula Sheet Name_____ CHEMISTRY ......

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