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Unit 4A Study Guide

Gases in the Atmosphere

How does the composition of Earth’s atmosphere affect atmospheric properties and behavior?

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http://upload.wikimedia.org/wikipedia/commons/9/91/Atmosphere_composition_diagram.jpg

Date: ___________Right Now

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States of Matter pHeT Date: _____________Open the ChemSimulation Folder from the Desktop. Run the States of Matter Simulation. Resize the window so you can see the tabs on the top.

Part 1: Solid, liquid and gas.1. Click on solid, liquid and gas tabs for each molecule to compare and contrast the main properties of each state

of matter. Make sure you use the following words in your description: movement, volume, mass, space between molecules, collisions, and temperature.

Solid Liquid GasDrawing:

Description:

Drawing:

Description:

Drawing:

Description:

2. How are the three states of matter similar?

3. How are the three states of matter different?

Part 2: Phase Change (change the tab)4. Click on the water. Change the temperature and volume until you get the liquid phase. You will need to

monitor the state of matter by looking at the red dot on the phase diagram (lower right of the simulation). Explain what you did.

5. Hold on the “remove” heat button until the temperature reaches 0 K. What happens to the molecules?

6. Continue to remove heat. Does anything change? Explain.

7. Click “Reset All”. Add heat to double the temperature. What changes? (State at least three things.)

8. Click “Reset All”. Click on the finger and decreases the volume approximately 75% to the top of the particles. What changes? (State at least three things.)

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Understanding Phase Changes Date: ___________

1. Explain what happens in the following phase changes and determine if the change is endothermic (needs energy) or exothermic (releases energy).

Phase ChangeStarting State of Matter

goes from a …Ending State of Matter

to a …Endothermic or Exothermic

Melting

Freezing

Boiling

Condensing

Sublimation

2. What is needed for all phase changes?

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Date: ___________

Right Now

Quick Notes: Reading a phase diagram

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Reading Phase Diagrams Date: __________Use the phase diagram below to answer the questions.

1. Label each region of the phase diagram as solid, liquid or vapor.2. Label the triple point (TP), the critical point (CP), the boiling point (BP) and the melting point (MP).3. Label each line:a. Use the letter A to label the line that

gives the conditions for equilibrium between solid and liquid phases of bromine

b. Use the letter B to label the curve that gives the conditions for equilibrium between liquid and vapor phases of bromine,

c. Use the letter C to label the curve that gives the conditions for equilibrium between solid and vapor phases of bromine.

4. Draw arrows and label where sublimation (S), vaporization (V) , and melting (M) occur.

5. What is the temperature and pressure of the triple point?

6. What states of matter are present at the triple point?

7. What is the temperature and pressure of the critical point?

8. What states of matter are present above the critical point?

9. What is the temperature and pressure of the normal boiling point?

10. What is the temperature and pressure of the normal melting point?

11. What is the boiling point of bromine when the external pressure is 75 kPa?

12. Bromine vapor at 15°C (condenses, sublimes) when the pressure is raised to 50 kPa.

13. Bromine liquid at 70 kPa (vaporizes, freezes) then the temperature is decreased to -15°C.

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Note: Atmospheric pressure is equal to

101.3 kPa


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Properties and Pressure of Gases Date: __________Because atmospheric gases are generally colorless, odorless, and tasteless, you might doubt they are forms of matter; they seem to be “nothing.” However, gases do have definite physical and chemical properties, just as the materials in the other two states of matter— solids and liquids—do.

Activity Detailed Observations Explanation of what is going on Drawing of Gas Molecules

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Understanding the Variables : Use the internet to complete the following chart. Date: _______Variable What does it measure? Si Unit Symbol

Pressure

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Temperature

Volume

moles

Use some of the following terms to complete the paragraph below: mass, volume, shape, liquid, gas, constant.

The relationships between pressure temperature and volume are not always true for solids because the molecules in a

solid have fixed ________________ and ________________ therefore they cannot be compressed. Even though

________________ take up the space of their container, they still are not completely compressible because the volume

is ________________. However, the molecules in a _____________________ are so far apart that you can push them

closer together and they will spread out to fill the space they occupy so the relationships between temperature,

pressure and volume are always true.

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Pressure Questions Date: _________

1. Describe an activity or experience that suggests that air is matter. Remember, matter is something that has mass and takes up space.

2. Describe an activity or experience that suggests that air exerts pressure. Remember that pressure is force per area.

3. Circle the correct response in the following sentence: Pressure (increases / decreases) with height. Why?

4. Is each brick exerting the same total force on the ground? Explain.

5. Is each brick exerting the same pressure on the ground? Explain.

6. When you dip a straw into water, placed your finger on top of the straw, and then lifted the straw out of the liquid the liquid stays in the straw. When you remove your finger off of the top of the straw, the liquid comes out. Why does the liquid fall out of the straw when your hand is removed?

7. Which would hurt more: the heel of a 150 lb woman in high-heels steps on your foot or the heel of a 150 lb woman in gym shoes steps on your foot? Explain why.

8. THINK: Your middle ear is a closed container of air next to your ear drum. Your ear drum is pushed out as air pressure around you decreases. The opposite happens as the air pressure around you increases. Tubes connect your middle ear chamber to your mouth so air can leave/enter your middle ear to balance the pressure on your ear. Use this information to answer explain why people chew gum on airplanes.

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4A7 Reading Guide Date: _________Read about the Kinetic Molecular Theory (KMT) and take notes about the 4 main postulates.

Main Idea of Postulate Details of Postulate Analogy (This is similar to…)

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Modeling the Kinetic Molecular Theory Date: ________1. Molecules are always moving. Describe the amount of kinetic energy of each state of matter.

a. Solid: _____________

b. Liquid: _____________

c. Gas: _____________

2. On the graph below, write the labels “lower temperature” and “higher temperature”.

Imagine that you cause 8 to 10 highly elastic, small “super-bounce balls” to bounce around inside a box that you steadily shake; this serves as an analogy for gas molecules randomly bouncing around inside a sealed container. The balls bounce randomly around inside the box. Use this situation for the questions below.

3. Draw what the “super-bounce balls” would look like at each state.

4. Match the four gas variables to the following factors in the “super-bounce balls” analogy

____ the number of super-bounce balls in the box

____ the size of the box

____ the vigor with which you shake the box

____ the number of collisions with the box walls

a. Volume

b. Temperature

c. Pressure

d. Number of moles

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Solid Liquid Gas

5. How does each of the following changes in the “super-bounce balls” analogy relate to what you have learned about gases and the kinetic molecular theory?a. The amount of shaking and the number of super-bounce balls remain the same, but the size of the box is

decreased.

b. The size of the box and the number of super-bounce balls remain the same, but the shaking becomes more energetic.

c. The size of the container and the amount of shaking are kept the same, but the number of super-bounce balls is increased.

d. Use the “super-bounce balls” to explain what happens when the kinetic energy is increased.

6. Use the kinetic molecular theory to explain why gas particles take the volume of their container.

7. All analogies have limitations or problems. Come up with two limitations for using “super-bounce balls” as gas particles.

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Unit 4A.8 & A.11 Content Reading Guide Date: ________Compare Boyle’s and Charles’ Laws in the chart below.

Boyle’s Law Charles’ Law

What properties are kept constant? (Temperature, Pressure, Volume)

What properties are changed? (Temperature, Pressure, Volume)

Describe a situation that illustrates each law.

Write a formula that shows the relationship between the variables.

What variables must be controlled for the above relationships to be observed?

Sketch a graph describing each law, and label the axes.

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Boyle’s and Charles’ Law Date: __________1. Boyle’s Law is a relationship between _____________________ and _____________________.

a. Draw the shape of the graph.

b. It is a(n) _____________________ relationship.

c. As P increases, V_____________________.

d. The equation for Boyle’s Law is _____________________.

e. When using Boyle’s Law, you measure the initial _________________(____) and

_________________(____). Then you change either _________________(____) or

_________________(____) and use the equation to calculate the fourth measurement (x).

f. If the pressure is doubled, the volume __________________________________________.

g. If the pressure is reduced by a third, the volume __________________________________________.

2. Charles’ Law is a relationship between _____________________ and _____________________.



c. As T increases, V_____________________.

d. The equation for Charles’ Law is _____________________.

e. When using Charles’ Law, you measure the initial _________________(____) and


_________________(____) and use the equation to calculate the fourth measurement (x).

f. If the temperature is doubled, the volume __________________________________________.

g. If the temperature is reduced by a third, the volume _______________________________________.

h. When the temperature is 0oC molecules _____________________, and there ____ volume. When the

temperature is 0 K, called _____________________, molecules _____________________, and there

____ volume.

i. When you use Charles’ Law you always need the temperature to be in ___________________________.

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Practice Problems for Boyle’s and Charles’ Laws Date: __________3. A sample of 100.0 mL of oxygen has a pressure of 4 atm. The pressure is then changed to 9.91 atm. Assume that temperature remains constant.

a. Should you use Boyle’s or Charles’ Law? Think about what variables are given.

b. Predict whether the volume will increase or decrease. Think about the relationship between the variables.

c. What is the new volume of the gas? Calculate the missing variable. Show your work!

4. A flask containing 95.0 mL of hydrogen was collected at a pressure of 0.5 atm. At what pressure would the volume of hydrogen be 70.0 mL? Assume that temperature remains constant.


b. Predict whether the pressure will increase or decrease. Think about the relationship between the variables.

c. What is the new pressure of the gas? Calculate the missing variable. Show your work!

5. The temperature of a gas is 0.0 °C and the temperature is changed so the gas volume increases from 13 mL to 26 mL.


b. Predict whether the temperature will increase or decrease. Think about the relationship between the variables.

c. What is the new temperature of the gas? Calculate the missing variable. Show your work!

6. A gas has a volume of 10.0 L at 273K. What volume will the gas occupy if the temperature increases to 298 K? a. Should you use Boyle’s or Charles’ Law? Think about what variables are given.

b. Predict whether the volume will increase or decrease. Think about the relationship between the variables.

c. What is the new volume of the gas? Calculate the missing variable. Show your work!21

Date: ______________Right Now

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Gay-Lussac’s and Avogadro’s Laws Date: __________

1. Gay-Lussac’s Law is a relationship between ___________________ and ___________________.



c. As T increases, P_____________________.

d. The equation for Gay-Lussac’s Law is _____________________.

e. When using Gay-Lussac’s Law, you measure the initial _________________(____) and


_________________(____) and use the equation to calculate the fourth measurement.

f. If the pressure is doubled, the temperature __________________________________________.

g. If the pressure is reduced by a third, the temperature ________________________________________.

2. Avogadro’s Law is a relationship between ___________________ and ____________________.



c. As n increases, V_____________________.

d. The equation for Avogadro’s Law is _____________________.

e. When using Avogadro’s Law, you measure the initial _________________(____) and


_________________(____) and use the equation to calculate the fourth measurement.

f. If the number of moles is doubled, the volume __________________________________________.

g. If the number of moles is reduced by a third, the volume _____________________________________.

3. Of the four gas laws, which ones have an equation in which you divide? Do these laws have a direct or indirect

relationship?

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Practice Problems for Gay-Lussac’s and Avogadro’s Laws Date: ______________4. A sample of gas has a pressure of 1 atm at 278 K. If the gas is cooled to 33K, what is the new pressure? Assume that volume remains constant.

a. Should you use Gay-Lussac’s Law or Avogadro’s Law?

b. Predict whether the pressure will increase or decrease.

c. What is the new pressure of the gas?

5. A sample of gas has a volume of 3500 mL containing 1.2 moles. If gas is added to the container so the sample has 1.8 moles, what is the new volume?


b. Predict whether the volume will increase or decrease.

c. What is the new volume of the gas?

6. What will be the new volume of a 25 L sample of gas containing 2000 moles that is reduced to 1500 moles?a. Should you use Gay-Lussac’s Law or Avogadro’s Law?

b. Predict whether the volume will increase or decrease.

c. What is the new volume of the gas?

7. If a sample of gas has a pressure of 0.92 atm at 283 K, what will be its temperature when the pressure is increased to 1.08 atm?


b. Predict whether the temperature will increase or decrease.

c. What is the new pressure of the gas?

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Mixed Gas Law Practice #1 Date: ________For each question: Underline the variables that are changing, identify the gas law that describes the change, write the equation, predict what should happen, and calculate the unknown value. Assume that the variables not given are kept constant. SHOW YOUR WORK!!!

1. A sample of gas at 310 K has a pressure of 1.3 atm. If the temperature is cooled to 255 K, what will its new pressure be?

a. Circle the variables that change: P, V, n, Tb. Circle the variables that are constant: P, V, n, Tc. Which gas law should you use? What is the equation?

d. The new value for the unknown will be _____________ (larger or smaller).e. Calculate unknown value.

2. A flask containing 95.0 mL of hydrogen was collect at 0.878 atm. At what pressure would the volume of hydrogen be 70.0 mL?



3. A 50 L sample of gas contains 1.2 moles. Additional gas is added until it reaches a volume of 95 L. How many moles will be in the container?



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4. A sample of gas containing 2 moles has a volume of 44 L. If the number of moles is reduced to 0.5 moles, what will its new volume be?



5. A gas with a volume of 3.5 L at a pressure of 199 kPa is allowed to expand to a volume of 9.5 L. What is the pressure in the container?



6. Determine the pressure change when a constant volume of a gas at 1.00 atm is heated from 20.0 ⁰C to 30 ⁰C.a. Circle the variables that change: P, V, n, Tb. Circle the variables that are constant: P, V, n, Tc. Which gas law should you use? What is the equation?


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QN: Ideal Gas Law Date: ____________

1. An Ideal Gas is a perfect gas because it ______________________________________________________ ,

which means the following rules apply:

a. _____________________________________________________________________________________

b. _____________________________________________________________________________________

c. _____________________________________________________________________________________

d. _____________________________________________________________________________________

2. Real Gases are not Ideal Gases because:

a. At low temperatures ____________________________________________________________________

b. At high pressures ______________________________________________________________________

3. An Ideal Gas obeys the equation: ________________________________a. Where the gas constant, R, is

________________ if Pressure is in atm, Volume is in L, and Temperature is in K

________________ Pressure is in kPa, Volume is in L, and Temperature is in K.

4. You will need the following key conversions:

a. ⁰C K: ________________________________

b. mL L: ________________________________

c. mass moles: ________________________________

5. However, the ideal gas law can be used under ordinary conditions to predict properties of gases, because the deviations from Ideal Gas behavior ______________ that they can be neglected

6. Calculating moles of gas:

A 50 L cylinder is filled with argon gas to a pressure of 1 atm at 30oC. How many moles of argon gas are in the cylinder?

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Helpful Hints:

Temperature needs to be in Kelvin.n is really total moles; if you are given more than one value for moles, add them up.700 mmHg = 0.92 atm16 g of O2 = 0.5 mols O2

2.P=V=n=R=T=

Units of answer:

3.P=V=n=R=T=

Units of answer:

1.P=V=n=R=T=

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4.P=V=n=R=T=

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5.P=V=n=R=T=

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6.P=V=n=R=T=

Units of answer:

7.P=V=n=R=T=

Units of answer:

Ideal Gas Law Practice Problems: Show your work for 7 problems in the spaces below.http://www.sciencegeek.net/Chemistry/taters/Unit5IdealGasLaw.htm

Go to the sciencegeek.net homepage Choose Chemistry Review Problems on the left Scroll down to unit 5 and click on Ideal Gas Law Problems.

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http://www.sciencegeek.net/Chemistry/taters/Unit5IdealGasLaw.htm

4A19 Supplement: The Ideal Gas Law Date: ___________Solve the following problems, using the ideal gas equation. SHOW YOUR WORK!!!!

1. What volume will 2.50 mol of hydrogen (H2) occupy at -20.0 °C and 1.5 atm?

Volume = __________________

2. How many moles of sulfur dioxide are held inside a 67.4 L canister at a pressure of 0.25 atm and a temperature of 40.0 °C?

Moles = __________________

3. At what temperature will a .450 L vessel hold 4.0 mol carbon dioxide (CO2) at a pressure of 1.25 atm?

Temperature = __________________

4. A neon light bulb (cylinder shaped, with a volume of 0.0260 L) at 0.0 °C and 1 atm contains how many moles of gas?

Moles = __________________

5. A balloon contains 12.5 moles of helium (He) gas at room temperature (25 °C) and occupies a volume of 75.0 L. How much pressure does the He gas exert on the walls of the balloon?

Pressure = __________________

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Unit 4A Review

1. From your observations in this section, cite evidence for the following statements.Statement Evidence

a. Air is composed of matter

b. Air exerts pressure

2. What is pressure?

3. What is the relationship between pressure and area?

4. What happens to the air pressure as you increase the altitude?

5. The air pressure at sea level is 1 atm. Can you ever have an air pressure more than 1 atm?

6. Complete the following table by describing the arrangement of, motion of, and attractive forces between particles in each of the three states of matter:

7. When using the gas laws, what unit should you use for each of the following variables?

a. Volume: ______

b. Pressure: ______

c. Temperature: ______

d. Moles: ______

8. Fill out the table comparing variables involved in the gas laws.

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State of Matter Drawing of Molecules Relative Speed of Molecules

Relative Intermolecular

Attractive Forces

Solid

Liquid

Gas

Variables Gas Law Graph Description of the Relationship

Pressure and Volume

Pressure and Temperature

Volume and Temperature

Volume and Moles

9. The volume of a container is halved. What will happen to the pressure, if temperature remains constant?

10. The pressure of the air in a scuba diving tank is 24 atm. What is the pressure of the tank when the temperature triples?

11. If a gas in a closed container is pressurized from 15.0 atm to 16.0 atm and its original temperature was 25.0 ⁰C, what would the final temperature of the gas be?

12. A balloon contains 30.0 L of helium gas when the atmospheric pressure is 1 atm. What will the volume of the balloon be if the balloon rises to an altitude where the atmospheric pressure is 0.5 atm.

13. A gas occupies 900.0 mL at -27.0⁰C. What is the volume at 132.0 ⁰C?

14. Use the Ideal Gas Law to determine the pressure exerted by 1 mol of O in a 220 mL container at 30.0 C?

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