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Honors Chemistry > Module 06: Phases of Matter > Flashcards

Module 06: Phases of Matter Flashcards

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1
Q

06.01 Kinetic Molecular Theory

06.01 Kinetic Molecular Theory

A
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2
Q

06.01 Kinetic Molecular Theory

Define Kinetic Theory of Matter

A

describes the physical properties of matter in terms of the motion of its particles

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3
Q

06.01 Kinetic Molecular Theory

What basic assumptions is the Kinetic Theory based on?

A
  1. Matter composed small particles (ions, atoms, molecules)
  2. Particles in matter are organized in different arrangements based on state of matter
  3. Particles of matter constant motion (different amount of kinetic every)
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4
Q

06.01 Kinetic Molecular Theory

Describe the flow of thermal energy in the Kinetic Theory:

A

Absord heat → faster

Release heat → slower

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5
Q

06.01 Kinetic Molecular Theory

Why is temperature measured in “average kinetic energy?”

A

Any time, one particles could have different kinetic energy than neigbor

Always averagee kinetic energy all particles

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6
Q

06.01 Kinetic Molecular Theory

According to kinetic theory, how is motion and arrangement influenced?

A
  1. Kinetic energy
  2. Intermolecular forces

Solid: tightly arranged → more force & less kinetic

Liquid and gasses: loose arrangement → strong kinetic (can break intermolecular forces)

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7
Q

06.01 Kinetic Molecular Theory

Solids: (Arrangement of particles, Motion, Shape, Volume, Compressibility)

A

Arrangement of particles:

  • close together
  • difinite pattern

Motion:

  • vibrate
  • fixed position

Shape: definite

Volume: definite

Compressibility: low

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8
Q

06.01 Kinetic Molecular Theory

Liquid: (Arrangement of particles, Motion, Shape, Volume, Compressibility)

A

Arrangement of particles:

  • close together
  • random pattern

Motion:

  • slide past one another

Shape: not definite

Volume: definite

Compressibility: low

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9
Q

06.01 Kinetic Molecular Theory

Gases: (Arrangement of particles, Motion, Shape, Volume, Compressibility)

A

Arrangement of particles:

  • far apart
  • random pattern

Motion: quick movement any direction

Shape: not definite

Volume: not definite

Compressibility: high

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10
Q

06.01 Kinetic Molecular Theory

Plasma: (Arrangement of particles, Motion, Shape, Volume, Compressibility)

A

Arrangement of particles:

  • far appart
  • pattern influenced attraction of ions

Motion: quick movement any direction

Shape: not definite

Volume: not definite

Compressibility: high

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11
Q

06.01 Kinetic Molecular Theory

What are the 5 basic properties of gases (under normal conditions)?

A
  1. Density
    • low compared to liquid or solid
    • far apart each other
  2. Compressibility
    • can be compressed smaller volumes (due to space between particles)
  3. Expansion
    • spread out fill entire container
  4. Diffusion
    • spread out and mix with other particles without being stirred
  5. Fluidity
    • easily glide part eachother
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12
Q

06.01 Kinetic Molecular Theory

Whta characteristics of a gas is needed to fully describe a sample?

A
  1. Volume (V) [liters]
  2. Pressure (P) [atomspheres (atm)]
  3. Temperature (T) [Kelvin]
  4. Number of particles (n) [moles]
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13
Q

06.01 Kinetic Molecular Theory

What is the pressure of the gas?

A

Collision of moving gas particles

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14
Q

06.01 Kinetic Molecular Theory

What are Pascal, atmospheres, and millimeters of mercury? What is the conversion factor?

A
  • Pascal (Pa): one newton per square meter
  • Atmostpheres (atm)
  • Millimeters of mercury (mm Hg) or torr

1 atmosphere (atm)

= 760 mm Hg

= 760 torr

= 101.3 kilopascals (kPa)

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15
Q

06.01 Kinetic Molecular Theory

What is an ideal gas?

A
  • behaves according all assumptions of kinetic molecualr theory
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16
Q

06.01 Kinetic Molecular Theory

What is the Kinetic Molecular Theory of Gases (5)?

A
  1. Particles gas are in constant motion
  2. Large number of tiny particles
  3. Collisions between partciles are elastic (no gain of loss of kinetic energy due to collision)
  4. No forces of attraction or repulsion are experienced between particles (moves fast enough so attractive forces are negligible)
  5. Average kinetic energy of particles of a gas is directly proportional to temperature (higher the temperature, greater kinetic energy)
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17
Q

06.02 Phase Changes

06.02 Phase Chagnes

A
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18
Q

06.02 Phase Changes

What are the 4 transition points from one state of matter to another?

A
  1. Melting (solid → liquid)
  2. Freezing (liquid → solid)
  3. Boiling (liquid → gas)
  4. Condensation (gas → liquid)
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19
Q

06.02 Phase Changes

What is dew?

A

Water vapor in air condenses to liquid

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20
Q
A
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21
Q

06.02 Phase Changes

How does water change its phase?

A
  • 0 C to 100C: liquid state & temperature and kinetic energy of molecules increase
  • large amount energy needed overcome intermolecular forces between water molecules
    • then break appart one another and move at high speeds and water becomes gas

Melting & boiling = temperature momentarily contant

  • break bonds

energy must be greater than potential energy of bonds between molecules

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22
Q

06.02 Phase Changes

What are heating curves and cooling curves? What is the purpose?

A
  • Heating Curve: line graph represents phase changes matter starting with solid and heating to a gas
    • contant heating
    • gain energy
  • Cooling Curve: graph of phase changes of matter starting with gas and cooling to solid
    • contant cooling
    • loose energy

Model temperature changes and phase transitions

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23
Q

06.03 Gas Laws

06.03 GAS LAWS

A
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24
Q

06.03 Gas Laws

Define Scientific Laws:

A

Generalization that describes a variety of behaviors in nature but does not attempt to explain them (why not how).

  • based on observations and experimentation
  • tested agian and peer reviewed
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25
Q

06.03 Gas Laws

What is Newton’s Law of Universal Gravitation?

A
  • force of attraction between any two option
  • attraction in mathematcis terms (not why it exists)
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26
Q

06.03 Gas Laws

What is Kepler’s Laws of Planetary Motion?

A
  • 3 mathematics laws describe motion planets in solar system
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27
Q

06.03 Gas Laws

What is Gas Law?

A

There are laws that predict the behavior of gases. These gas laws describe the relationship between volume, temperature, pressure, and mole amount, and how all gases will act under certain conditions.

28
Q

06.03 Gas Laws

What 4 factors causes changes in gases?

A
  1. Volume (V)
  2. Pressure (P)
  3. Temperature (T)
  4. Number of particles (n)
29
Q

06.03 Gas Laws

What are the 7 Gas Laws?

A
  1. Changes to V, n, and T will affect pressure, kinetic energy, and the number of collisions within a sample.
  2. If the volume of a sample is large, the pressure will be low, and there will be few particle collisions.
  3. If the volume of a sample is small, the pressure will be higher, and more collisions will occur.
  4. If the number of particles decreases, the number of collisions will decrease.
  5. If the number of particles increases, the number of collisions will increase.
  6. If temperature increases, the number of collisions will increase.
  7. If temperature decreases, the number of collisions will decrease.
30
Q

06.03 Gas Laws

What are the variables and their meating in the Gas Laws?

A

Initial Quantities:

P1 = initial pressure

V1 = initial volume

T1 = initial temperature

n1 = initial number of moles

Final Quantities:

P2 = final pressure

V2 = final volume

T2 = final temperature

n2 = final number of moles

31
Q

06.03 Gas Laws

What is Boyle’s Law?

A

Pressure and Volume

  • Relationship: P1V1 = P2V2
  • Gas Behavior: Inverse relationship between pressure of gas and volume
    • ↑P↓V and ↓P↑V
  • Contants: Temperature and numbers of moles are held constant
32
Q

06.03 Gas Laws

What is Charles’s Law?

A

Volume and Temperature

  • Relationship: V1÷T1=V2÷T2
  • Gas Behavior: Direct relationship between volume of gas and temperature
    • ↑V↑T and ↓V↓T
  • Constants: pressure and number moles constant
33
Q

06.03 Gas Laws

What is Gay-Lussac’s Law?

A

Pressure and Temperature

  • Relationship: P1÷T1=P2÷T2
  • Gas Behavior: Direct relationship between presssure of a gas and temperature
    • ↑P↑T and ↓P↓T
  • Constants: Volume and number of moles of gas are held constant
34
Q

06.03 Gas Laws

What is Avogadro’s Law?

A

Volume and Moles

  • Relationship: V1÷n1=V2÷n2
  • Gas Behavior: direct relationshiip between volume of gas and number of moles of a gas
    • ↑V↑n and ↓V↓n
  • Constant: Pressure and temperature are constant
35
Q

06.03 Gas Laws

A scientific law is the explanation of multiple scientific theories. (1 point)

True

False

A

False

36
Q

06.03 Gas Laws

Which of the following would not cause an increase in the pressure inside a sealed container of neon gas? (4 points)

  1. Increasing temperature
  2. Adding more neon gas
  3. Increasing the volume of the container
  4. Adding helium gas
A

3. Increasing the volume of the container

37
Q

06.03 Gas Laws

At 0.750 atm, the volume of a gas is 300.0 mL. If the temperature remains constant and the pressure is changed to 0.600 atm, what is the new volume of the gas? (4 points)

  1. 0.00150 mL
  2. 0.00200 mL
  3. 155 mL
  4. 375 mL
A

4. 375 mL

38
Q

06.03 Gas Laws

A 6.0 L sample of nitrogen gas contains 0.50 mole of a gas. If enough gas is added to make a total of 0.75 moles at the same pressure and temperature, what is the resulting total volume of the gas? (4 points)

  1. 2.3 L
  2. 4.8 L
  3. 7.5 L
  4. 9.0 L
A

4. 9.0 L

39
Q

A gas at constant volume has a pressure of 3.20 atm at 300. K. What will be the pressure of the gas at 290. K? (4 points)

  1. 2.86 atm
  2. 3.09 atm
  3. 3.31 atm
  4. 3.56 atm
A

2. 3.09 atm

40
Q

06.04 Ideal Gas Law

06.04 Ideal Gas Law

A
41
Q

06.04 Ideal Gas Law

Define Ideal Gas Law:

A

the state of an ideal gas follows the equation PV = nRT

42
Q

06.04 Ideal Gas Law

What is the equation in the Ideal Gas Law?

A

PV = nRT

  • P = pressure (atm)
  • V = volume (V)
  • n = number of moles (mol)
  • R = ideal gas constant = 0.0821 (L x atm)÷(mol x K)
  • T = temperature (K)
43
Q

06.04 Ideal Gas Law

How can ideal gas relationships predict the volume of gases in a chemical reaction?

A
  • Volume ratio same steps as mole ratios
    *
44
Q

06.04 Ideal Gas Law

What is the Volume ratio?

A

the ratio of volume of one gaseous reactant or product to the volume of another determined using the coefficients in a balanced equation

45
Q

06.04 Ideal Gas Law

Assuming all volume measurements are made at the same temperature and pressure, how many milliliters of carbon dioxide gas can be produced when 206.5 milliliters of oxygen gas react with excess carbon monoxide?

2CO(g) + O2(g) → 2CO2(g)

A

The coefficients in this balanced equation provide a volume ratio between gases when they are all at the same temperature and pressure. A ratio of 1:2 of O2 to CO2 means that a given volume of oxygen gas will react with twice the volume of carbon dioxide.

206.5 mL O2 × [2 mL CO2]÷[1 mL O2] = 413.0 mL CO2 can be produced

The ideal gas law uses the liter as the unit of volume for gas; however, this works for any unit of volume if the units are the same as the units in the volume ratio and both substances are gases under the same conditions.

46
Q

06.04 Ideal Gas Law

What are the standard conditions for gases?

A

STP: an abbreviation that represents standard temperature and pressure

  1. Standard Temperature: 273 K
  2. Standard Pressure: 1 atm
47
Q

06.04 Ideal Gas Law

What is the volume to mole conversion factors?

A

1 mole of gas / 22.4 L or 22.4 L / 1 mole of gas

48
Q

06.04 Ideal Gas Law

To use the gas law constant R = 0.0821, the unit for temperature should be Kelvin and the unit for volume should be milliliters. (2 points)

True

False

A

False

49
Q

06.04 Ideal Gas Law

What is the volume of 2.1 moles of nitrogen gas at standard temperature and pressure (STP)? (3 points)

  1. 11 L
  2. 22 L
  3. 47 L
  4. 82 L
A

3. 47 L

50
Q

06.04 Ideal Gas Law

A reaction is expected to produce 28.3 moles of hydrogen gas. If the hydrogen is collected at 297 K and 1.08 atm, what is the volume? (3 points)

  1. 305 L H2
  2. 639 L H2
  3. 948 L H2
  4. 1,240 L H2
A

2. 639 L H2

51
Q

06.04 Ideal Gas Law

Zinc metal and hydrochloric acid react together according to the following equation:

2HCl(aq) + Zn(s) → ZnCl2(aq) + H2(g)

If 5.98 g Zn reacts with excess HCl at 298 K and 0.978 atm, what volume of H2 can be collected? (3 points)

  1. 2.29 L H2
  2. 3.32 L H2
  3. 4.58 L H2
  4. 7.41 L H2
A

1. 2.29 L H2

52
Q

06.04 Ideal Gas Law

Read the given equation.

Na2O2 + CO2 → Na2CO3 + O2

What volume of O2 gas is produced from 2.80 liters of CO2 at STP? (3 points)

  1. 5.60 liters
  2. 4.20 liters
  3. 2.10 liters
  4. 1.40 liters
A

4. 1.40 liters

53
Q

06.04 Ideal Gas Law

Read the given equation.

2Na + 2H2O → 2NaOH + H2

During a laboratory experiment, a certain quantity of sodium metal reacted with water to produce sodium hydroxide and hydrogen gas. What was the initial quantity of sodium metal used if 8.40 liters of H2 gas were produced at STP? (3 points)

  1. 17.2 grams
  2. 15.8 grams
  3. 12.3 grams
  4. 10.0 grams
A

1. 17.2 grams

54
Q

06.04 Ideal Gas Law

Which of the following factors does not determine the movement of particles in the atoms or molecules of a gas according to the ideal gas law? (3 points)

  1. Pressure
  2. Temperature
  3. Volume
  4. Type of particles
A
  1. Type of particles
55
Q

06.06 Honors Gas Behavior

06.06 Honors Gas Behavior

A
56
Q

06.06 Honors Gas Behavior

Define Effusion:

A
  • movement of gas particles through a small opening in container wall due to pressure and particle movement inside the container
57
Q

06.06 Honors Gas Behavior

When does Diffusion and Effusion increase and decrease?

A

both dependent on velocity of gas particles (influenced by temperature and molar mass of gas)

Diffusion/Effusion increase:

  1. temperature increases
  2. gas lower molar mass
  3. particles are moving quickly

Diffusion/Effusion decreases:

  1. temperature decreases
  2. gas has higher molar mass
  3. particles moving slowly
58
Q

06.06 Honors Gas Behavior

: We can also make comparisons of velocity, rate of effusion, or rate of diffusion based on molar mass. Gas particles with less mass have higher velocities (and rates of effusion and diffusion) than gas particles with greater mass. Which sample of gas would effuse the fastest under the same temperature and pressure conditions?

CH4

Cl2

O2

Ne

A

CH4 would effuse the fastest because it has the lowest molar mass of the gases above.

59
Q

06.06 Honors Gas Behavior

What information can be used to compare the molar masses and velocity of different gases?

A

Less massive gas particles move faster with an increase in temperature

60
Q

06.06 Honors Gas Behavior

What is Graham’s Law?

A

law stating that the rates of diffusion and effusion of a gas are inversely proportional to the square root of the density of the gas

61
Q

06.06 Honors Gas Behavior

What is the steps to solve a problem with Graham’s Law?

A

Step 01: Setup equation with given rate comparison

Step 02: Substitute known molar masses

Step 03: Solve the molar mass for the unknown variable

62
Q

06.06 Honors Gas Behavior

How can the mole ratio and ideal gas law be used to determine a substance molarity?

A
  1. Ideal gas law PV = nRT (n = moles)
  2. Stoichiometry: moles of sample (n) = mass sample (m)/ molar mass substance (M)

M = mRT/PV

63
Q

06.06 Honors Gas Behavior

What is the formula for molar mass (derived from ideal gas laws)?

A

M = mRT/PV

Step 01: Identify variables
Step 02: Solve

64
Q

06.06 Honors Gas Behavior

How can density be derived from the ideal gas laws?

A
  1. Ideals gas laws: n = PV/RT
  2. Replace moles (n) with mass (m)) over molar mass (M) → m/M = PV/RT
  3. Use algebra allows us swap positions of M and V to give m/V = PM/RT
  4. Density of gas is mass perunit volume → d = m/v

d = PM/RT

65
Q
A
66
Q

06.06 Honors Gas Behavior

How do real gasses deviate from the ideal gas concept?

A
  • finite volume
  • interact through intermolecular forces
67
Q

06.06 Honors Gas Behavior

Name two extreme conditions that results in a deviation from ideal conditions?

A
  1. Very high pressure (additional volume becomes significant under high pressure)
  2. Very low temperatures (intermolecular forces is significant - less kinetic energy to overcome intermolecular forces)

Honors Chemistry (8 decks)

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