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Advanced Chemistry > Unit 1 - Matter and Energy - Gas Laws > Flashcards

Unit 1 - Matter and Energy - Gas Laws Flashcards

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1
Q

What is the Kinetic Molecular Theory? (3)

A
  1. Describes the behaviour of gases
  2. In terms of motion
  3. And relationships between gas particles
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2
Q

What does the Kinetic Molecular Theory explain?

A

Describes relationship of:

  1. Pressure
  2. Volume
  3. Temperature
  4. Velocity
  5. Frequency
  6. Force

between collisions of gas molecules

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3
Q

According to the Kinetic Molecular Theory, what is the volume of gases? (3)

A
  1. Gas particles have a negligible volume
  2. Most of the volume is empty space
  3. Gas can be compressed very easily because you are just removing a part of the empty space!
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4
Q

According to the Kinetic Molecular Theory, what is the relationship between gas particles? (4)

A
  1. Have neither attractive/repelling forces
  2. They don’t stick to each other OR push each other away
  3. Allows them to space out & fill up the whole volume
  4. If there were significant attractive forces, the gas particles would clump together, and the gas wouldn’t behave as freely compared to liquids and solids
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5
Q

According to the Kinetic Molecular Theory, how do you describe the collisions? (3)

A
  1. Collisions are Elastic
  2. No kinetic energy in the closed system is lost
  3. This helps predict gas behaviour
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6
Q

According to the Kinetic Molecular Theory, how do you describe transfer of energy? (4)

A
  1. When two gas particles collide, one slows down while they other speeds up!
  2. This means that kinetic energy was transferred between the particles
  3. However, in a closed system, although energy is getting transferred, the total kinetic energy in that system will always stay the same
  4. This explains why gases maintain a consistent temperature and pressure under stable conditions
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7
Q

Definition of Vacuum (4)

A
  1. Empty space
  2. No particles
  3. No collisions
  4. No Pressure
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8
Q

Definition of the Ideal Gas Model (4)

A
  1. Model that explains the behaviour of gases based on the KMT
  2. Low Pressure and High Pressure help represent the Ideal Gas Model
  3. L Pressure: Indicates less collisions
  4. H Temp: High KE can overcome attractive forces

HELPFUL: WHERE WOULD A GAS LIKE TO SPEND ITS VACAY? (BEACH HAS HIGHER TEMPERATURE AND LOWER PRESSURE)

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9
Q

What are two things you can do when molecules collide?

A
  1. Bounce apart
  2. React to form something new
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10
Q

Definition of Collision Therory

A
  1. In collisions, wiith proper energy and orientation
  2. Chemical reactions will occur
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11
Q

Definition of Pressure

A

A force exerted on a specific area

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12
Q

What is the kinetic - molecular view of gas pressure?

A

More Collisions = More Pressure

The greater amount of collisions means that there is a greater force. Therefore, since pressure is force/area, pressure increases

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13
Q

Standard Unit of Pressure

A

Pascal (Pa)

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14
Q

Atmospheric Pressure at sea level in KiloPascal

A

101.3 kiloPascal

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15
Q

Atmospheric Pressure at sea level in Atmospheres

A

1 Atmosphere

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16
Q

Atmospheric Pressure at sea level in millimeters of mercury

A

760 mm Hg

17
Q

Atmospheric Pressure at sea level in Torr

A

760 Torr

18
Q

What is the relationship between temperature and velocity?

A

The greater the average kinetic energy of the molecules, the greater the speed of those molecules

19
Q

What is the relationship between mass (weight of particles) and the velocity?

A

The greater the mass, the lower the velocity

Analogy: Heavier molecules move more slowly because they need more energy to reach the same speed as lighter molecules.

20
Q

Avogrado’s Hypothesis (4)

A
  1. Equal volumes of gases
  2. Same temperature
  3. Same Pressure
  4. Equal number of particles

Mnuemonic: S.T.E.V.E.N

Same Temperature, Equal Volume, Equal Number

21
Q

Definition of Boyle’s Law (5)

A
  1. As long a temp. stays the same
  2. As Volume Decreases
  3. Pressure Increases
  4. When one goes up the other goes down
  5. Smaller volume means more collisions AND MOLECULES ARE EXERTING MORE FORCE AGAINST WALLS

Analogy: If you squeeze a balloon (decrease vol.), the air inside pushes harder against the balloon (increase pressure)

Let the balloon expand (increase the volume) and the pressure inside the balloon decreases.

22
Q

Definition of Charles’ Law (4)

A
  1. If pressure stays the same
  2. When Temperature Increases
  3. Volume Increases
  4. Vice Versa - when one goes up, other goes down

Analogy:
Balloon is heated - expands
Balloon is cooled - contracts

23
Q

How does pressure influence Charles’ law?

A

The container must get bigger when heated in order for the pressure to stay the same.

24
Q

Why does an increase in temperature mean an increase in pressure (4)?

A
  1. Higher Temp = Higher KE
  2. Higher KE = Faster particles
  3. Faster particles = more collisions with container walls
  4. More collisions = Higher pressure
25
Q

WHY will pressure stay the same when the volume increases in Charles’ law? (4)

A
  1. When the volume increases
  2. More room for faster moving particles
  3. Limits # of collisions
  4. Keeps pressure the same
26
Q

When should you check the pressure - before or after?

A

After

27
Q

What is the formula for Charles’ law?

A

Initial Volume/Initial Temperature =
Final Volume / Final Temperature

28
Q

Definition of the Combined Gas Law (3)

A
  1. press. X vol /temp. of a system remains constant (RATIO)
  2. Combines Boyle’s Law and Charles’s Law
  3. If you change one factor, the others adjust PROPORTIONALLY to maintain equilibrium
29
Q

What occurs if there is a fixed volume for gases? (4)

A
  1. Typically, if walls are flexible and gases are heated, it’ll expand and push those walls back
  2. However, if walls are rigid and gases are heated, the gas cannot expand
  3. So, the pressure will keep building up in that container
  4. If the pressure gets too high, the container will explode
30
Q

Definition of Standard Pressure & Temperature (STP) (2)

A
  1. Standard conditions for temp. and pressure
  2. Used as a comparison
31
Q

Formula for Boyle’s Law

A

P1V1 = P2V2

32
Q

Formula for Charles’ Law

A

V1 / T1 = V2 / T2

Advanced Chemistry (15 decks)

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