Gases, Liquids, and Solids Flashcards

1
Q

Pressure

A

Force/unit of area

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2
Q

Gas properties

A
  • Take the shape of the container
  • No definite shape
  • No definite volume
  • Least dense phase of a substance
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3
Q

Standard pressure

A

1 atmosphere, 101.3 kPa, 760 torr, 760 mm Hg

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4
Q

Boyle’s Gas Law (movable piston)

A

P1V1 = P2V2

  • Indirect relationship
  • As pressure increases, volume decreases
  • As pressure decreases, volume increases
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5
Q

Charles’ Gas Law

A

V1/T1 = V2/T2

  • Direct relationship
  • As temperature increases, volume increases
  • As temperature decreases, volume decreases
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6
Q

What is important to remember about Charles’ law?

A

Temperature must be in Kelvin

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7
Q

Combined gas law

A

P1V1/T1 = P2V2/T2

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8
Q

Diffusion

A

The movement of gas particles from a region of high concentration to low concentration

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9
Q

Graham’s law of diffusion

A

v1/v2 = square root of m2/m1

v = velocity
m = mass

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10
Q

Which gas diffuses the fastest? Slowest? Why?

a) CO2 b) He c) N2 d) SO2

A

He diffuses the fastest because it has the smallest mass

SO2 diffuses the slowest because it has the largest mass

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11
Q

Dalton’s law of partial pressure

A

The total pressure in a room is equal to the sum of the partial pressures of the gases

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12
Q

Partial pressure setup for air

A

P total pressure of air = P N2 + P O2 + P Ar

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13
Q

How do you calculate partial pressure?

A

Moles of one individual gas x total pressure/sum of total moles

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14
Q

Characteristics of an ideal gas

A
  • Gas particles are in constant, random, straight line motion
  • Gases collide with each other and the walls of the container
  • Gas particles are separate by great distances and have a negligible volume
  • Gas particles do not attract each other
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15
Q

Which 2 gases behave most like an ideal gas?

A

Hydrogen and helium because they are the smallest elements with the smallest densities and radii. Helium is also inert.

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16
Q

Under which conditions does a gas become an ideal gas?

A

High temperatures and low pressure

17
Q

Liquid properties

A
  • More dense than gas phase, but less dense than solid phase
  • Takes shape of container
  • Definite volume
18
Q

Vapor pressure

A

In a closed system, the vapor formed from the evaporation of a liquid or the sublimation of a solid that exerts a pressure on the walls of the container

19
Q

What happens to vapor pressure as temperature increase?

A

As temperature increases, vapor pressure increase

20
Q

If particles have a high vapor pressure and escape easily to the gas phase, they have…

A

Weak bonds or intermolecular forces

21
Q

Intermolecular forces

A

Forces between molecules

22
Q

If particles have a low vapor pressure, they have…

A

Strong intermolecular forces

23
Q

Boiling point

A

The temperature at which the vapor pressure of the liquid or solid is equals to the external air pressure around it

24
Q

Normal boiling point

A

The temperature at which vapor pressure equals standard pressure

25
Solid properties
- Definite shape and definite volume - Most condense phase
26
What is the only exception to the density rules of solids, liquids, and gases?
Water in the solid ice phase is less dense than water in the liquid water phase (ice floats)
27
Crystal/crystalline solids
A regular, repeating, geometric pattern
28
Examples of crystals
NaCl, dry ice or CO2(s), Cdiamond, Cu)
29
Amorphous solids
Lacks structure and doesn’t have a regular, repeating, geometric pattern
30
Examples of amorphous solids
Glass, plastic, silicon, clay
31
Do solids have kinetic energy?
Yes, solids have kinetic energy even though their relative position doesn’t change