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Gases Flashcards

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1
Q

States of matter

A

Gas, Liquid, Solid

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2
Q

Kinetic Molecular Theory

A

Properties of matter are influenced by the energy and motion of the molecules

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3
Q

Kinetic energy of particles

A

Solids least, liquid medium, gas most

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4
Q

Motion of particles

A

Solids limited/ordered, liquid medium, gas random chaos

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5
Q

Empty space/closeness

A

Solids close/no space, liquid close/space, gas ton of space

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6
Q

IMF define

A

Intermolecular forces

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7
Q

IMF 3 states

A

Solids most, liquid medium, gas least

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8
Q

Vol/shape in closed container

A

Solids NA, liquid same shape, diff volume , gas take on vol and shape of container

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9
Q

Vol/shape in open container

A

Solids NA, liquid same shape, diff volume , gas dissipate

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10
Q

Density

A

Solids most, liquid medium, gas least

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11
Q

Compressibility

A

Solids no, liquid sometimes, gas very

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12
Q

Diffusion

A

Solids no, liquid yes, gas yes

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13
Q

Ideal gas

A
  1. Gases have a large number of tiny particles that are

very far apart from one another.

  1. When they collide, they bounce off of each other.
  2. The particles are in continuous, random motion.
  3. There are no forces of attraction or repulsion

between particles.

  1. The kinetic energy of the particles depend on the

temperature of the gas.

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14
Q

Compressibility

A

Ability to be compressed into smaller volume

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15
Q

concentration

A

number of particles within a volume

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16
Q

diffusion

A

higher concentration moves into areas w lower concentration

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17
Q

How does molecular mass relate to diffusion rate?

A

Lighter=faster

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18
Q

Temperature

A

Average kinetic energy of particles

Unit k or c

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19
Q

Higher temp =

A

higher energy

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20
Q

absolute 0

A

temp of which there is no kinetic energy in the particles (0 kelvin)

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21
Q

What does doubling the kelvin temp do to the average kinetic energy

A

doubles it

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22
Q

Endothermic

A

cooling process, releasing heat

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23
Q

exothermic

A

heating process, absorbing heat

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24
Q

sublimation

A

solid immediately heated to gas

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25
depostion
gas immediately cooled to solid
26
examples of endothermic
melting, vaporization
27
examples of exothermic
freezing, condensing
28
Why do solids exist at lower temp
KE is lower
29
Liquid to Gas-IMFs, name
Breaking, vaporization
30
Gas to Liquid-IMFs, name
Forming, condensing
31
Liquid to Solid-IMFs, name
Rigid structure of H bonds are formed, freezing
32
Solid to Liquid-IMFs, name
Rigid structure of H bonds are broken, melting
33
If you have a mixture of ice and water what is the | temperature
0 C
34
What doesn't change during a phase change?
The temperature does not change during a phase change.
35
Each graph of phase changes is for...
Each graph is for a specific substance at a determined pressure
36
A stronger IMF means a higher ___ for solids
melting/freezing point
37
What can change a melting point? What is this called?
Adding certain substances (ex. ionic compounds) to liquids can cause a "freezing point depression," lowering the melting point.
38
Condensation
slow gas molecules that get near the surface of liquid and stick to the liquid
39
Vaporization types
Boiling and Evaporation
40
Evaporation
Vaporization of an uncontained nonboiling liquid. water molecules must be close to surface and have a higher than average k energy. Surface molecules will break away and dissipate into the atmosphere if they have enough KE.
41
Boiling
Vaporization at the boiling point. Making bubbles of gas in the liquid, forcing the liquid level to rise. bubbles have enough force to form and push out of the liquid. Energy goes into breaking forces, not moving faster.
42
Exo or Endo: Evaporation
Endothermic
43
Water cycle
study it
44
Normal Boiling point
the temperature a substance boils at
45
The temperature of a liquid cannot rise above ___
its boiling point
46
Weak IMF =
lower boiling point.
47
Lower BP
Lower the pressure * Easier to make bubbles * Food cooks slower.
48
one atm of pressure
one atmosphere-how much air pressure there is at sea level
49
Raising BP
Raise the external pressure * Harder to make bubbles * Food cooks faster.
50
Pressure
P-how hard the gas is pushing on walls of container | Unit is ATM
51
1 atm
Atmosphere at sea level
52
Volume
Amount of space it takes up | Unit is L
53
1 L =
1 dm3
54
n
Number of moles
55
Boyle's Law
Changing variables P,V Constant n,T the less pressure the more volume; the more pressure the less volume(Inverse relationship) V=k/P P1V1=P2V2
56
Mmhg
Millimeters of mercury
57
kPa
Kilopascal
58
Charles' Law
``` Changing are V,T Constants are P, n Direct relationship Lower temperature, lower volume, Higher temp, higher vol V1/T1 = V2/T2 (Convert to kelvin) ```
59
Kelvin/Celsius
0K=-273C. 1k=-272c To convert C to K add 273 to the C To convert K to C subtract 273 from the C
60
Gay-Lussac's Law
Changing is P,T Constant is V, n P1/T1 = P2/T2 Direct relationship
61
Avogadro's law
V is directly proportional/related to number of moles V=kn V1/n1 = V2/n2 V[]n (see notes for symbol)
62
Standard temp and pressure
STP is 273 kelvin, 1 atm
63
Combined gas law for Boyle, Charles, and G-L
P1V1/T1 = P2V2/T2
64
When to use combined Law of B, C and G-L(throwaway)
All three are changing
65
Dalton's law of partial pressures
When two amounts of gas are combined to same vol and temp, pressure is sum of two previous pressures
66
Ideal gas law
PV=nRT Or P1V1/n1T1 = P2V2/n2T2 = R Can be rewritten to solve for molar mass as
67
R
Ideal gas constant
68
Where are laws found within ideal gas laws
Changing variables
69
R in terms of units
R in terms of units R= (atm * L)/mol * k
70
When does numerical value of R change?
Numerical value of R changes if you change the units
71
1L*atm
101.325J
72
Numerical values of R in terms of L*atm/mol*k? J/mol*k?
.0821, 8.314
73
What can be determined by the density of the gas? How?
``` Molar mass of gas can be determined by density of the gas (by rearranging the equation, not numerical answer) Steps: D=m/V Molar mass. M=m/n or n=m/M PV=nRT ```
74
Ideal gas law Can be rewritten to solve for molar mass as
PV=(m/M)RT
75
Given gas, pressure, volume and temp. Solve for mass of gas.
1. Find molar mass of gas 2. Find n using PV=nRT 3. n=m/Molar mass m=answer
76
m
Mass of sample
77
M
Molar mass
78
Cartesian Diver
Boyle's Law-pressure is low, vol is high, squeezing the bottle adds pressure, causing the volume to sink
79
Potato Gun
Boyle's Law-pressure is low, vol is high, shooting the gun causes pressure to rise, causing the volume to sink
80
Balloon in flask
Charles' Law-heating up flask attached to balloon--increasing temp increases volume (of balloon)
81
Crushed can
G-L-crushing a can

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