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10th Grade Chemistry > Chapter 12-Kinetic Theory-Finals > Flashcards

Chapter 12-Kinetic Theory-Finals Flashcards

(90 cards)

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1
Q

Kinetic energy definition

A

The energy an object has because of its motion

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2
Q

What characteristics do particles in a gas, whether atoms or molecules, have in relation to motion?

A

The particles in a gas are in rapid, constant and random motion.

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3
Q

What does the fact that the particles in a gas are in rapid, constant, and rando motion cause?

A

This causes them to collide with each other as well as with the walls of their containers.

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4
Q

Describe what the particles in a gas themselves are like.

A

The particles in a gas are considered to be small, hard spheres with an insignificant volume.

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5
Q

What are collisions between particles in a gas like?

A

All collisions between particles in a gas are perfectly elastic.

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6
Q

When collisions between particles in a gas happen, what remains constant?

A

The total kinetic energy of the system remains constant.

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7
Q

What is gas pressure the result of?

A

Simultaneous collisions of billions of rapidly moving particles in a gas with an object.

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8
Q

Vacuum definition

A

An empty space. There are no particles so there is no pressure.

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9
Q

How does atmospheric pressure happen?

A

It results from the collisions of atoms and molecules in the air with objects.

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10
Q

Barometer definition

A

A device used to measure atmospheric pressure

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11
Q

At the top of a mountain, are there less or more air particles than there are at sea level?

A

At the top of a mountain, there are less air particles than there are at sea level

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12
Q

Is atmospheric pressure on the top of a mountain higher or lower than at sea level?

A

Here, Patm is less than that at sea level

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13
Q

At the bottom of Death Valley, are there less or more particles than at sea level?

A

At the bottom of Death Valley, there are more air particles than there are at sea level.

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14
Q

At the bottom of Death Valley, is atmospheric pressure higher or lower than at sea level?

A

Here, Patm is greater than that at sea level.

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15
Q

Temperature definition

A

A measure of the average kinetic energy of particles in a collection of matter

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16
Q

Why is temperature the AVERAGE kinetic energy of particles?

A

It is average because in a collection of matter, some particles are moving slowly, some moderately, and some rapidly, so the average of the motion of these particles gives us the temperature.

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17
Q

Do particles of all substances have the same average KE?

A

At any given temperature the particles of all substances, regardless of their physical state, have the same average KE.

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18
Q

What happens to the temperature of a substance if particles in the substance are moving fast?

A

The faster the particles of a substance are moving, the greater the average KE they have and hence the higher the temperature will be.

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19
Q

What happens to the temperature of a substance if particles in the substance are moving slowly?

A

The slower the particles of a substance are moving, the lesser the average KE they have and hence the lower the temperature will be.

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20
Q

What effect do intermolecular forces of attraction have on the volume of a liquid?

A

Intermolecular forces of attraction between the particles in a liquid keep the particles close enough together to give the liquid a definite volume (contrast this with a gas)

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21
Q

Are liquids denser than gasses? Why or why not?

A

Since the particles in a liquid are closer together than those in a gas, liquids are denser than gases

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22
Q

Does increasing the pressure on a liquid effect its volume?

A

Increasing the pressure on a liquid had basically no effect on its volume

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23
Q

What implications does the fact that the particles of a liquid possess kinetic energy have?

A

The particles of a liquid, like those of a gas, possess kinetic energy and, as such, they are able to flow past one another.

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24
Q

Fluids definition

A

Substances that flow.

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25
What does the ability to flow allow gasses and liquids to do?
The ability to flow allows gases and liquids to take the shape of their containers
26
Evaporation definition
the conversion of a liquid to a gas or vapor below its boiling point
27
Is evaporation a surface phenomenon?
yes
28
How does evaporation in an open container happen?
Particles near the surface can acquire sufficient KE can escape the confines of the liquid phase and enter the gaseous or vapor phase
29
When does evaporation in an open container end?
This process continues until all of the liquid disappears
30
Does evaporation in an open container require the addition of heat?
It doesn't require the addition of any heat
31
What happens during evaporation in a closed container that doesn't happen during evaporation in an open container?
Particles near the surface that acquire sufficient KE leave the liquid phase and enter the gaseous or vapor phase. Here, however the particles that have entered the gaseous or vapor phase are trapped
32
What happens as more and more particles begin to leave the liquid phase and fill the space above the liquid? (2 things)
They exert a pressure on the surface of the liquid called vapor pressure and the number of collisions between the particles here increases.
33
What will happen to some particles that entered the gaseous or vapor phase during condensation in a closed container
Some particles that entered the gaseous or vapor phase will lose a sufficient amount of KE and return to the liquid phase.
34
Equilibrium vapor pressure definition
At some point, in a closed container, the # of particles leaving the liquid will equal the # of particles re-entering the liquid.
35
What happens when a system (closed container) is at equilibrium vapor pressure?
There is no NET change in the rates of evaporation and condensation.
36
What can affect equilibrium vapor pressure?
The addition or removal of heat and the size of the container.
37
How does adding heat affect equilibrium vapor pressure in a closed container?
If heat is added, the average KE of the particles of the liquid increases and more particles acquire sufficient KE to leave the surface and enter the gaseous or vapor phase, so equilibrium vapor pressure increases.
38
How does removing heat/cooling affect equilibrium vapor pressure in a closed container?
If heat is removed, the average KE of the particles of the liquid decreases and fewer particles can acquire sufficient KE to leave the surface and enter the gaseous or vapor phase, so equilibrum vapor decreases.
39
How does the size of the container getting bigger affect equilibrum vapor pressure? Why?
If the amount of liquid remains constant but the volume of the container increases, the equilibrium vapor pressure will decrease. This is because there would be more space above the surface of the liquid
40
How does the size of the container getting smaller affect equilibrum vapor pressure? Why?
If the amount of liquid remains constant but the volume of the container decreases, the equilibrium vapor pressure will increase. This is because there would be less space above the surface of the liquid
41
Why is evaporation a cooling process?
When the particles with the greatest KE leave the surface of the liquid, those left behind have a lower average KE. Since they have a lower average KE, they aren't moving as quickly so the temperature is lower. (temp and KE are related)
42
Vaporization definition
conversion of a liquid to a gas or a vapor
43
Vapor pressure definition
the tendency of molecules to leave at the surface
44
Can boiling take place at any temperature or pressure?
No, it takes place at specific temperatures and pressures
45
Describe the process of boiling.
Patm opposes the formation of bubbles in a liquid. Bubbles form only when the temperature is such that particles throughout the liquid have enough KE to vaporize. Boiling occurs when vapor pressure is equal to Patm.
46
Boiling point definition
The temperature at which the vapor pressure of the liquid is just equal to the external pressure (P atm) on the liquid
47
Do liquids always boil at the same temperature?
Liquids don't always boil at the same temperature
48
Does altitude affect the bp of a liquid?
Yes
49
Explain boiling at higher altitudes.
Patm is lower at higher altitudes, so there is less pressure on the surface of water in a pot. Since there is less resistance to the formation of bubbles the water will boil more quickly and at a lower temperature. Food would take longer to cook.
50
Do liquids all have the same boiling point?
No, a liquid can have various boiling points depending on pressure
51
What pressure is the normal boiling point at?
The normal boiling point is defined as the bp of a liquid at a pressure of 101.3 kPa
52
Is boiling a cooling process? Explain?
No because boiling is adding heat. Evaporation is a cooling process.
53
Can the temperature of a boiling liquid ever rise above its bp? Explain?
No, because added heat goes into converting the liquid to vapor, not increasing the temperature.
54
Explain why a burn from steam is more severe than a burn from an equal mass of boiling water at the same temperature
Steam contains more energy per gram than boiling water
55
Do solids flow? Why?
The particles in a solid tend to vibrate about fixed points, unlike those of gases and liquids, and as such do not flow
56
Are solids compressible? Why?
The particles are packed tightly together, unlike those gases and liquids, making solids dense and basically incompressible
57
Melting point definition
The temperature at which the solid is converted into a liquid
58
Describe the process of melting
When a solid is heated the particles vibrate more quickly and their KE increases. At some point, the particles will move rapidly enough, and they will overcome the attractive forces keeping them in fixed positions. i.e. they will flow
59
Freezing point definition
The temperature at which a liquid is converted into a solid
60
Describe the process of freezing
When heat is removed, the KE of the liquid particles decreases, and they tend to come closer together. Their attractive forces then keep them in fixed positions, so they don't flow.
61
Keep in mind that
The melting point and freezing point of a substance are the same
62
How are the particles of a crystalline solid arranged?
The particles are arranged in an orderly, repeating, 3-D pattern called a crystal lattice.
63
What determines the shape of a chrystal?
The crystal lattice pattern of the particles.
64
Unit cell definition
The smallest representative part of a crystal lattice.
65
What does the type of bonding between solids determine?
The type of bonding between particles determines the mp of the solid.
66
What determines the melting point of a solid?
The type of bonding between particles determines the mp of the solid
67
What type of solids tend to have a higher melting point? Why?
Ionic solids tend to have high mp because of the ionic bonds present
68
What type of solids tend to have a lower melting point? Why?
Molecular solids tend to have low mp because of the covalent bonds present.
69
Do all solids melt?
Not all solids melt, some decompose upon heating
70
Allotropes definition
Two or more different molecular forms of the same element in the same physical state.
71
Do all allotropes of the same element have the same properties?
Although allotropes are composed of atoms of the same element, they have different properties because their structures are different.
72
Best example of an allotrope
carbon
73
Amorphous solids definition
Solids that lack an ordered internal structure because atoms are randomly arranged.
74
What is an example of an amorphous solid?
Glass
75
Is glass realllyyyy a solid?
It is actually a supercooled liquid.
76
What is the sign for molar heat of fusion?
(ΔHfus)
77
Molar heat of fusion definition
the heat absorbed by one mol of a solid substance as it melts to a liquid at a constant temperature
78
Molar heat of solidification sign
(ΔHsolid)
79
Molar heat of solidification definition
the heat lost when one mole of a liquid solidifies at a constant temperature
80
Molar heat of vaporization sign
(ΔHvap)
81
Molar heat of vaporization definition
the amount of heat needed to vaporize one mol of a given liquid
82
Molar heat of condensation sign
(ΔHcond)
83
Molar heat of condensation definition
the amount of heat released when one mole of vapor condenses at the normal bp
84
What are sloped regions of a heating or cooling curves
The addition of heat makes the particles move more quickly so the temperature rises. The converse is also true.
85
What are plateau regions of a heating or cooling curves
Phase changes. The addition of heat serves to break the bonds between the particles so a change of state can occur. However, only when the change of state is completed will the addition of heat cause a rise in temperature. The converse is also true.
86
Sublimination definition
The change of a substance from a solid to a vapor without passing through the liquid state
87
What is sublimination due to
It is due to the vapor pressure of the solid
88
What needs to be true about the vapor pressure of a solid to cause a substance to sublime?
If the vapor pressure of a solid is greater than Patm at or near room temperature, then the substance will sublime
89
Name 3 substances that sublime
moth balls, dry ice, solid air fresheners
90
What is the use of a manometer?
A manometer measures the pressure of gases or liquids.

10th Grade Chemistry (10 decks)

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