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Thermal Properties Flashcards

Understand thermal properties (52 cards)

1
Q

What is the kinetic model?

A

Gases, liquids, and solids are made up of atoms, molecules, and/or ions, with differing behaviors across the three phases.

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2
Q

Describe the arrangement of particles in gases.

A

Particles are well separated with no regular arrangement.

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3
Q

Describe the arrangement of particles in liquids.

A

Particles are close together with no regular arrangement.

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4
Q

Describe the arrangement of particles in solids.

A

Particles are tightly packed, usually in a regular pattern.

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5
Q

How do particles in gases move?

A

They vibrate and move freely at high speeds.

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6
Q

How do particles in liquids move?

A

They vibrate, move about, and slide past each other.

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7
Q

How do particles in solids move?

A

They vibrate but generally do not move from place to place.

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8
Q

What are the two types of energy present in particles?

A

Kinetic energy and potential energy.

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9
Q

What determines the temperature of a body?

A

Kinetic energy.

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10
Q

What determines the state of a body?

A

Potential energy.

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11
Q

List the four states of matter.

A
  • Solid
  • Liquid
  • Gas
  • Plasma
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12
Q

What happens to energy during a change of state?

A

Energy is either taken in or given out.

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13
Q

What is latent heat?

A

Energy absorbed during a change of state that does not produce a change in temperature.

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14
Q

What is the latent heat of vaporization compared to the latent heat of fusion?

A

Latent heat of vaporization is higher than the latent heat of fusion for the same substance.

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15
Q

How does evaporation differ from boiling?

A

Evaporation occurs over a wide range of temperatures, while boiling occurs at a single temperature.

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16
Q

What factors affect evaporation?

A
  • Surface area
  • Wind
  • Pressure
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17
Q

Define boiling point.

A

The temperature at which saturated vapor pressure equals external atmospheric pressure.

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18
Q

What is specific heat capacity?

A

The heat energy required to increase the temperature of 1 kg of a substance by 1 °C or 1 K.

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19
Q

What is the unit of specific heat capacity?

A

J kg-1 K-1 or J kg-1 °C-1.

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20
Q

What is heat capacity?

A

The heat energy required to increase an object’s temperature by 1 °C or 1 K.

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21
Q

What is the unit of heat capacity?

A

J K-1 or J °C-1.

22
Q

What is the principle behind measuring specific heat capacity?

A

Supply a known amount of energy to a known mass of material and measure the rise in temperature.

23
Q

What is the specific latent heat of fusion?

A

The energy required to change the state of 1 kg of material from solid to liquid without a change of temperature.

24
Q

What is the specific latent heat of vaporization?

A

The energy required to change the state of 1 kg of material from liquid to vapor without a change of temperature.

25
What is the specific latent heat of vaporization of water?
Approximately 2.3 x 10^6 J kg-1.
26
What is the specific latent heat of fusion of ice?
Approximately 3.3 x 10^5 J kg-1.
27
What is the First Law of Thermodynamics?
The internal energy of a system depends only on its state; the increase in internal energy equals the sum of the energy supplied by heating and the work done on the system.
28
What does the internal energy of a gas depend on?
The state of the system and the sum of the random distribution of kinetic and potential energies associated with its molecules.
29
How can the internal energy of a gas be increased?
* Heating the body * Doing work on the body
30
Write the equation for the First Law of Thermodynamics.
ΔU = ΔQ + ΔW.
31
What happens to temperature when work is done on a gas?
The gas becomes hotter.
32
If 100 J of energy is added to a system that does no external work, what is the increase in internal energy?
ΔU = 100 J.
33
If 100 J of energy is added to a system that does 40 J of external work, what is the increase in internal energy?
ΔU = 60 J.
34
What is the work done against the atmosphere when a gas expands?
p ΔV.
35
What is the significance of the continuous-flow calorimeter?
It measures specific heat capacity without needing to know the thermal capacity of the apparatus.
36
What is the gain in potential energy of a molecule?
6.3 x 10-20 J molecule-1 ## Footnote Calculated using the formula: (18 x 10-3 kg x 2.1 x 106 J) / 6.x 10 23
37
What does the area under a pressure-volume graph represent?
The work done on or by a gas ## Footnote This is also referred to as an indicator diagram.
38
What is an isothermal change?
A change from P to Q where the gas expands at constant temperature ## Footnote Boyle’s law applies.
39
What happens to ΔU during an isothermal change?
ΔU = 0 ## Footnote There is no change in temperature.
40
What is the sign of ΔW during an isothermal expansion?
ΔW is negative ## Footnote Work is done by the gas as it expands.
41
What happens to ΔQ during an isothermal change?
ΔQ is positive ## Footnote Equal to the work done by the gas.
42
What is an isobaric change?
A change from Q to R when the gas is cooled at constant pressure ## Footnote Charles’ law applies.
43
What happens to ΔU during an isobaric change?
ΔU is negative ## Footnote The temperature is decreasing.
44
What is the sign of ΔW during an isobaric change?
ΔW is positive ## Footnote Work is done on the gas as it contracts.
45
What happens to ΔQ during an isobaric change?
ΔQ is positive ## Footnote Heat is removed from the gas to keep pressure constant.
46
What is an isovolumetric change?
A change from R to P where the gas is warmed at constant volume ## Footnote The pressure increases.
47
What happens to ΔW during an isovolumetric change?
ΔW is zero ## Footnote There is no change in volume.
48
What happens to ΔQ during an isovolumetric change?
ΔQ is positive ## Footnote Heat goes into the system to raise the pressure.
49
What happens to ΔU during an isovolumetric change?
ΔU is positive ## Footnote Equal to the heat going in.
50
What is an adiabatic change?
An expansion or contraction in which no heat enters or leaves the gas ## Footnote ΔQ is zero.
51
What happens to ΔW during an adiabatic expansion?
ΔW is negative ## Footnote Work is done by the gas as it expands.
52
What happens to ΔU during an adiabatic expansion?
ΔU is negative ## Footnote The internal energy is decreasing.