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# Heat

Changes of state

Earth’s mantle convection

The triple point

Thermodynamics, an intro

Internal combustion engines

MCAS Heat Problems

Thermodynamics, an intro

Second law of thermodynamics

The Quantum Thermodynamics Revolution

Time’s Arrow Traced to Quantum Source

New resources to look at

https://www.ck12.org/physical-science/Thermal-Energy-in-Physical-Science/lesson/Thermal-Energy-MS-PS/

## Chapter 12: Thermal Energy

Introduction: How much heat energy is in sunlight? View this clip from “James May’s Big Ideas.” This parabolic mirror reflects infrared, visible and UV light energy from the sun, onto a focal point, producing about 1000 watts of power/square meter.

At the end of this chapter you should be able to answer MCAS heat problems.

## Thermal energy – Page 320

Molecule with vibrational KE

Molecule with rotational KE

Molecule with translational KE (moving sideways, without rotating)

A cup of water may appear to be still, yet the water molecules have KE.
Put a thermometer in it:
The temperature is the average amount of KE of the water molecules.

When the temperature of an object increases, the particles vibrate more rapidly, rotate faster, and move sideways with greater speed.

As water in a pot is heated, its molecules move with greater speed, reflected by a higher thermometer reading.

If a sample of water is placed in the freezer, its molecules move slower… reflected by a lower thermometer reading.

Additional info: How do thermomters work? physicsclassroom.com

Translational motion of atoms in a gas or liquid:

Vibrations of H2O molecules

http://www2.ess.ucla.edu/~schauble/MoleculeHTML/H2O_html/H2O_page.html

## Thermal Energy and Temperature (p.321)

What is temperature? Colloquial definition: The degree of hotness or coldness

Scientific definition: a measure of the average KE (kinetic energy) of the particles, in a sample of matter.

Question 2: What is figure 3 (p.321) showing us? Explain how this is possible.

## Equilibrium and thermometers p.322

3. How does heat transfer from your mouth to a thermometer?

4. What is thermal equilibrium?

5. Is there an upper limit to temperature? If so, what?
6. Is there an lower limit to temperature? If so, what?
7. On the Celsius scale, what is absolute zero?

## Temperature scales and thermometers p.324

There are three temperature scales

Fahrenheit
Water freezes at 32 degrees and boils at 212 degrees
There are 180 Fahrenheit degrees between the freezing point and the boiling point.

Celsius
Water freezes at 0 °C and boils at 100 °C.
There are 1o0 C degrees between the freezing point and the boiling point.
Therefore C degrees must be larger than F degrees.
Most of the world uses this scale.

Kelvin
Kelvin scale is useful because it starts at absolute zero.
A Kelvin temperature measures the actual energy of atoms – relative to zero energy.
There are 1o0 K degrees between the freezing point and the boiling point.
They are the same size as the Celsius degree.
Water freezes at 273K and boils at 373K.

Another way of viewing the 3 temperature scales.

Questions

8. Which degrees are smaller – C or F?

9. What is a normal body temperature in all 3 systems?

10. Does 0 degrees have any special meaning in the F system? C system? K system?

## Heat and Thermal Energy Transfer p.324-325

Three mechanisms of energy transfer as heat are conduction, convection, and radiation

Conduction
Touch a metal spoon that was left in a hot pan. Painful! Conduction is the transfer of heat, through matter: molecule energy is transferred – by collisions – from one molecule to another.

Metals are good conductors! (Don’t touch hot metal!) But air  is a poor conductor of heat. That’s why our winter jackets are filled with fluffy stuffing: the fluffy fibers in our jacket have only one job; trap air. The trapped air does the insulating!

Here are some metal atoms – notice how they vibrate, and transfer heat from one to the next: That is heat conduction. Hmm – metals atoms are also good at conducting electricity.

http://www.gcse.com/energy/conduction.htm

Look closely: The atoms are not touching each other.
Each metal atom has electrons, and a few of the electrons are free. They can leave their parent atom, and move around to nearby atoms. It becomes a sea of electrons, moving freely in a solid chunk of metal.
These free electrons transfer energy much faster than just vibrations.
That’s why metal is better at conducting heat than non-metals.

http://www.gcse.com/energy/conduction2.htm

Question

11. How is heat conducted through a solid object?

Convection
Here we see a flame heating up a pot of water.
Heated water expands & becomes less dense.
So the hot water (red) rises.
Eventually that water becomes cooler (bluer)
Cooler water contracts & becomes more dense
So the cooler water falls, and then eventually gets heated again.
The produces a cycle of motion that transfers heat.

This is how heat is transferred in our atmosphere:
Hot air rises, cool air descends.

Figure 7.5 in The Atmosphere, 8th edition, Lutgens and Tarbuck, 8th edition, 2001

Convection also takes place in solids, such as Earth’s mantle.
Yup, Earth’s mantle behaves like a fluid – over a long period of time.

Question

12. How does convection transfer heat in the atmosphere? Within the Earth?

Radiation travels out in all directions from its source. Unlike conduction and convection,which need material to travel through, radiant energy can travel through the vacuum of space. Solar energy reaches Earth by radiation.

## Specific Heat p.325-328

How much heat energy is needed to raise this 1 kg dumbbell by 1 degree?
How much heat energy is needed to raise this 1 kg chocolate by 1 degree?
It won’t be the same amount!

Different materials need a different amount of heat, to rise in temperature.

Specific heat = amount of heat needed to raise the temp of 1 kg of a material, by 1 degree ( C or K)

(This could also be in calories, instead of joules)

### Example specific heat capacities (What are the units? Read the vertical axis)

CPO Physical Science

Matter with high specific heat capacities take a lot of heat energy to heat up – and so need a long time to cool down.

How much heat energy is needed to raise some material, by a certain number of degrees?

Heat energy = mass x (specific heat capacity) x (temperature change)

The specific heat of gold is over 30 times smaller than that of water.
So with the same amount of added heat, a kg of gold will go from 20°C to 90°C
While a kg of water will only go from 20°C to 22°C.

Specific heat of gold is 0.031 calories per gram per degree Celsius (0.031 cal/g·°C).

For example, the specific heat of gold is over 30 times smaller than that of water. In other words, a kilogram of gold will go from 20°C to 90°C, while water will only go from 20°C to 22°C when they both are heated equally. The specific heat of gold is 0.031 calories per gram per degree Celsius (0.031cal/g·°C).

Why such a big difference?

lesson https://arenahanna.wordpress.com/specific-heat-energy/

Each material have a different rate of heating. Here we see that gold heats up 7 times faster than aluminum.
Everything has its own specific heat (aka heat capacity). A
luminum’s specific heat is 0.216 cal/g·°C, 7 times more than that of gold (0.031 cal/g·°C).

Questions:

Carefully study the example problem on page 326.
Following this same format, solve problems #1, 2 and 3.

At the end of this chapter you should be able to answer MCAS heat problems.

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AP Physics PowerPoint: Heat Kinetic Theory Giancoli Chap 13

## Learning Standards

2016 Massachusetts Science and Technology/Engineering Curriculum Framework

7.MS-PS3-5. Present evidence to support the claim that when the kinetic energy of an object changes, energy is transferred to or from the object. Examples of empirical evidence could include an inventory or other representation of the energy before and after the transfer in the form of temperature changes or motion of an object.

7.MS-PS3-6(MA). Use a model to explain how thermal energy is transferred out of hotter regions or objects and into colder ones by convection, conduction, and radiation.

8.MS-PS1-4. Develop a model that describes and predicts changes in particle motion, relative spatial arrangement, temperature, and state of a pure substance when thermal energy is added or removed. Emphasis is on qualitative molecular-level models of solids, liquids, and gases to show that adding or removing thermal energy increases or decreases kinetic energy of the particles until a change of state occurs

HS-PS3-2. Develop and use a model to illustrate that energy at the macroscopic scale can be accounted for as either motions of particles and objects or energy stored in fields.
Clarification Statements: Examples of phenomena at the macroscopic scale could include evaporation and condensation, the conversion of kinetic energy to thermal energy,

HS-PS3-4a. Provide evidence that when two objects of different temperature are in thermal contact within a closed system, the transfer of thermal energy from higher temperature objects to lower-temperature objects results in thermal equilibrium, or a more uniform energy distribution among the objects and that temperature changes
necessary to achieve thermal equilibrium depend on the specific heat values of the two substances. Energy changes should be described both quantitatively in a single phase (Q =m·c·∆T) and conceptually either in a single phase or during a phase change.