Thermal Energy and Heat Notes. Ch. 14

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1 Thermal Energy and Heat Notes Ch. 14

2 Temperature When scien<sts think about high and low temperatures they don t think about hot and cold. They think about par<cles of mader in mo<on

3 Temperature Defined as: a measure of the average kine<c energy of the individual par<cles Since all mader is made up of <ny par<cles and they are always in mo<on, even if the mader they make up is sta<onary. The faster the par<cles move, the more kine<c energy they have

4 Which has more kine<c energy? (answer on paper)

5 What happens if you heat the milk? (answer on paper)

6 Measuring Temperature Using a thermometer Narrow glass tube containing alcohol When heated, the par<cles of the liquid speed up and spread out so the par<cles of the liquid speed up and spread out. So, the par<cles take up more space or volume. This is why you see the level of the liquid rise When cooled the reverse happens, the par<cles slow down and come back together. So, the par<cles take up less space or volume and the liquid level lowers.

7 Temperature Scales Fahrenheit scale: most common in US, only 2 other countries use this Boiling point is 212 C Freezing point 32 C Celsius scale: used in nearly all other countries 1 degree Celsius is larger than one degree Fahrenheit Boiling point is 100 C Freezing point is 0 C

8 Temperature Scales Kelvin scale: commonly used in physical science Units on this scale are the same size as the Celsius scale So, an increase of 1 Kelvin is the same as an increase of 1 Celsius The degree is not used with this scale, you just say 1 Kelvin Boiling point: 373K Freezing point: 273K

9 Absolute zero The number 273 is very special. This is the number used to convert between Celsius and Kelvin ( C +273 = K) Also, C or 0 K is known as absolute zero This is the lowest possible temperature. At this point no more thermal energy can be removed and nothing moves (not even the par<cles that make up mader) Scien<sts have been able to get close this achieving this temperature in labs, but currently they have not been able to achieve absolute zero.

10 Check Point #1 1. Why do you have to mul<ply Fahrenheit by 5/9 to change to Celsius? 2. What are the freezing and boiling points on the Fahrenheit scale? 3. What is absolute zero on the Celsius scale? 4. What occurs at absolute zero? 5. What is absolute zero on the Kelvin scale? 6. What are the freezing and boiling points on the Celsius scale? 7. What are the freezing and boiling points on the Kelvin scale? 8. How does a thermometer work?

11 Thermal energy and Heat Different objects at the same temperature can have different energies. Temperature, thermal energy, and heat are closely related, but they are all different

12 Thermal Energy Thermal energy: total energy of all of the par<cles in an object. Measured in Joules Depends on the number of par<cles in the object, temperature of the object, and the arrangement of the par<cles. More par<cles an object has at a given temperature, the more thermal energy it has. The higher the temperature of an object, the more thermal energy it has (since the par<cles are moving more) Arrangement of par<cles depends on the phase of mader it s in (so, gases have the most thermal energy since their par<cles are moving the fastest).

13 Heat Defined as: the transfer of thermal energy from mader at a higher temperature to mader at a lower temperature. This is much different from its everyday use Objects contain thermal energy, not heat as we oien say in everyday conversa<on. Heat is thermal energy moving from a warmer object to a colder object. Since it is the transfer of thermal energy, it is measured in Joules.

14 Specific Heat Defined as: the amount of energy needed to raise the temperature of 1 kilogram of a material by 1 Kelvin. When an object is heated, its temperature rises. However, the temperature does not raise at the same rate for all objects. The rate temperature changes depends on the chemical makeup of the material If a material has a high specific heat it can absorb a great deal of thermal energy without a great change in temperature. On the other hand, a material with a low specific heat would have a large temperature change aier absorbing the same amount of thermal energy. This explains why sand changes temperature throughout the day while the ocean water does not. Sand has a specific heat of 800 J/ kg*k and water is 4,180 J/kg*K.

15 Check Point #2 1. Define temperature 2. Define thermal energy 3. Define heat 4. What three things does thermal energy depend on? 5. Which has more thermal energy: 1- liter pot of hot cocoa at 75 C or a 0.2- liter mug of hot cocoa at 75 C? Why? 6. Which has more thermal energy: an ice cube or a glass of water? Why? 7. Why do some materials get hot more quickly than others? 8. True of False: Objects contain heat 9. The specific heat of copper is 385 J/(kg*K) and the specific heat of sand is 800 J/(kg*K), which material will have temperature changes more quickly?

16 How is Heat Transferred? Conduc<on: heat is transferred from one par<cle to another without the movement of mader. Ex. Metal spoon in a pot of water on an electric stove: the fast moving paricles in the hot electric coil collide with the slow moving- moving par<cles in the cool pot. This causes the pot s par<cles to move faster, then the pot s par<cles collide with the water s par<cles. Which in turn collide with the par<cles of the spoon. As the par<cles move faster the spoon becomes hoder. There is not movement of mader, just the par<cles within it. The par<cles of one material collide with others that are touching it.

17 How is Heat Transferred? Convec<on: heat is transferred by the movement of currents within a fluid Ex. When the bodom of a pot is heated, its par<cles move faster and move further apart. This causes the water to become less dense (this cause the less dense, hea<ng water to float to the top). Then the surrounding cooler water (more dense) takes the place of the raising warmer water. This flow creates a circular mo<on known as a convec<on current. This works in all fluids (liquids and gases)

18 How is Heat Transferred? Radia<on: transfer of energy by electromagne<c waves Ex. You can feel the radia<on from a fire in a fireplace all the way across the room. The thermal energy radiates out of the fire and travels to you as electromagne<c waves. Unlike conduc<on and convec<on, radia<on does not require mader to transfer thermal energy.

19 Heat Moves One Way If two objects have different temperatures, heat will flow from the warmer to the colder one. This con<nues un<l both objects have the same temperature. Ex. A bowl of hot soup will cool to room temperature if you don t eat it fast enough. Heat transfer only occurs in one direc<on Ex. When making ice cream you might think the ice transfers cold to the ingredients, but actually the ingredients grow colder as they transfer thermal energy to the ice.

20 Conductors and Insulators Conductor: transfers thermal energy well Examples: metals such as silver and stainless steel A <le floor feels cool to the touch because it easily transfers thermal energy away from your skin Insulator: does not transfer thermal energy well Examples: wood, wool, straw, and paper Clothes and blankets are insulators that slow the transfer of thermal energy from your body

21 Check Point #3 1. Which type of heat transfer works currents in a fluid? 2. Which type of heat transfer occurs by direct contact? 3. Which type of heat transfer occurs with waves? 4. What direc<on does heat transfer occur? 5. Describe the difference between an insulator and a conductor.

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