THERMODYNAMICS. Thermodynamics is the study of energy relationships that involve heat, mechanical work, and other aspects of energy and heat transfer.

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1 THERMODYNAMICS Thermodynamics is the study of energy relationships that involve heat, mechanical work, and other aspects of energy and heat transfer. Central Heating

2 Objectives: After finishing this unit, you should : Be familiar with & able to convert between the 3 temperature scales (Celcius, Farenheit, & Kelvin. Define temperature, heat, & energy and discuss their relationship with each other. Know & apply the 3 methods of Heat transfer and understand Thermal Equilibrium. Calculate & apply knowledge of Specific Heat Capacity. State and apply the four laws of thermodynamics.

3 Physics Classroom Use the physics classroom website to complete your notes information. Study the quiz review & take Quiz #1 Intro to Thermodynamics Complete the Thermochemistry Notes WS.

4 Specific Heat Capacity Use the next few slides to fill in VII of your notes. Add any extra info into your notes

5 Heat Energy don t need to write out! The amount of heat energy needed to change the temperature of a substance depends on: (a) what the substance is; (b) how much of it is being heated; (c) what rise in temperature occurs.

6 Specific Heat Capacity Define: The amount of heat energy needed to raise 1 g of a substance by 1 o C Formula: Q= m Cp T T = Tf Ti (what does each variable stand for?) Watch the units of mass and the units in the Cp they must match up

7 Specific Heat Capacity do not need to memorize values Specific heat capacity is given the symbol Cp. The units for Cp are J/(kg K) or J/(kg o C). Sometimes you will see the unit g for mass. The values for the specific heat capacities of some common substances are given in the following table: Substance Specific heat capacity (J/kg K) Substance Specific heat capacity (J/kg K) Water 4200 Aluminium 913 Cast iron 500 Brick 840 Copper 385 Concrete 880 Lead 126 Marble 880

8 Specific Heat Capacity Substances with high specific heat capacities can absorb or release large quantities of heat energy BEFORE their temperatures ever change. Therefore they take a long time to heat up and also a long time to cool down.

9 Specific Heat Capacity Applications One interesting effect is the way in which the land heats up quicker than the sea - the specific heat capacity of sea water is greater than that of the land and so more heat energy is needed to heat it up by the same amount as the land and so it takes longer. It also takes longer to cool down.

10 Application: Insulators & Conductors Insulators are materials with High specific heat capacities that resist changes in their temperature. Conductors are materials with Low specific heat capacities that change temperatures more quickly.

11 Complete your SHC practice worksheet. Then you can get the real WS! Show all your problem setup & be sure to put the correct unit on your answers! Due Wednesday for a grade!

12 Write these next few slides on the last page of your notes. They are explanation information for what we will be discussing in VIII

13 Phases of matter Particle arrangement Volume? Shape? Know the basic differences in the phases

14 Effects of Heating & Cooling Heating up substances makes the molecules move faster and farther apart (increases the KE) Cooling substances (making the heat leave) makes the molecules move slower and come closer together (decreases KE)

15 Phase Changes complete columns 1 & 2 of the chart in your notes pg 3. Process Melting Freezing Vaporization Condensation Sublimation Deposition Change of State Solid to Liquid Liquid to Solid Liquid to Gas Gas to Liquid Solid to Gas Gas to Solid

16 Phases of Matter A phase change is a physical change of matter. The substance does not change only the form it is in. If energy is added (like increasing the temperature) or if energy is taken away (like freezing something), you have created a physical change.

17 Endothermic vs. Exothermic + or shows direction of energy flow (into or out of object) Endothermic: energy is going into the substance (or being absorbed) Exothermic: Energy is going out of the substance (being released) Complete the chart: Think about which processes must have heat put IN to cause the change and vice versa.

18 Phase Diagram indicates phases at different temperature & pressure combinations. Add a labeled sketch to your notes You will need to be able to read a phase diagram. 1 atm is average land level pressure

19 Phase Change Diagram shows relationship between temperature, time and phase See the diagram example at the bottom of page 3 of your notes. Color the red/blue lines in your notes! The correct formulas are listed at each place on the diagram You need to be able to read a phase change diagram.

20 Now complete your WS on Specific Heat and your WS on phase diagrams & phase changes. They are all due tomorrow!!

21 Thermal Expansion Define: increase in dimensions of a solid or in volume of a fluid because of rise in temperature Each substance has its own set of thermal expansion values Used in construction of buildings, bridges, etc.

22 Thermal Expansion

23 Thermal Expansion

24 Latent heats Latent heat: The quantity of heat absorbed or released by a substance during the actual phase change. (flat line portion of graph) This heat is energy working on the actual atoms position so it causes no temperature change until all the atoms are ready.

25 Latent Heat Δh fusion : Latent heat of fusion Δh vaporization : Latent heat of vaporization We will practice with an EC WS in a minute

26 Calorimetry Science of determining changes of energy in a SYSTEM by measuring heat energy exchanged with SURROUNDINGS. Calorimeter: The device used to measure the quantity of heat transferred to or from an object. Application: used to determine calories in food.

27 Calorimeters

28 Calories vs. Joules To convert between calories and joules: 1 Calorie (kcal) = kilojoules (kj) Our food calories are really Calories (kilocalories)!

29 Laws of Thermodynamics

30 Zeroth Law Law of Thermal Equilibrium When two systems are sitting in equilibrium with a third system, they are also in thermal equilibrium with each other When systems come in contact with each other, they will transfer energy in order to reach thermal equilibrium.

31 1 st law of Thermo Law of Thermal Conservation Heat energy cannot be created or destroyed only converted into different forms. The energy of an entire system will stay constant.

32 2 nd law of Thermo Law of Entropy The entropy of an isolated system not in equilibrium will tend to increase over time, approaching a maximum value at equilibrium. Entropy: the degree of disorder in a system. (how much the energy is spread out Entropy is always either staying constant or increasing. Entropy never decreases!

33 3 rd law of Thermo As the temperature of a system approaches absolute zero the entropy approaches a minimum. Just think about it: When all molecular motion stops, there can be nothing spreading out

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