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Physics 1. Thermal Physics Chapters 21-23. Links: http://homepage.mac.com/phyzman/phyz/BOP/2-06ADHT/index.html and http://www.colorado.edu/physics/2000/index.pl. What do you think? know?. Why does popcorn pop?

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Physics 1

Physics 1

Thermal Physics

Chapters 21-23

Links: http://homepage.mac.com/phyzman/phyz/BOP/2-06ADHT/index.html and http://www.colorado.edu/physics/2000/index.pl


What do you think know
What do you think? know?

  • Why does popcorn pop?

  • On a camping trip, your friend tells you that fluffing up a down sleeping bag before you go to bed will keep you warmer than sleeping in the same bag when it is still crushed. Why?


3. Why is it difficult to build a fire with damp wood?

4. Why does steam at 100oC cause more severe burns than liquid water does at 100oC?


5. Until refrigerators were invented, many people stored fruits and vegetables in underground cellars. Why was this more effective than keeping them in the open air?

6. In the past, when a baby had a high fever, the doctor might have suggested gently sponging off the baby with rubbing alcohol. Why would this help?


7. Why does water expand when it freezes? fruits and vegetables in underground cellars. Why was this more effective than keeping them in the open air?

8. Why, during the final construction of the St. Louis arch, was water sprayed on the previous sections as the last section was put in place?


Objectives
Objectives fruits and vegetables in underground cellars. Why was this more effective than keeping them in the open air?

  • 1. Describe thermal energy and compare it to potential and kinetic energies.

  • 2. Describe changes in temperatures of two objects reaching thermal equilibrium

  • 3. Identify various temperature scales, and convert between them


Objectives1
Objectives fruits and vegetables in underground cellars. Why was this more effective than keeping them in the open air?

  • 4. Explain heat as energy transferred between substances at different temperatures in one of 3 ways (conduction, convection, radiation)

  • 5. Relate heat and temperature

  • 6. Apply principle of energy conservation to calculate changes in potential, kinetic, & internal energy


Objectives2
Objectives fruits and vegetables in underground cellars. Why was this more effective than keeping them in the open air?

  • 7. Perform calculations with specific heat capacity

  • 8. Interpret the various sections of a heating curve


Objectives3
Objectives fruits and vegetables in underground cellars. Why was this more effective than keeping them in the open air?

  • 9. Recognize that a system can absorb or release energy as heat in order for work to be done on or by that system

  • 10. Compute work done during thermodynamic process

  • 11. Distinguish between isovolumetric, isothermal, and adiabatic thermodynamic processes


Objectives4
Objectives fruits and vegetables in underground cellars. Why was this more effective than keeping them in the open air?

  • 12. Illustrate how the first law of thermodynamics is a statement of energy conservation

  • 13. Calculate heat, work, and change in internal energy using lst law of T-D

  • 14. Apply 1st law of T-D to describe cyclic processes

  • 15. Recognize why 2nd law of T-D requires 2 bodies at different temps.


1 relate temperature to the kinetic energy of atoms and molecules
1.Relate temperature to the kinetic energy of atoms and molecules

  • Temperature scales

  • In the USA, the Fahrenheit temperature scale is used. Most of the rest of the world uses Celsius, and in science it is often most convenient to use the Kelvin scale.

  • The Celsius scale is based on the temperatures at which water freezes and boils. 0°C is the freezing point of water, and 100° C is the boiling point. Room temperature is about 20° C, a hot summer day might be 40° C, and a cold winter day would be around -20° C.

  • To convert between Fahrenheit and Celsius, use these equations:


21.1 moleculesTemperature

Temperature and Kinetic Energy

Temperature is related to the random motions of the molecules in a substance.

In the simplest case of an ideal gas, temperature is proportional to the average kinetic energy of molecular translational motion.


  • Convert 72 moleculesoF to oC

  • C = 5/9 (F-32)

  • C = 5/9 (72-32) = 22oC

  • Convert -10 oC to oF

  • F = 9/5 C + 32

  • F = 9/5(-10) + 32 = 14oF


Objective 3: molecules

Temperature Scales

Temperature degree scales comparison


Celsius to Kelvin: T = Tc + 273.15 molecules

Problem:

1. The lowest outdoor temperature ever recorded on Earth is -128.6 o F., recorded at Vostok Station, Antarctica, in 1983. What is this temperature on the Celsius and Kelvin scales?

Answers: -89.22oC, 183.93 K


  • Obj. #2 - Hotter temperature means molecules

  • – more heat present in a substance

  • – the faster the molecules of the substance move.

  • Obj #5 – Relate heat and temperature

  • Heat units: calorie or joule (amount of heat energy present in a substance)

  • Temperature units: degree (proportional to heat energy present in a substance)


21.2 moleculesHeat

If you touch a hot stove, energy enters your hand from the stove because the stove is warmer than your hand.

If you touch ice, energy passes from your hand into the colder ice.

The direction of spontaneous energy transfer is always from a warmer to a cooler substance.

The energy that transfers from one object to another because of a temperature difference between them is called heat.

Heat unit: calories or Joules (4.186 J/cal)


2 describe changes in temperatures of two objects reaching thermal equilibrium
2.Describe changes in temperatures of two objects reaching thermal equilibrium

  • The temperature of the hotter substance will decrease. The temperature of the colder substance will increase. Each change will stop when the temperatures are the same – thermal equilibrium. In other words, thermal energy travels from hot to cold.

  • Obj. #4 - Heat energy can be transferred by

    • Convection (motion of fluid), conduction (touching), or radiation (electromagnetic waves)


Convection thermal equilibrium

Heat transfer in fluids generally takes place via convection. Convection currents are set up in the fluid because the hotter part of the fluid is not as dense as the cooler part, so there is an upward buoyant force on the hotter fluid, making it rise while the cooler, denser, fluid sinks.

Conduction

When heat is transferred via conduction, the substance itself does not flow; rather, heat is transferred internally, by vibrations of atoms and molecules.


Radiation: thermal equilibrium

energy is transferred in the form of electromagnetic waves.


22.1 thermal equilibriumConduction

  • Touch a piece of metal and a piece of wood in your immediate vicinity. Which one feels colder? Which is really colder?

    • If the materials are in the same vicinity, they should have the same temperature, room temperature.

    • The metal feels colder because it is a better conductor.

    • Heat easily moves out of your warmer hand into the cooler metal.

    • Wood, on the other hand, is a poor conductor.

    • Little heat moves out of your hand into the wood, so your hand does not sense that it is touching something cooler.


22.1 thermal equilibriumConduction

The good insulating properties of materials such as wool, wood, straw, paper, cork, polystyrene, fur, and feathers are largely due to the air spaces they contain.

Birds fluff their feathers to create air spaces for insulation.

Snowflakes imprison a lot of air in their crystals and are good insulators. Snow is not a source of heat; it simply prevents any heat from escaping too rapidly.


22.1 thermal equilibriumConduction

Strictly speaking, there is no “cold” that passes through a conductor or an insulator.

Only heat is transferred. We don’t insulate a home to keep the cold out; we insulate to keep the heat in.

No insulator can totally prevent heat from getting through it. Insulation slows down heat transfer.


22.2 thermal equilibriumConvection

Convection occurs in all fluids, liquid or gas.

When the fluid is heated, it expands, becomes less dense, and rises.

Cooler fluid then moves to the bottom, and the process continues.

In this way, convection currents keep a fluid stirred up as it heats.


22.5 thermal equilibriumAbsorption of Radiant Energy

A blacktop pavement and dark automobile body may remain hotter than their surroundings on a hot day.

At nightfall these dark objects cool faster! Sooner or later, all objects in thermal contact come to thermal equilibrium.

So a dark object that absorbs radiant energy well emits radiation equally well.


22.3 thermal equilibriumRadiation

  • Radiant energy is any energy that is transmitted by radiation.

  • From the longest wavelength to the shortest, this includes:

    • radio waves,

    • microwaves,

    • infrared radiation,

    • visible light,

    • ultraviolet radiation,

    • X-rays,

    • and gamma rays.


22.3 thermal equilibriumRadiation

  • Radio waves send signals through the air.

  • You feel infrared waves as heat.

  • A visible form of radiant energy is light waves.


22.3 thermal equilibriumRadiation

Most of the heat from a fireplace goes up the chimney by convection. The heat that warms us comes to us by radiation.


22.5 thermal equilibriumAbsorption of Radiant Energy

Good emitters of radiant energy are also good absorbers; poor emitters are poor absorbers.


22.5 thermal equilibriumAbsorption of Radiant Energy

  • Because the sun shines on it, the book absorbs more energy than it radiates.

    • Its temperature increases.

    • As the book gets hotter, it radiates more energy.

    • Eventually it reaches a new thermal equilibrium and it radiates as much energy as it receives.

    • In the sunshine the book remains at this new higher temperature.


22.6 thermal equilibriumNewton’s Law of Cooling

An object hotter than its surroundings eventually cools to match the surrounding temperature.

Its rate of cooling is how many degrees its temperature changes per unit of time.

The rate of cooling of an object depends on how much hotter the object is than the surroundings.


Specific heat capacity
Specific heat capacity thermal equilibrium

The amount of energy that must be added to raise the temperature of a unit mass of a substance by one temperature unit.

  • Units: cal/goC

  • For Water: 4.186 J/goC

  • For Aluminum: 0.900 J/goC

  • Which one heats faster?


21.6 thermal equilibriumSpecific Heat Capacity

think!

Which has a higher specific heat capacity—water or sand? Explain.


21.6 thermal equilibriumSpecific Heat Capacity

think!

Which has a higher specific heat capacity—water or sand? Explain.

Answer:

Water has a greater heat capacity than sand. Water is much slower to warm in the hot sun and slower to cool at night. Sand’s low heat capacity, shown by how quickly it warms in the morning and how quickly it cools at night, affects local climates.


A table similar to this is on page 413 of the Hewitt book. thermal equilibrium

Not shown: Clay (14,000), Olive Oil (19,700), and Steel (448)


Heat transfer q mc t mc t f t i
Heat Transfer thermal equilibriumQ = mCΔT = mC (Tf – Ti)

  • Heat Transfer

  • Q = mcΔT = mc(Tf – Ti)

  • Q, quantity of heat in joule

  • m, mass of substance in g

  • c, specific heat for water in 4.186 J/goC

  • t, temperature in Celsius


See table 12-1 on page 318 thermal equilibrium

Find the amount of heat needed to change the temperature of 5.0 g of liquid water from 8.0oC to 100oC.

Q = mcDt = 5.0g(4.186 J/goC) (92oC) = 1.9 x 103 J

Again,

specific heat is the amount of heat necessary to change one g of a substance 1 degree Celsius or Kelvin.


  • 12/3 When you turn on the hot water to wash dishes, the water pipes have to heat up. How much heat is absorbed by a copper water pipe with a mass of 2.3 kg when its temperature is raised from 20.0oC to 80.0oC?

  • Q = mcDt

  • Q = (2300g)(0.386J/goC)(60.0oC)

  • Q = 53268 J or 5.3x104 J


Q = mc water pipes have to heat up. How much heat is absorbed by a copper water pipe with a mass of 2.3 kg when its temperature is raised from 20.0Dt

Dt = Q

mc

Dt = 836,000 J goC

20,000g (4.186 J)

Dt = 9.98oC


Specific heat capacities
Specific Heat Capacities water pipes have to heat up. How much heat is absorbed by a copper water pipe with a mass of 2.3 kg when its temperature is raised from 20.0

Which

one is

greatest

that you

use

everyday?

OR J/kgoC


Law of heat exchange q lost q gained
Law of Heat Exchange water pipes have to heat up. How much heat is absorbed by a copper water pipe with a mass of 2.3 kg when its temperature is raised from 20.0 Q lost = Q gained


Emily is testing her baby’s bath water and finds that it is too cold so she adds some hot water. If she adds 2.00 kg of water at 80.0oC to 20.0kg of bath water at 27.0 oC, what is the final temperature of the bath water?

Q lost = Q gain

2.00kg(1cal)(80oC-tf) = 20.0kg(1cal)(tf-27oC)

goC goC

160 – 2tf = 20 tf – 540

-22 tf = -700

tf = 31.8oC


Latent heat is energy transferred during phase changes
Latent Heat is energy transferred during phase changes is too cold so she adds some hot water. If she adds 2.00 kg of water at 80.0oC to 20.0kg of bath water at 27.0 oC, what is the final temperature of the bath water?

Crystalline materials change phase -- melt and freeze or vaporize and condense -- at a single, fixed temperature. Energy is required for a change of phase of a substance. It is called latent heat because there is no change or difference in temperature.

Latent heat of fusion Lf describes the heat necessary to melt (or freeze) a unit mass of a substance.Q = m Lf

Latent heat of vaporization Lv describes the heat necessary to vaporize (or condense) a unit mass of a substance.

Q = m Lv


Temperature vs heat
Temperature vs Heat is too cold so she adds some hot water. If she adds 2.00 kg of water at 80.0oC to 20.0kg of bath water at 27.0 oC, what is the final temperature of the bath water?


Formulas
Formulas is too cold so she adds some hot water. If she adds 2.00 kg of water at 80.0oC to 20.0kg of bath water at 27.0 oC, what is the final temperature of the bath water?

  • Temperature change use: Q = mc D t

  • Melting or freezing: Q = m Lf

  • Evaporation or Condensation: Q = mLv

  • Lf is latent heat of fusion, 80 cal/g

  • Lv is latent heat of vaporization, 540 cal/g

  • These values are for water.


How much heat must be gained by 0.100 kg of ice at 0 oC in order for all of it to melt?

Q = m Lf

Q = 100g (80cal)

g

Q = 8000 or 8.00 x 103 g


Q = mc order for all of it to melt?Dt + mLf Specific Heat of Ice = 0.49 cal

g oC

Q = 100g(0.49cal)(20.0 oC) + 100g(80cal)

g oC g

Q = 8980 = 8.98 x 103 cal


Problem
Problem order for all of it to melt?

  • A jar of tea is placed in sunlight until it reaches an equilibrium temperature of 32oC. In an attempt to cool the liquid to 0oC, which has a mass of l80 g, how much ice at 0oC is needed? Assume the specific heat capacity of the tea to be that of pure liquid water.


  • m tea = 180g m ice = ? which is the mass of the water that has melted

  • c tea = c water = 4186 J/kgoC

  • H f = 3.33 x 105 J/kg and t final = 32oC

  • Q lost = Q gained tea loses and water gains only melting the ice

  • (mcDt)tea = (mHf)ice

  • m ice= (mcDt)tea

  • Hfice

  • m ice = (.180kg)(4186J/kgoC)(32oC)

  • 3.33x105 J/kg

  • = 7.2 x 10-2kg


1 st law of thermodynamics
1 has meltedst Law of Thermodynamics

  • U = Q - W

    The change in thermal energy of an object is equal to the heat added to the object minus the work done by the object.

See Fig 12-11 on

Page 326


A heat engine
A heat engine has melted

Transforms heat at high temperature into mechanical energy and low-temperature waste heat

A heat pump (refrigerator) absorbs heat from the cold reservoir and gives off heat to the hot reservoir.


2 nd law of thermodynamics
2 has meltednd Law of Thermodynamics

  • In the 19th Century French engineer Sadi Carnot studied the ability of engines to convert thermal energy into mechanical energy.

  • He developed a logical proof that even an ideal engine would generate some waste heat.

  • Carnot’s result is best described by the term entropy which is the measure of the disorder in a system.


  • The change is entropy, D S, is shown by the equation: has melted

  • S = Q / T Units: J/K

    The change in entropy of an object is equal to the heat added to the object divided by the temperature of the object.

    Natural processes occur in a direction that increases the entropy of the universe. All processes tend toward disorder unless some action occurs to keep them ordered. i.e., heat can flow only from hot to cold naturally.


Practice problems
Practice Problems has melted


12 32 answer
12/32 answer has melted


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