For more information, please see full course syllabus of High School Physics

For more information, please see full course syllabus of High School Physics

### Change Due to Heat

- As an object's temperature rises, its dimensions will begin to increase. Different materials have different coefficients of linear expansion (α). The change in length is given by
∆L = L α(∆T). - Similarly, the volume will also increase as the temperature rises. The coefficient of volume expansion is β = 3α.
∆V = V β(∆T). - The above two formulas do
__not__work for gases. They work fine for solids and liquids, but because gases already expand to fill their container, we need a different equation. And for that, we need- - -The
*Mole*(mol) is a measure of how many atoms/molecules/objects there are in a substance. If m is the__molecular mass__of the substance and M is the mass of the substance in, then n=[M/m] is the number of moles.__grams__ - In a mole there are N
_{A}= 6.022 ·10^{23}[objects/mol]. This is called*Avogadro's number*. - We can model the behavior of a gas with the
*Ideal Gas Law*:pV = nRT. - p is the pressure of the gas. [Note:
__absolute__, not gauge pressure]. - V is the volume of the gas.
- n is the number of moles of gas.
- R is the
*gas constant*: R = 8.314 [J/(mol·K)]. - T is the temperature (in
__kelvin__) of the gas.

- p is the pressure of the gas. [Note:
- As more and more thermal energy is added to a substance, it will change phase: first from solid to liquid, then from liquid to gas. If thermal energy is removed, it will do the reverse. The specific change over temperatures vary depending on pressure.
- It takes thermal energy to change phase. The amount of heat depends on the substance and the mass of the object:

where L is a proportionality constant that varies depending on substance and phase type. This heat is put into the substance if it is going to a higher energy phase, and removed if going to a lower energy phase.Q = Lm,

### Change Due to Heat

Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.

- Intro
- Linear Expansion
- Volume Expansion
- Gas Expansion
- The Mole
- Ideal Gas Law
- Ideal Gas Law: pV = nRT
- p = Pressure of the Gas
- V = Volume of the Gas
- n = Number of Moles of Gas
- R = Gas Constant
- T = Temperature
- A Note On Water
- Change of Phase
- Heat of Transformation
- Example 1: Linear Expansion
- Example 2: Explore Why Î² = 3Î±
- Example 3: Ideal Gas Law
- Example 4: Heat of Transformation

- Intro 0:00
- Linear Expansion 1:06
- Linear Expansion: âˆ†L = Lα(âˆ†T)
- Volume Expansion 2:34
- Volume Expansion: âˆ†V = Vβ(âˆ†T)
- Gas Expansion 3:40
- Gas Expansion
- The Mole 5:43
- Conceptual Example
- The Mole and Avogadro's Number
- Ideal Gas Law 9:22
- Ideal Gas Law: pV = nRT
- p = Pressure of the Gas
- V = Volume of the Gas
- n = Number of Moles of Gas
- R = Gas Constant
- T = Temperature
- A Note On Water 12:21
- A Note On Water
- Change of Phase 15:55
- Change of Phase
- Change of Phase and Pressure
- Phase Diagram
- Heat of Transformation 20:38
- Heat of Transformation: Q = Lm
- Example 1: Linear Expansion 22:38
- Example 2: Explore Why β = 3α 24:40
- Example 3: Ideal Gas Law 31:38
- Example 4: Heat of Transformation 38:03

### High School Physics Online Course

### Transcription: Change Due to Heat

*Hi. Welcome back to educator.com. Today weâ€™re going to be talking about changes due to heat.*0000

*Weâ€™re already talked about how more thermal energy in a substance causes the molecules of the atoms in the substance to vibrate more and more.*0007

*As those molecules vibrate more against one another theyâ€™re going to be bouncing off each other more often.*0014

*Theyâ€™re going to push against each other harder. So as they push harder against each other, theyâ€™re going to have more pressure in between them which is going to cause the substance to expand some amount.*0020

*If itâ€™s a solid substance, we wonâ€™t see much expansion. If itâ€™s a liquid substance, weâ€™ll see of that internal pressure in the thermal energy will cause things to push out slightly, a little bit more push in our thing.*0030

*Itâ€™s going to grow a little bit. At very high levels of vibration, very high levels of thermal energy the material will actually change phases as the pressures inside the vibrations inside become so large that theyâ€™re able to break being in a solid substance and become able to just move on each other fluidly.*0043

*Like a in a liquid. Then eventually so much that theyâ€™re able to completely pull off of one another and turn into a gas.*0059

*First idea, linear expansion. When we heat or cool any substance weâ€™re going to get some slight fluctuations in size.*0068

*The amount of that fluctuation is going to depend on the original length of the object, l. The specific properties of the substance.*0074

*Some substances will wind up expanding a lot more; some of them wonâ€™t expand very much.*0080

*The change in temperature delta t. Put together we get the equation delta l is equal to l times alpha times our change in temperature.*0084

*Even the ones that are large fluctuations, the large alphas are still pretty small.*0093

*All of these alphas are very small. Itâ€™s going to basically vary somewhere between 10^-6 and 10^-4 for most substances.*0098

*Even a really big alpha is still a huge amount of temperature going to have to be changed before weâ€™re actually going to have any really noticeable difference that weâ€™d be able to see with a naked eye.*0105

*For the most part we arenâ€™t going to actually see this sort of thing. It will have effects on very large structures though, say if you were to build a bridge, youâ€™d want to be able to have that bridge expand and contract without ripping itself apart or smashing into itself.*0116

*They wind up creating these slots like this so that the bridge can expand into the slots and pull back out without completely ripping itself apart.*0129

*If they were to build one long many hundreds of meters continuous bridge, when it got very hot it might expand so much that it actually causes itself to pull apart.*0140

*Itâ€™s really important to have those contractions and expansion points otherwise bridges wouldnâ€™t be able to be built.*0149

*Linear expansion is great and thatâ€™s really interesting, but thatâ€™s not enough to describe lots of things out there.*0156

*If we wanted to talk about volume expansion, if we wanted to talk about how much liquid in a cup, what its volume changes to as it gets hotter, it will change.*0162

*Since its length is changing, but we donâ€™t have length in a liquid. We canâ€™t pour something into some funny shaped container, we canâ€™t pour water into this funny shaped container and say â€˜Oh look that has a length ofâ€¦â€™*0171

*It doesnâ€™t make sense. We canâ€™t sayâ€¦we canâ€™t put a width and length and a depth and be able to easily come up with cubic volume.*0184

*Instead we just need to be able to talk about volume direct. So itâ€™s very similar, itâ€™s going to be that the change in v is equal to the original volume times beta, the new coefficient for that times the change in temperature.*0191

*Beta is related to our original alpha and beta equals 3xalpha.*0203

*Why is that the case? Weâ€™ll explore this actually in example two.*0208

*Itâ€™s going to turn out that beta isnâ€™t precisely equal to 3alpha but itâ€™s good enough that itâ€™s going to work for all of our purposes and most purposes youâ€™re going to possibly have.*0212

*Finally weâ€™re ready to talk about gas expansion. Solids, liquids, they bothâ€¦they push against one another theyâ€™re going to expand out just a little bit as they get higher and higher temperatures theyâ€™re going to push harder.*0221

*But a gas, itâ€™s already pushing hard enough and bouncing off of itself. If you put it into a container, it fills out the whole container.*0231

*Itâ€™s not like liquid where it just fills up to the level you poured it in or solid where it just sits there.*0237

*A gas is going to expand to whatever container size itâ€™s put inside.*0242

*Since gas isâ€¦are already completely filling the container, theyâ€™re not going to expand the way we talk about liquid and solids expanding.*0246

*Instead weâ€™ll talk about how hard theyâ€™re pushing. How hard are they pushing against the walls of the containers and how hard theyâ€™re pushing against each other.*0253

*Itâ€™s their pressure. In addition weâ€™ll also have to talk about the size of the container, v and the temperature of the gas, t, and how many molecules are in that gas.*0261

*If we had a box with one atom in it. One single atom in it bouncing around, itâ€™s not going to have that many bounces.*0270

*If we give it a certain temperature and the same volume, itâ€™s not going to have that many bounces because itâ€™s just one atom.*0278

*If we were to do the same thing, same size box but now we put in 10 different atoms.*0285

*If itâ€™s go the same temperature, meaning that each of the atoms is moving at the same rate as this one over here.*0295

*If weâ€™ve got the same temperature between those two boxes, weâ€™re going to get way more bounces going on in that second box.*0301

*That means that second box is hitting things more often. Means itâ€™s pushing against stuff more often.*0306

*It keeps bouncing off repeatedly, that effectively turns into one continuous push when youâ€™ve got millions upon millions upon millions upon millions of molecules doing all of these pushes one after another.*0311

*Thatâ€™s what weâ€™re going to feel as pressure. Itâ€™s going to really matter how many of these molecules, how many of these atoms do we have doing the bouncing.*0322

*Thatâ€™s going to be a really important idea but we havenâ€™t talked about a way to describe how many molecules, how many atoms we have.*0329

*Thatâ€™s going to bring up an entirely new idea; itâ€™s going to bring up the mol, which we shorten to m o l.*0335

*Now we need to talk about mols. Real quick, letâ€™s say you worked in a nail factory and you had a crate of nails.*0342

*If you needed to know how many nails where in the crate you could count them but that would be a really, really slow process.*0349

*Say you have a big crate of nails, thatâ€™s going to take you hours if not days to be able to count through each of those nails by hand.*0354

*Thatâ€™s not a very good way to figure out how many nails youâ€™ve got in the crate.*0362

*But you might still need to know how many nails you have in the crate if youâ€™re going to do some sort of job in construction or try to sell it somebody; youâ€™re going to need to know how many nails are present.*0365

*So what you can do instead is you could measure the mass per quantity for a small amount.*0372

*You might be able to figure out â€˜Oh, for every kilogram of nails I have, Iâ€™ve got 230 nails in that kilogram.â€™*0379

*Youâ€™d be able to come up with a conversion ratio of 230 nails per kilograms. Now if youâ€™ve got that you can just dump the whole crate onto a scale.*0386

*You weigh all of those nails at once and boom; just with a little bit of math youâ€™re able to figure out â€˜Oh thatâ€™s how many nails Iâ€™ve got.â€™*0394

*Way, way easier than trying to sit there and do it by hand. Now imagine if you were trying to do something like count molecules.*0401

*Thereâ€™s no way we could count it by hand. First off, thereâ€™s way too many molecules for us to ever have any hope of counting something by hand.*0408

*Two, I canâ€™t pick up a molecule. Can you? I can pick up a bunch of molecules at once, but I certainly canâ€™t just pick up one individually and put it over somewhere else.*0413

*Weâ€™ve got no hope of counting molecules but this idea of being able to change mass for quantity is going to work perfectly for us.*0421

*In general if you know how many objects are some unit mass, you can easily count a substance by using its weight.*0429

*You figure out what its weight is depending on what local gravity is. In our case weâ€™re on Earth, youâ€™re probably going to be using 9.8.*0434

*You figure out what its weight is, you then figure out what the mass is from that and using that mass you can boomâ€¦if youâ€™ve got a conversion ratio you can easily find out how many of the thing youâ€™ve got.*0440

*With that idea we can do the exact same thing with molecules. Since every atom or molecule already has an atomic or molecular mass.*0449

*Where molecular mass is just adding up all of the atomic masses for the number of oneâ€™s weâ€™ve got.*0459

*Depending on what the molecule is. We can connect that to the masses we can measure.*0463

*Weâ€™ve got this idea of molecular mass. You figure out what he molecular mass for your molecule is or the atomic mass if itâ€™s just a single atom.*0468

*Let little m be the molecular mass. So little m is the molecular mass, we can now also weigh the quantity we have.*0476

*Say weâ€™ve got some pure amount of lead. We know itâ€™s just lead so we go, we look up the atomic weight for lead and then weigh the quantity of lead we have.*0483

*We measure it in grams. Itâ€™s really important to notice it is grams that weâ€™re using. Itâ€™s not kilograms.*0493

*We normally use kilograms for everything else but we get this idea from Chemistry and because weâ€™re dealing with normally small quantities, we use grams.*0499

*Measure mols in grams, not in kilograms, in grams. We measure our quantity of lead and then we divide it by what that atomic mass is.*0508

*Whatever number we get in the end, weâ€™ve got the number of mols.*0517

*n equals m over m is the number of mols. In each mol there are many, many, many molecules.*0523

*Specifically the number is 6.022 x 10^23 objects per mol.*0530

*If youâ€™re doing it with molecules and youâ€™ve got 1 mol of molecules. Then what youâ€™ve got is 6.022 x 10^23 many molecules.*0537

*Thatâ€™s a whole lot of molecules. This number is called Avogadro's number because he did pioneering work in figuring out quantities.*0546

*He wasnâ€™t actually the person to figure precisely this number but he did a lot of work in figuring out how much of a substance is there and how it connects to other things.*0554

*Now weâ€™re ready to get back to the idea of expanding a gas. Weâ€™re finally ready to relate gas, temperature, and the number of mols, and all these sorts of things.*0563

*We do this with the ideal gas law, so named because it models an ideal gas. There isnâ€™t such a thing as an actual ideal gas.*0570

*Itâ€™s just a theoretical gas that we use to create a useful formula. It does allow us to really closely model real world gases.*0578

*Itâ€™s not absolutely perfect but for our purposes itâ€™s going to be well within .1% or .01% of what weâ€™re going to have if not even better.*0587

*Itâ€™s going to do great for our problems, but if we were trying to do something really, really careful weâ€™d have to come up with a new way to model it.*0593

*Weâ€™d need more data, but for our purposes itâ€™s really great and itâ€™s a great way for being able to get a close estimation of whatâ€™s going to be going on.*0601

*Now we need to figure out how to read this. This is a lot of letters.*0608

*P is the pressure of the gas. Note that this absolute pressure, not gauge pressure. If we had air in a tire and we wanted to see what the pressure on that was, we wouldnâ€™t just be able to take a measure on the tire using a gauge.*0612

*Weâ€™d have to figure out whatâ€™s the pressure in that tire but then also add what local air pressure is. Weâ€™d have to use the absolute pressure.*0627

*Next up v, is the volume of the gas. Whatever size container it is. Expanding on that tire idea, if would be the volume inside of that tire, how much space the gas is filling out.*0634

*N is the number of mols of the gas that we have to figure out by knowing what the mass of our quantity is. Youâ€™d have to figure out some way to measure the amount of gas youâ€™ve got.*0645

*If you know how many mols youâ€™ve got youâ€™re ready to keep going. R is just a single number, itâ€™s the gas constant and r is equal to 8.314 joules per mol x kelvin.*0655

*Interesting thing to note, that also means that the left and the right side wind up equaling joules in the end. Because weâ€™ve got mols x kelvin, so n and t are going to cancel out the mol and kelvin.*0666

*So weâ€™re only going to be left with joules, so that means that pressure times volume is actually a measure of the energy in the system.*0677

*The number of molecules youâ€™ve got times the temperature times the special constant is also a measure of how much energy in the system.*0685

*Which makes sense, a really, really pressurized container has a lot more energy in it than a container that has almost no pressure in it.*0692

*If youâ€™ve got a balloon, itâ€™s not going to do much if itâ€™s completely deflated and you poke a pin in it. But if youâ€™ve got a fully inflated balloon and you poke a pin in it somethingâ€™s going to happen.*0700

*Thatâ€™s a display of the energy occurring. Not of the energy occurring, I should rephrase that as you seeing how much energy is in that. The energy is already there but youâ€™re now causing it to change in other forms.*0708

*T is the temperature in kelvin of the gas. Remember weâ€™ve got to have this kelvin otherwise it isnâ€™t going to work.*0720

*We put all those things together and weâ€™ve got this really useful equation for being able to connect how much the gas will expand and how much the gas will push in on the walls of its container with the volume and the pressure and the number of molecules there are in the special gas constant.*0726

*One special note on water. Water is really special. Water is maybe almost unique. It might actually be fully unique. It has many, many special properties.*0742

*Some of those properties are shared with other things but as far as an object that has all of those properties in it. One substance that is all of those properties, itâ€™s really amazing. I donâ€™t know of anything else that has as many extremely unusual properties.*0753

*Water has a number of these unusual properties and if youâ€™re interested just take a quick internet search on special properties of water or waters properties.*0768

*Youâ€™ll find that thereâ€™s a whole bunch of these things and each one of them is incredibly important to the way our world works.*0778

*Life wouldnâ€™t be able to exist without pretty much any of these.*0784

*First off we already its amazingly high specific heat, previously water has one of the highest specific heats out there.*0787

*Another thing thatâ€™s really strange about it is the fact ice floats in water. You probably havenâ€™t thought about this too much because weâ€™re used to it.*0794

*Ice has always floated for our lives so we sort of take it for granted. Everything that weâ€™ve learned so far has been the opposite direction.*0801

*Weâ€™ve discussed that every time we have a hot object and you make it hotter it causes it to expand.*0810

*If you make it colder you cause it to become denser. So a cold object shrinks in is volume while retaining the same mass.*0815

*That means the colder you make an object the denser you make an object. If you make an object denser, wouldnâ€™t that mean the solid form of it would always sink in the liquid form of it?*0822

*That is true for most substances, if we did this with a brick of iron and dropped it into a molten container of iron that brick would fall to the bottom before eventually melted by that heated self.*0833

*For water near the freezing point, at aroundâ€¦I think precisely 4 degrees centigradeâ€¦Celsius not centigrade. Celsius, they changed the name a while ago.*0843

*At 4 degrees Celsius it actually stops contracting and expands to create the crystalline structure we know as ice.*0851

*At a certain point it begins to line up into ice. Before that it becomes very, very dense. Once itâ€™s at 4 degrees Celsius. But after that point, it starts to get prepared for its transition into ice.*0859

*Ice is a really specially arranged crystalline structure. And that crystalline structure causes it to have more space in between the molecules than the liquid form does.*0871

*Since itâ€™s got that more space in its structure itâ€™s going to be less dense than the water and itâ€™s going to actually wind up floating.*0880

*This is really, really cool and itâ€™s actually one of the things that allows life to exist on Earth.*0885

*Its possible life would still be able to exist without it but it certainly makes it a lot easier for complex life forms to exist.*0892

*If it were otherwise, if water were to get really dense when it was frozen then that would mean the coldest part of the water would be on the bottom.*0897

*That means if you had a lake it would wind up freezing from the bottom up. If it froze from the bottom up that would mean everything in that lake would die.*0907

*Because it would freeze from the bottom up to the top, youâ€™d have a fully solid lake and fish in there, in plants in there would just wind up dying off.*0917

*That means that you wind up killing off a huge amount of your aquatic life. Instead the way things occur now ice rises to the top.*0924

*At the top it winds up actually providing an insulating layer from the cold exterior.*0933

*Because weâ€™ve got that nice ice on top the fish are able to go down a lower level and theyâ€™re able to survive for the winter.*0938

*Theyâ€™re able to survive this thing that would otherwise cause all the water to freeze up and kill them off.*0945

*So because of the fact that ice floats itâ€™s one more reason we can have life on Earth. Itâ€™s really cool.*0950

*Now weâ€™re ready to switch gears and weâ€™re ready to talk about change of phase.*0957

*So far weâ€™ve talked about expanding within a phase but we havenâ€™t talked about how weâ€™re going to be able to jump from being a solid to a liquid or a liquid to a gas.*0960

*We want to talk aboutâ€¦so this idea is substances are held together by inner molecule forces. We enough latent energy, enough temperature, the molecules start to bounce around more and more.*0968

*These inner molecular forces that hold them together can actually be overcome by these being energetic enough to just pop out.*0977

*If weâ€™re in a solid, weâ€™re in this structure where their fairly rigidly head together. Eventually weâ€™re able to put enough energy in there for instead of being rigidly held together theyâ€™ll sort of turn into a slush and theyâ€™ll be able to slide on one another.*0984

*If we put in even more energy theyâ€™ll be able to jump out of the slush and fly around. Theyâ€™ll be able to just fly around whatever container theyâ€™re in.*0995

*If itâ€™s on Earth theyâ€™ll just be able to fly through the atmosphere. Youâ€™re able to jump out of the liquid with enough energy.*1004

*As we manage to switch from one phase to the next, weâ€™re clearly going to get some different properties.*1010

*Solids are different than liquids are different than gases. As more and more heat is added to a substance it changes phase.*1014

*Starting at a solid and applying heat, it will first melt into a liquid and then it will vaporize into a gas.*1021

*Thatâ€™s how we switch forward with more and more energy. If we do the reverse and pull heat energy out, if we cool the substance the process reverses.*1028

*We start at gas and then it will condense into a liquid and then it freezes into a solid. We first condense into a liquid, it condenses into a liquid and then gas will freeze into a solid. It freezes into a solid.*1038

*Inner molecular attraction is not the only force holding a substance together. We also have to account for pressure.*1053

*If weâ€™ve got inner molecular force holding it in, pressure is doing the exact same thing from a different point of view.*1059

*Its just pushing down. If itâ€™s pushing from all sides, itâ€™s going to help keep whatever it is, itâ€™s going to help keep it together. Itâ€™s going to pushing it together all the time.*1066

*If a substance is immersed in a fluid like our atmosphere the pressure of that fluid is going to keep pushing on the substance and it will back up those inner molecular forces and will help hold the substance together against rising temperatures.*1074

*While that temperature might be able to defeat the inner molecular force on it, it might not also be able defeat, defeat being sort of an odd word to use here, but it wonâ€™t be able to stronger than the force of the pressure and the inner molecular forces.*1088

*It might be strong enough to overcome one of them but not necessarily both. This means that the phase of substance is determined not by just temperature or pressure; itâ€™s determined by the combination of them.*1103

*Temperature and pressure. If we want to understand how a substance is going to behave with temperature and pressure weâ€™re going to have to look at both of those together.*1112

*The specific change over points will vary from substance to substance and to be able to show any given substance we make a phase diagram.*1123

*A phase diagram will look something like this picture right here. As we have higher and higher temperatures we become things likes gases and liquids.*1129

*At low temperatures and high pressure, its stays solid but if we drop the pressure, we could become a liquid at the same temperature or even a gas at the same temperature.*1139

*Notice how easy it is with very low pressures to be able make that switch over from solid to gas. At low pressures itâ€™s easy for the thing to break apart.*1148

*At higher and higher pressures it takes more and more thermal energy.*1158

*Itâ€™s possible for a solid to transform directly into a gas. If we had a really low pressure we could hop over by just increasing the temperature without ever having to touch liquid.*1163

*This is a process called sublimation. Youâ€™ve probably seen it if youâ€™ve ever played with dry ice or seen dry ice before.*1174

*It manages to jump directly from being a solid hunk of dry ice into being carbon dioxide, Iâ€™m pretty sure its carbon dioxide, but if youâ€™re doing an experiment with it you might want to double check.*1180

*I should have looked this up beforehand. Anyway, dry ice is able to sublimate directly from its solid from to its gas form.*1192

*Thereâ€™s also another special thing to talk about. Right here is the triple point. This is a special point thatâ€™s going to occur on each phase diagram at different locations.*1199

*Thatâ€™s going to be a unique state where all three forms can exist at once. All three phases will be able to simultaneously exist. You could have solid next to liquid next to gas.*1208

*Which is a really amazing thing. You couldnâ€™t really imagine something thatâ€™s able to be same temperature and have steam and ice and water all floating together happily coexisting.*1218

*Thatâ€™s a really, really hard thing to achieve because we have to be at just the right pressure and just the right temperature but it is possible for any substance.*1230

*Now getting from one phase to the next isnâ€™t just as simple stepping over a line. For a given mass to be able to change phase it has to overcome its heat of transformation.*1239

*What this means is that to be able to jump from being a solid to a liquid you donâ€™t have to just hitâ€¦for water for example we donâ€™t just get to 99 degrees and then 100 degrees and then 101 degrees and then it changes from water, water, gas.*1249

*Water, water, steam. It doesnâ€™t work like that, instead we get 99 degrees centigrade, 100 degrees centigrade, and then we have to put in a whole bunch more energy before weâ€™re able to get it to jump up to the steam level.*1265

*Thereâ€™s a big difference between managing to get up to the line and actually crossing the line on that phase diagram.*1275

*This is called the heat of transformation. Itâ€™s going to vary depending on the mass of the object. More mass means itâ€™ll take more energy to get to jump that line.*1283

*The amount of energy we take is heat is equal to l x m. Where l is going to be proportionately constant that will vary from substance to substance and what kind of transformation it is.*1293

*If itâ€™s a solid to a liquid or a liquid gas transformation, itâ€™s going to be different for even the same substance.*1304

*Weâ€™ll have to look up the specific substance weâ€™re talking about and what kind of transformation, but whatever the l is we could figure it out or look it up in a table.*1309

*If a substance is moving to a higher energy phase like solid to liquid to gas it has to take in q from its environment.*1318

*If on the other hand itâ€™s going to lower energy phase like gas to liquid to solid it actually releases the energy.*1324

*When water becomes ice it actually puts out energy into the environment around, which makes a lot of sense because thatâ€™s why we have to put it in a freezer, weâ€™re having the environment constantly pump the heat away from that area.*1331

*Thatâ€™s what the point of a refrigerator is. Weâ€™ve got a heat pump where it takes the heat inside of the box and it puts it somewhere else.*1342

*Because itâ€™s putting all that heat somewhere else weâ€™ve got a lower environmental temperature which allows things to give off their own temperature and become things like ice for example.*1349

*Now weâ€™re ready to go on to some examples. First off being able to change the length of temperature.*1360

*If weâ€™ve got a brass pipe of initial length of 20 meters and its alpha, its coefficient for transformation is 18.7 x 10^-6 per kelvin and it has a temperature rise of 80 kelvins, what would the new length be?*1364

*Well weâ€™ve got that the change in the length is equal to the original length times alpha times the change in temperature. If we want to know what the change in length is we just toss each of those in.*1380

*Weâ€™ve got 20 meters times 18.7 x 10^-6 times 80 kelvins. We multiply those altogether and we get 0.03 meters. So it manages to gain a positive 0.03 meters.*1392

*If we want to know what the final length is, we add that to our original length and weâ€™ll get 20.03 meters is our final length.*1408

*Notice even with the changeover of 80 kelvin, a fairly large amount of temperature from my point of view. It manages to only grow .03; this is a really small amount.*1419

*The amount of changeover that weâ€™re going to get is really small compared to the temperature difference that we have to have here.*1430

*Weâ€™re either going to have to be talking about absolutely giant lengths or absolutely giant temperatures differences before weâ€™re really going to notice this.*1438

*This is why we donâ€™t notice it in our daily lives. Although if you wanted to have one experiment or actually a useful thing, if you ever have a stuck jar, one trick you can do is run the lid under really, really hot water.*1445

*Because metal has a higher coefficient of expansion than the glass so that means the metal on that lid will wind up become a little bit larger and so you can then grab it and twist off and make it a little bit easier to turn and take it off.*1456

*There of course be careful if youâ€™re going to do this, you are running it under hot water and you donâ€™t want to accidentally burn your hand when youâ€™re taking it off.*1469

*It will make it slightly easier because youâ€™ll be changing that friction because it will have less pressure holding it to the glass.*1475

*Letâ€™s talk about why volume has beta equals 3 alpha. Previously I talked a little briefly about the fact that beta isnâ€™t precisely equal to 3 alpha but itâ€™s really good, itâ€™s good enough for our purposes.*1480

*It will almost always be good enough. Letâ€™s try to figure out how another way, how we could figure out what beta should be.*1492

*Another way to get to beta. The way that weâ€™ll do this is weâ€™ll start off the cube where all the lengths will undergo linear expansion.*1500

*What would the new volume of this cube be? Letâ€™s say one of the lengths in our original thing was l. If l is what the original length is, l new, the new l would be equal to l plus the change in l.*1508

*Well we know what the change in l is; change in l is just the original length times alpha times the change in temperature.*1524

*Now itâ€™s going to make this problem a lot easier if we set change in temperature equal to 1.*1532

*Because that change in temperature is just going to wind up showing up throughout the entire problem and itâ€™s just going to be multiplicative fact that keeps stacking and so itâ€™s actually not going to be a problem.*1539

*We should do thisâ€¦if were being really, really rigorous weâ€™d want to not make it simpler on ourselves, but weâ€™ll still be able to see the same reasoning so itâ€™s okay in this case to change it just to 1.*1549

*Now weâ€™ve got at this point that itâ€™s going to be equal. New l is equal to l plus l alpha.*1558

*What was the old volume of our cube? Our old volume of our cube was equal to l times l times l. Which is equal to l cubed.*1566

*If we want to know what the new volume is, weâ€™ll thatâ€™s going to be v old plus whatever the change in the volume was.*1577

*Now we want to figure out a way to solve for change in volume. Also notice v old is just the same thing as l cubed.*1586

*So weâ€™ve got l cubed plus whatever the change in volume wind up being is the way to find out what v new is.*1592

*If thatâ€™s the case, whatâ€™s another way to figure out what v new is? We managed to apply that heat so all of our lengths turn into l new. So v news length, the new lengthâ€¦sorry the new volume just has to be based off of the new lengths.*1599

*The way we find volume is a cube is the side cubed. So l new cubed is equal to v new. Weâ€™ve got l new cubed equals l cubed plus change in v.*1613

*Well l new is the same thing as l plus change in l cube equals l cubed plus change in v.*1626

*Start working this out, so weâ€™ll have l plus change in l, we can do l plus change in l squared in our head so that becomes l squared...whoops.*1634

*L squared, what was changed in l, change in l was l alpha, that will make it easier to do. So l plus l alpha cubed, so l plus l alpha cubed. We take off one of those and weâ€™ve now got l plus l alpha times l plus l alpha squared.*1645

*If we do that in our head we get l squared plus 2 l squared alpha plus l squared alpha squared equals l cubed plus the change in v.*1664

*We multiply that out some more and weâ€™re going to get l times l squared l cubed plus 2 l cubed alpha plus l cubed alpha squared.*1675

*We also do l alpha plus l alpha times l squared becomes l cubed alpha plus 2 l cubed alpha squared plus l cubed alpha cubed equals l cubed plus change in v.*1686

*That this point we want to solve and figure out what is change in v in terms of those old lengths.*1700

*That will give us a way to connect alpha to the other stuff. Notice at this point weâ€™ve l cubed and l cubed show up on both sides.*1706

*One other thing, weâ€™ve got l cubed everywhere. L cubed is run amuck. So what is l cubed equal to? L cubed equal to the old volume.*1713

*Now weâ€™re just going to say thatâ€™s just going to be v. Weâ€™ll make that v on its own.*1722

*So weâ€™ve got v plus 2â€¦sorry letâ€™s simplify this as we go along.*1726

*Thereâ€™s 2 l cubed alpha plus l cubed alpha so weâ€™ve now got 3v alpha plus l cubed alpha squared. 2 l cubed alpha squared so weâ€™ve got 3v alpha squared plus l cubed alpha cubed on its own.*1732

*V alpha cubed equals l cubedâ€¦oops... make that v cubed as well, plus change in v.*1747

*If thatâ€™s the case, not v cubed. There we are, sorry. So weâ€™ve got a v and v on both sides, so we knock those out and what weâ€™ve really got is 3 v alpha plus 3 v alpha squared plus v alpha cubed equals change in v.*1758

*Well thatâ€™s totally different than the formula we had originally. Which was change in v equals v beta change in temperature, since weâ€™re just dealing with change in temperature is equal to 1; weâ€™ll make that v beta.*1780

*Since beta we were told was equal to 3 alpha, then weâ€™ve got 3 v alpha. Notice this is totally different than this whole long thing.*1797

*How is it we can get away with just using v alphaâ€¦just using alpha 3 alpha as opposed to 3 alpha plus 3 alpha squared plus 3 alpha cubed.*1807

*Why? Because alpha is tiny remember, alpha was somewhere between 10^-4 and 10^-6. If its 10^-4 a big alpha, 10^-4 squared is 10^-8.*1816

*10^-8 is almost certainly going to have no impact practically. Itâ€™s going to turn negligible.*1832

*This right here is going to be really negligible. And this right here is going to be super-duper negligible because of alpha cubed and alpha squared.*1838

*Alpha is practically negligible unless weâ€™re dealing with really big volumes or really big temperature differences. Thatâ€™s going to have almost no effect unless weâ€™re dealing with really giant things.*1846

*Alpha squared and alpha cubed, theyâ€™re so small theyâ€™re going to have almost no effect entirely.*1857

*Weâ€™re able to drop them and use the much simpler formula of beta equals 3 alpha.*1863

*If we were dealing with really, really, really, really giant numbers, absolutely huge numbers we might want to wind up including the 3 v alpha squared.*1869

*If there absolutely fantastic ginormous we might even decide to include that one as well.*1879

*For the most part itâ€™s plenty fine to just go with that. Itâ€™ll be enough information for us to be able to do a great job.*1885

*Weâ€™re able to set beta equal to 3 alpha and be able to have really good understanding of how itâ€™s working.*1893

*Now weâ€™re ready to try using that fancy ideal gas law. Whatâ€™s our ideal gas law?*1901

*If weâ€™ve got a gas comprised entirely of O2 with a mass of 1.43 grams and itâ€™s held in a 1 liter container at this pressure and a temperature of thisâ€¦okay great.*1907

*If we bring the temperature to a new temperature and we keep the volume fixed what will the pressure increase to?*1917

*What if we also doubled v while doing it? To do this weâ€™re going to need the ideal gas law.*1922

*Whatâ€™s the ideal gas law? Itâ€™s the pressure times the volume is equal to the number of mols times the gas constant times temperature.*1927

*What was the gas constant again? We go, we look it up, we get 8.314 joules per mol per kelvin.*1934

*To figure out what the number of mols we have is, weâ€™ll have to know that the atomic mass for oxygen. We go we look it up on our periodic table, we get 15.9994 is the mass of oxygen.*1946

*Remember weâ€™re not going to be dealing with oxygen, weâ€™re dealing with O2. Weâ€™re dealing with molecules of oxygen.*1962

*If the mass for oxygen is 15.9994 the mass for O2 is going to be double that and weâ€™re going to get 31.988 is what weâ€™re going to get for the mass of O2.*1968

*If thatâ€™s the case then our number of mols is the number grams we have of our gas, 1.43 grams divided by the molecular mass, 31.988 and that gives us n is equal to 0.0447 mols.*1985

*We also need to talk about whatâ€™s the temperature. If ti is equal to -.5 degrees Celsius, how do we convert from Celsius to kelvin?*2007

*Remember weâ€™re not allowed to use Celsius with temperature when weâ€™re dealing with ideal gas law.*2020

*We can talk about it when weâ€™re just talking about change in tempreture because Celsius and kelvin have the same change size but they have totally different absolute values.*2026

*If weâ€™re talking about what the full value of it is weâ€™re going to have to switch over to kelvin because the ideal gas law its defiantly using the full value.*2036

*It needs t, not change in t. So how do we convert over? Temperature in Celsius is equal to the temperature in kelvin minus 273.15.*2042

*If we want to know what the initial temperature is over here, temperature initial, we can switch it over by adding 273.15 and so we get 272.62 kelvin.*2054

*What if we want to know what t final is? T final, once again, we had 273.15 and weâ€™re going to get 313.15 kelvin.*2065

*Interesting thing to note, we didnâ€™t actually have to convert ti. In fact as far as this problems concerned we didnâ€™t ever have to know ti because this formula right here, it doesnâ€™t concern itself with the difference.*2078

*It only concerns itself with the ending value is. If we had to figure out something from the beginning we would have needed to know what that starting value was, but we didnâ€™t.*2090

*Everything was given to us, so in the end we actually donâ€™t need to know it because itâ€™s already set what itâ€™s going to wind up being, what itâ€™s going to wind up ending at.*2096

*At this point weâ€™ve got everything figured out so we can start plugging things in. The equation p v equals n r t.*2105

*We do the first part of the problem first. Whatâ€™s the pressure that weâ€™re at? We donâ€™t know what the pressure is, weâ€™re solving for pressure.*2113

*Whatâ€™s the volume that weâ€™re at? Weâ€™re in a 1 liter containerâ€¦oh whoops, thatâ€™s one more thing we have to solve for.*2119

*What is 1 liter as a volume? Volume equals 1 liter, weâ€™re not allowed to use liters. We donâ€™t use liters for this, we use cubic meters.*2125

*One thing weâ€¦Iâ€™m not sure if you know this already, if weâ€™ve already talked about this. 1 literâ€¦well whatâ€™s 1 milliliter? 1 milliliter is the same thing as 1 cubic centimeter.*2136

*If 1 milliliter is equal to 1 cubic centimeter then 1 liter would a thousand of those. So 10 x10 x 10. So 1 liter is the same thing as .1 meter cubed.*2147

*If its .1 meter cubed then weâ€™ve got 0.001 cubic meters is our volume.*2163

*So we plug that in and we got pressure times 0.001 cubic meters, remember we canâ€™t use liters for this we have to do it in cubic meters because thatâ€™s how everythingâ€™s been built.*2172

*Thatâ€™s what Pascal is based on. Then we plug in the number of mols weâ€™ve got, 0.0447 mols times the gas constant, 8.314 times the temperature that we end at 313.15.*2184

*We solve for what the pressure is using a calculator and we get that the pressure wind up being 116,378 Pascals. If we want it to be something a little bit more hand able, thatâ€™s approximately same thing as 116.4 Kilopascals.*2201

*For the second part of this problem, weâ€™re just going to need to also change the volume. So the new volume itâ€™s going to change to is double its original amount, so itâ€™s going to be pressure times 0.002 cubic meters, because itâ€™s doubling to 2 liters now.*2219

*Is equal to exact same stuff for everything else; weâ€™ve got the same number of mols, same gas constant, same ending temperature.*2234

*We solve that out for our pressure and get 58,189 Pascals, which is equal to something a little bit more sensible, weâ€™ll talk about it in Kilopascals.*2247

*Notice changing that volume, since itâ€™s got double the space to bounce around in, it actually winds up being half the amount of pressure.*2264

*Since they bounce, since theyâ€™ve got double the space to bounce around in, youâ€™ve got half the number of bounces occurring on average. So with half the number of bounces occurring on average, youâ€™re going to have half the pressure.*2273

*Weâ€™re ready to do our final example. If weâ€™ve got 2 liters of water on a stove thatâ€™s currently at 20 degrees Celsius, how much heat energy cubed do we have to put in that water to bring it to boil?*2284

*How much more heat energy will we have to put in to boil off all the water?*2296

*First thing to notice, we donâ€™t have liters as mass. Weâ€™ve just got 2 liters of water.*2299

*If weâ€™re dealing with standard room temperature water and standard pressure, which we are reasonably thing to assume since weâ€™re dealing with a stove.*2304

*We can convert that since 1 milliliter of waterâ€¦sorry 1 milliliter of water, standard atmosphere and pressure is the same thing as 1 gram of water.*2311

*Then a liter of water is the same thing as 1 kilogram. So a liter is a kilogram of water.*2323

*If a liter is equal to a kilogram then 2 liters is equal toâ€¦well theyâ€™re notâ€¦liters not equal to kilogram, but liter goes to kilogram when itâ€™s in terms of water.*2329

*So 2 liters goes to 2 kilograms. Weâ€™ve got a mass of 2 kilograms of water, which weâ€™re going to need to use to be able to do any of this.*2340

*Also whatâ€™s the specific heat for water? Specific heat for water is equal to 1 calorie per gram per kelvin.*2349

*If its 1 calorie per gram per kelvin, well thatâ€™s the same thing as 4.1868 joules per gram per kelvin.*2361

*So 4.1868 joules per gram per kelvin, but if we want to do that we can also up convert that to kilograms, 4.1868 kilojoules per kilograms. Kilo both on the top and bottom.*2369

*Now weâ€™ve got thatâ€™s what our specific heat is. Thatâ€™s how much energy it takes in to be able to raise it 1 degree.*2388

*If we need to get from 20 degrees Celsius to 100 degrees Celsius, whatâ€™s our change have to be?*2395

*Our change in temperature is going to be equal to 80 kelvin. Since a kelvin and a Celsius are the same thing.*2401

*Weâ€™re going to start boiling once we hit 100 Celsius, but it will take a lot more energy, because we have to then push over. We have to push over all of that extra energy to be able to actually get over that line.*2406

*To be able to get all of our liquid over the line and into the gas phase. Weâ€™re going to need even more energy on top of just getting it to 100 Celsius.*2419

*Change in temperature equals 80 kelvin. Our formula is the amount of energy that we have to put in to get a given temperature increase for a given substance is the specific heat of that times the mass weâ€™re dealing with times the change in temperature.*2428

*Our specific heat is 4.1868 kilojoules per kilogram, so its 4.1868 times 10^3 since weâ€™re dealing with kilojoules, times the mass weâ€™re dealing with is 2 kilograms, times the change in temperature, is 80 kelvin.*2446

*We hit that with a calculator and we get 669,888, way too many significant digits and so that becomes 670 kilojoules.*2465

*We need 670 kilojoules of energy to be able to move 2 liters of water from room temperature to a boiling temperature.*2476

*Thatâ€™s not enough energy to be able to get rid of all it. From there we know how to use the heat of transformation.*2485

*The heat of transformation to get from liquid into gas, the heat of vaporization for water is 2,257 kilojoules per kilogram.*2491

*If thatâ€™s how much it is weâ€™re going to use heat of transformation is equal to l our coefficient of transformation times the mass weâ€™re dealing with.*2502

*So l is 2,257 kilojoules, so kilo x 10^3 times 2 kilograms. We get 4,514,000,000 joules which is then the same thing as 4.154 mega joules of energy.*2510

*4.154 mega joules of energy, thatâ€™s more than 6.67 times energy. It takes way, way more energy to get it to actually boil off than it does to get it to the point of where it can just begin to boil.*2530

*As we add in a little bit of energy a little bit of the water will manage to boil off, but to actually boil off all 2 liters, it takes well more than 6x, almost 7x more energy.*2552

*Weâ€™re not even including the fact weâ€™re going to actually lose some of this heat energy. It doesnâ€™t all perfectly go into heating the water.*2563

*As itâ€™s a hotter temperature itâ€™s going to be radiating more heat greatly to the area around it.*2569

*Itâ€™s going to take probably even more than 6.67x energy to get that water to actually boil off.*2574

*Thatâ€™s a huge difference. Thatâ€™s the reason why you can bring water to a boil, toss in your spaghetti and come back and not have all the water gone.*2579

*Itâ€™s because itâ€™s actually going to take, if consuming a constant amount of heat going to that pot, itâ€™s actually going to take more than 6x the amount of time to get it to go from starting to boil then all the water gone.*2587

*If it takes you 10 minutes to bring a given amount of water to boil, you know youâ€™ve got at least an hour before all of that water will have wind up boiling off.*2603

*So itâ€™s a really interesting thing to think about and thatâ€™s specific heat of vaporization is also one of the things thatâ€™s so amazing about water. That high specific heat of vaporization means that we can things like sweat happen.*2611

*Where the amount of heat in our skin gets transferred into the water and since it has such a high vaporization heat, weâ€™re able to transfer lots of energy into it and have it get wicked away into the atmosphere.*2621

*So weâ€™re able to conveniently, usefully cool ourselves because of this high vaporization heat for water. One of the really cool things that water gives us.*2631

*Alright, hope you enjoyed that, hope it made a lot sense and weâ€™ll see you later. Bye.*2639

1 answer

Last reply by: Professor Selhorst-Jones

Mon Aug 26, 2013 11:06 PM

Post by enya zh on August 18, 2013

What about plasma?

3 answers

Last reply by: Professor Selhorst-Jones

Wed May 1, 2013 2:21 PM

Post by Abdulrahman Alhassawi on April 29, 2013

I have a question, in example 4 when you plugged in the numbers for the formula of Q=Lm, why did multiply the latent heat by 10^3 ? Isn't it already in kj?