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### Course: MCAT > Unit 10

Lesson 21: Thermodynamics- Thermodynamics questions
- Thermodynamics article
- Specific heat and latent heat of fusion and vaporization
- Zeroth law of thermodynamics
- First law of thermodynamics equation
- First law of thermodynamics problem solving
- PV diagrams - part 1: Work and isobaric processes
- PV diagrams - part 2: Isothermal, isometric, adiabatic processes
- Second law of thermodynamics

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# PV diagrams - part 2: Isothermal, isometric, adiabatic processes

There are three types of thermodynamic processes you should know: isothermal, isometric, and adiabatic. An isothermal process is all about keeping the temperature constant, while an isometric process maintains a constant volume. The trickiest of the three is the adiabatic process, where no heat is exchanged and changes in volume can alter both pressure and temperature. Created by David SantoPietro.

## Want to join the conversation?

- Why is an adiabat steeper than an isotherm??(24 votes)
- A short answer

In the case of an adiabatic process the molecules move faster (on average) than in the case of an isothermal process and thus the pressure is higher (steeper curve)....(18 votes)

- This guy is really good(8 votes)
- How does the pressure get decreased in Isothermal Expansion? I know that PV=Constant but I want to know what actually happen inside the system due to which internal energy remains constant and pressure get decreased .(2 votes)
- Gas pressure comes from the impact of gas molecules against the inner walls of the container. This pressure depends on the speed of the molecules and the number of impacts per square inch of the internal surface . The speed does not change because the temperature is constant, but the overall number of impacts decrease because the molecules have to travel longer before they hit the wall, and the number of impacts per sq inch also decreases because the internal surface is expanding. This causes the gas pressure to decrease.(11 votes)

- Why is the internal energy constant in case of an isothermal condition?

Why is delta-U equal to 0 for the same?

I don't seem to get it physically. I do get it mathematically.(3 votes)- 'U' for gases is mainly due to kinetic energy of the molecules nd we know that avg KE of a sample of gas purely depends on the temperature of the system . Since the temperature remains constant during an isothermal process , there should be no change in the avg KE of the sample, nd thus internal energy remains constant(3 votes)

- I want to know examples of adiabatic system in daily or some system look like this

Could you tell me?(2 votes)- Examples of adiabatic compression: (1) the compression of the air-gas mix in a car engine. (2) The shock wave at the nose of a supersonic aircraft.

Examples of adiabatic expansion: any explosion, from a firecracker to an atomic bomb.

The foregoing examples are adiabatic because they occur so fast that no heat is transferred into or away from the gas itself.(5 votes)

- i can't seem to find what im looking for im looking for isometric just isometric drawings and i can't find it?? Help MEE!(1 vote)
- 3:30-3:35what is a kelvin?(0 votes)
- Simply Kelvin is another form of measuring temperature like Celsius, it's just that Kelvin is the Absolute temperature ( more like standard way of measuring the temperature ) so for a simple relationship between Celsius and kelvin its, Kelvin = 273 + Celsius.(3 votes)

- how would you work out a ISOMETRIC grid, when a question gives you a question about figures.?? I NEED HELP /)_(\(1 vote)
- Can any when one tell what is happening on the molecular level during adiabatic process when the piston is suddenly moved up or down why the internal energy increases or decreases(1 vote)
- Does this apply to ideal and non-ideal gases?(1 vote)

## Video transcript

- All right, so last time we
talked about isobaric processes This time let's talk about
isothermal processes. Iso means constant, thermal,
this is short for temperature so this is a process where the
temperature remains constant. Or, in other words, T equals
a constant, which we could also write, if temperature
is constant, that means the change in the temperature, that means there is no
change in the temperature, so the change in the
temperature is just zero. Now, before we move on,
let me show you one more important thing. Remember, we said previously,
the internal energy of a gas is not equal to, but it's proportional to, the temperature of a gas. And so if the temperature doubles, the internal energy doubles. If the temperature doesn't change, the internal energy doesn't change. So for an isothermal
process, not only is ΔT=0, but more importantly, in terms of the First Law of Thermodynamics,
ΔU is also equal to 0. This is important, this is
something you have to know. For an isothermal process, ΔU is 0. Now you might be confused here. You might say, "Hold on a
minute, how can you have "a thermal process if there's
no thermal, if there's "no change in the temperature at all?" Well, you can, stuff's gonna happen here. This doesn't mean nothing happens. Things are gonna happen,
but they're gonna happen in such a way that there's
no change in the temperature and there's no change
in the internal energy, so what can we say? Well, let's look at the
First Law of Thermodynamics. The First Law holds, for
any thermal process in here, whether it's an isotherm,
an isobar, any of them, so we can say that ΔU has got to equal Q, which is the heat that flows into a gas, plus W, which is the work done on the gas, and now we know, for an isothermal
process the ΔU is just 0. So what does that mean? That means that Q + W have to add up to 0. So this means if you do,
say, 300 joules of work by pushing this down, you
do 300 joules of work. The only way the temperature's
gonna remain constant is for 300 joules of
heat to leave the gas, 300 joules of heat would have to leave. That would mean that Q
is -300 joules, that way 300 joules and -300 joules add up to 0, you've got an isothermal process. But it's not enough for
just the initial temperature to equal the final temperature. In order for this process
to be truly isothermal, the temperature has to remain
the same at every moment during the process. So every bit of energy
you add has to immediately get taken away, or every bit of energy you
take away has to immediately get added back in. There can't be a delay, otherwise you'd add this 300 joules, the temperature of the gas would increase, and then the heat would
conduct outta here, you know, at its leisure, it would take some time, and then finally you'd reach
the same temperature as before, that doesn't count. That's not an isothermal process. The gas has to be at the same
temperature at all moments. So how do you do this? Well, just make sure you
push down the piston, or if you're pulling it
up, you do so very slowly. That way, the heat always
has time to conduct out or in accordingly. If you make the process happen too fast, this heat, yanno it takes
some time for heat to conduct through a container, and if you make the
process happen too fast, this heat can't conduct
out of the container or into the container fast enough, so you've gotta make the
process happen very slow, add 1 joule per hour or per
day, make it as slow as possible so that this heat always has
time to conduct accordingly and maintain a constant temperature. Constant temperature with what? Well, just stick this whole
thing in a thermal reservoir, this is how you could actually do it. Put the whole container in a tank of water that has a temperature of, say, 290K, a huge tank of water. Water doesn't change its
temperature very easily since it has such a high specific heat, so if the tank is very large,
this water's gonna maintain the same temperature,
it's not gonna care about a little piston in here, but the gas in the piston
is gonna try to maintain equilibrium with temperature of the water. So if you make this
process happen very slow, if I push down the piston
very slow, I'll add energy, but that energy's gonna get
taken out, the temperature of the gas will remain the
same if I do it slow enough, or I can pull up on the piston
very slowly, then some heat has to enter into the gas
so that it always maintains the same temperature with
the outside environment, ensuring that it's an isothermal process. So what's an isothermal process
look like on a PV diagram? Well, let's look at the Ideal Gas Law. The Ideal Gas Law says that
P x V = NKT, at least the Boltzmann's Constant version of it does, so I want to know what the pressure is as a function of volume, let
me just solve for pressure. Pressure = NKT/V. Now lookit. N number of molecules
in here, that's a constant we're not letting any
gas molecules in or out. K, that's Boltzmann's Constant,
that number doesn't change. For an isothermal process,
temperature's also a constant. Everything up here in the
numerator's a constant, and we just have P, as a
function is constant/V, so P just goes like 1/x. It's like having a function
y = a constant over x, and we know what 1/x looks
like, it looks like that. So on a PV diagram, an
isothermal process is gonna look something like this,
it's gonna curve like 1/x and it can be an isothermal
expansion if volume increases or an isothermal compression
if volume decreases. So the actual shape of the
line drawn on a PV diagram for an isothermal process is sometimes called an isotherm and they look like that. Notice that we cannot find
the work done by just saying Work is PΔV. Remember, that's how we found
the work done by the gas in an isobaric process, but that was because we
had a nice rectangle. The area underneath this
graph is still gonna give us the work done, that's true. This definitely is the
work done by the gas, but it's not a perfect
rectangle so you can't use this formula, you'll have to know, you'll have to be given
the heat and then you can figure out the work or given the work, you'll find the heat. There's not a really good way, unless you're gonna do calculus, to figure out the area
underneath this curve. One more thing that you
should definitely know. Because the NKT is a constant,
right, all of this stuff is not changing for an isothermal process, that means P x V is also not changing. That's another thing that doesn't change. So T doesn't change, U, the internal energy, doesn't change, and P x V does not change as
well because T isn't changing over here in the Ideal Gas Law. That means, if you take the
pressure times the volume at any point along this isotherm,
you'll get the same number so this volume here and
this pressure right here, if I take those two and I
multiply those two together, I'll get some number, and if I take the final one,
this volume and this pressure, and I multiply those two numbers,
I'll get the same number. I'll get the same result for P x V. I'll get the same result
here, if I take these two, any P x V value along this
line is gonna be the same because that number can't
change, cause if it did that'd mean the temperature
had to be changing and then you wouldn't have an isotherm. So that's the isothermal process. That's one of the four most
common thermal processes. We've got two more to go. Let's talk about the isometric process. The first thing you should know
is this is sometimes called isochoric, and it's also
sometimes called isovolumetric. Why does it have three names? I don't know, but they
all mean the same thing. Iso means constant, volumetric and choric and metric
all refer to size or volume This means constant volume. How do you make sure that happens? Well, just don't let the piston move. The piston is the thing
that regulates the volume. Well, that thing's shut,
I dunno, keep that thing from moving and you'll have,
no matter what else happens, an isometric, isochoric,
or isovolumetric process, which all mean the same thing. Now, since the piston
can't move, that means no work can be done. The gas can't do any work, the outside forces can't do
any work, you can't do any work on the gas. No work can be done if
this piston cannot be moved up or down. So W's always going to
equal 0 for one of these isometric processes. That means if we write the First Law, the First Law of Thermodynamics
is true for every process, says that ΔU = Q, the
amount of heat that flows into or out of the gas, + W, except W is 0, so
we have no work done. This is 0 and our First
Law just becomes ΔU = Q or, in other words, for
an isometric process, the only way to change the
internal energy would be to add heat or to take heat away. So these isometric processes
are actually pretty simple. What do they look like on a PV diagram? Well, the volume is staying constant. Pressure staying constant
is a horizontal line, so volume staying constant
is a vertical line. And if I add heat, I'll
increase the pressure, and if I take heat away,
I'll decrease the pressure, and this volume will remain
the same, cause this piston is not allowed to move. Now remember that work is the
area underneath the curve. Does that make sense over here? How much area is underneath this curve? There's no area underneath this curve. There's no area, you've
just got this line here, that's not an area, that's
infinitesimally thin and so that means there's no area, no area means no work is done, and that agrees with what we
know about an isometric process All right, one more of the
big four processes to go. Let's talk about the adiabatic process. This is one in which no heat is exchanged, so sometimes people hear
that and they think, "Oh, that means that there's no change "in the temperature, right?" No, that is not right. This is definitely not what we're saying. No heat exchanged means that
Q, our letter that we use to represent the heat, is 0. It means that no heat
is allowed into the gas, no heat is allowed to flow out of the gas. These do not happen for
an adiabatic process. And that does not mean that
the temperature can't change. The temperature can change
here because the piston can do work or the work
can be done by the gas, but no heat can flow in or out. So you've gotta get good at delineating between the temperature and the heat. These are not the same thing. Temperature is kind of a
measure of how much energy a gas has at a given moment. Q, the heat, is how much
thermal energy is flowing into that gas or out of that gas. It doesn't represent how much
energy the gas actually has, it's how much thermal energy
you're adding or taking away. And for an adiabatic process, there is no thermal energy conducted in or out. What does that mean for the First Law? The First Law is true for every process, ΔU = Q + W, the work done on the gas, but for an adiabatic
process, there is no heat, so that just means ΔU equals
the work done on the gas, that's the only way you're
gonna add energy to the gas is by doing work on the gas or
allowing the gas to do work, then energy can be removed, but you can't add or take
away energy thermally, conductively, through the
walls of the container. It has to be done by the piston. So how do you do this? How do you make sure
no heat gets conducted? One thing you should do is insulate this so that the heat does not
easily conduct through the walls of this container, but that's not really good enough. You've gotta make sure
no heat is exchanged, so you take this piston
and you shove it down as fast as you can or you
lift it up as fast as you can. It's the opposite of
an isothermal process. There we wanted the process
to happen slow so that the heat always had
time to flow in or out. Here we want the process to happen so fast that the heat has no
time to flow in or out. That way, we ensure that
it's an adiabatic process and that Q is actually 0. So what does an adiabatic process
look like on a PV diagram? It looks kind of like
an isothermal process, it's just steeper. So this would be an adiabatic expansion, and these lines are
sometimes called adiabats, and if you have an adiabatic compression, it would look like that. If you compare that to
an isothermal process, say that started here, it would not get as far down. You can tell that that's
an isothermal process because it's not as steep. So those are the four most
common thermal processes you'll hear about when
talking about PV diagrams, and each of them had something
unique and special about them The isobaric process had constant pressure and you could find the
work easily because it was a nice rectangle, which
meant you could just do height times width to get
the work done by the gas. There's the isothermal process
where temperature is constant internal energy is constant, and the quantity P x V,
pressure times volume, is also constant. There's the isometric process,
also known as isochoric or isovolumetric, where
the change in volume is 0, which meant, remember, that
means no work can be done. The work was also 0 for
an isometric process. And then there's the adiabatic
process where no heat is allowed to flow into
or out of the system.