Inhaling and exhaling
Find out exactly why air goes in and out of the lungs. Rishi is a pediatric infectious disease physician and works at Khan Academy. Created by Rishi Desai.
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- at2:20it was mentioned that air pressure is measure in mmHg. Why is that unit used.(41 votes)
- mmHg is the unit of measure that barometers use. Barometers measure pressure using a long u-shape tube (generally glass). Mercury was usually used in the barometer, and the level of the mercury would rise or drop depending on the pressure on the mercury. Mercury is not used very often because of new discovers of it's toxicity. Water is now often used in the barometer.
If you would like to see a picture or get more info, here is a link:
- In the lungs what keeps air pressure from equlizing,(13 votes)
- At the end of exhalation the alveolar pressure within the lungs is equal to the atmospheric pressure (the pressure that the atmosphere exerts at the nose/mouth. When a person inhales, their diaphragm contracts along with their external intercostal muscles. The diaphragm decreases pressure in the thorax downwards, and the external intercostals move the ribcage up and out. Because of the close association of the parietal and visceral pleura which surrounds the lungs, and the small amount of pleural fluid which separates them, a decrease in pressure caused by muscular contraction is translated into a decrease in pressure in the alveoli. As we know from basic PV=nRT, all things the same, if pressure decreases then volume will increase. It is when the stimulation of the inspiratory muscles ceases that alveolar and atmospheric pressure begin to equalize again. Think about what would happen if the pleural sac were to rupture...(25 votes)
- Why on increasing the volume of the jar, pressure decreases(757 mmHg) and then again increases(again to 760 mmHg)?
I could not understand this properly.
Thank You!(7 votes)
- the jar is full of millions of molecules moving around, slamming into each other and into the wall of the jar
that slamming and hitting is pressure
if you increase the volume of the jar, you make more room inside the jar
that means the molecules have more room to move around and are less likely to slam into each other
and when a molecule slams into the wall, it will probably not have any molecules near by (because the bottom dropped of the jar dropped, so the walls actually became longer, but the number of molecules stayed the same, so now instead of a million molecules slamming all over a one foot high wall, they'll slam all over a 5 foot high wall, they're more spread out)
so less pressure
and then when you raise the floor the reverse happens(12 votes)
- Does diaphragm muscle start the process of breathing?
If we didn't have diaphragm or if it was injured could we still breathe?(8 votes)
- Injury in the diaphragm leads to a condition referred as Atelectosis. This reduces the ability of a person to inhale, because the outer and inner pressures become the same and he can't breathe.(9 votes)
- Just wondering, when a baby takes birth, does it have oxygen in the form of air in his body, or not?(4 votes)
- At birth babies don't have oxygen or air in their lungs as they have been supplied with nutrients (including oxygen) by the mother via placenta and umbilical cord. Upon birth the baby will take a large gasp like breath allowing the alveoli to inflate (due to the decreased surface tension from surfactant) the following breaths and crying will aid in more completely inflating all the alveoli(16 votes)
- Not really relative to the video itself, but...
Seeing as air is ~78% Nitrogen, ~21% Oxygen, ~0.9% Argon, ~0.04% Carbon Dioxide, and less than 0.002% (each) of: Neon, Helium, Krypton, Hydrogen and Xenon; wouldn't the probability of each molecule being a specific element be subject to said percentages?
eg: Using Rishi's example, with five molecules in a jar; wouldn't the odds for each molecule to be a specific element be: ~78% chance to be Nitrogen, ~21% chance to be Oxygen, etc.?(4 votes)
- Yes, actually. Those percentages are based on volume fractions, which are usually pretty close to the mole fractions for air at STP. If you picked five air molecules at random, you'd be most likely to have four N2 molecules and one O2 molecule.(9 votes)
- so why can humans hold their breath without pinching their nose (or at least slow down the process) or mouth?(5 votes)
- We can close our throat to stop anything going down (eg. why you can open your mouth underwater), and also just to close the windpipe the epiglottis (a small flap) can cover it.(4 votes)
- So, I understand that the diaphragm assists in pushing on the lungs in order to help with exhaling the air out of the lungs. Or is it really the lungs wanting to equalize pressure that make us breath in and out?(2 votes)
- The lungs work on a pressure system. When the diaphragm contracts, it flattens and increases the chest cavity causing the pressure in the chest cavity around the lungs to decrease, drawing in air. When the diaphragm relaxes, it relaxes into the bow-like shape, decreasing the size of the chest cavity, which increases the pressure around the lungs, forcing the air out.
Hope this helps!(10 votes)
- I don't understand how this works, because the lungs are not directly connected to the bronchi, bronchioles, or alveoli. So, the lungs are actually closed off from the trachea and opening, creating a closed jar. If the pressure in the lungs decreases, how does it cause a decrease in pressure in the alveoli, bronchioles, etc? Because the air is not entering the lungs, it is entering the bronchiole and alveoli.(3 votes)
- I'm not sure where you got the idea that "the lungs are not directly connected to the bronchi, bronchioles, or alveoli" — those are all components of the lungs!
Maybe it will help to think of the lungs as being like a hollow tree — the air comes in through the trunk (trachea) and follows the two major branches (primary bronchi) into smaller branches (secondary and then tertiary bronchi). These small branches then split into tiny
branches aka. twigs (bronchioles) that then connect to leaves (alveoli).
This wikipedia article may also be helpful:
Does that help?(6 votes)
- Can someone give me an idea of how much pressure an (or many) mmhg is/are?(3 votes)
- 1mm Hg (1 Torr) equals 1.3332 · 10^2 Pascal or 1.3332 · 10^−3 bar(5 votes)
If you could have a magical ability to actually see all the air molecules in the air, you might see something like this. It would be a lot more crowded, but you could imagine it might look like this. And let's say that you actually decide to do something a little interesting, and that is to take a jar and simply capture some of the air molecules in your jar. So I've got my jar here. And I'm actually going to put a little opening on my jar. So let's say there's a little opening there. And I take that opening, and I'm going to just make it kind of a stretched-out neck. So this is my stretched-out neck on my jar. And there's the opening to my jar. And on the other side, what I want to do is actually kind of compare what's going on inside of my jar to what's going on outside of the jar. So to make it fair, let me actually try to create a purple box-- kind of a dashed line around an equivalent volume. So this is going to be, basically, a similarly-sized part of the air. And of course, this dashed line is just to show you which part I'm talking about, because, of course, this is an imaginary line. But let's say we're comparing what's going on inside of my blue jar with what's going on inside of this purple dashed line. Now, we know that that purple dashed line is kind of capturing a certain amount of the air in the atmosphere. And that air is going to have molecules that are bouncing off of each other. Let's say something like this. And you've got a bunch of random collisions happening. And these collisions-- the more frequently the collisions are happening, the higher the pressure in the air. And in fact, measured pressure in the air is around 760 millimeters of mercury. So that's how we think about air pressure. So that's the pressure in the atmosphere. And if I was to measure my jar pressure, it would be, of course, the same thing. It would be 760 millimeters of mercury. And as a quick aside, just thinking about what these molecules are, if there are five of them, then you might say that this is nitrogen, this one is nitrogen, this one is nitrogen, this could be nitrogen, and this one might be oxygen. Because remember, oxygen is about 21% of air. And so that might be a fair estimation of what these five molecules could be-- mostly nitrogen. So in the air, we've got nitrogen and oxygen. It's bouncing around in my jar, just as it is in the atmosphere itself. And now let's say I decide to do kind of an interesting experiment. I decide to drop the floor-- just stay with me here-- I drop the floor of my jar. So I actually expand the bottom of my jar. For the moment, don't worry so much about how that could possibly happen. Let's just assume that I do creatively somehow kind of drop the floor. And now it looks a little bit lower. So the volume has gone up in my jar. And actually, simultaneously, I should mention-- I just want to mention here that this door, or opening, of my jar is closed at the moment. So my opening, I've put a lid on it. So that's closed, and my floor just got a little bit lower. So the volume has gone up. That's the big change, right? Actually, let me write that up here in the corner. I'm just going to erase some of these molecules to create some space. And the first thing I want to mention is that the volume has gone up in my jar. So all of the green stuff I write in the corner is going to be from the jar's perspective. If the volume goes up now-- if that's the case, then these molecules inside the jar, they're excited. They've got more room to kind of run around and play and not bump into each other. So if they're not bumping into each other as much-- because of course, they've got all this extra space down here-- then the pressure on the inside of the jar is going to go down, right? Because there are less collisions happening. So now we've got, let's say, a slight decrease. It went to 757. So a little bit less than what's on the outside. So because the volume went up, the pressure went down. And again, that's because you have fewer collisions. And the new pressure is 757, which is a positive number. But sometimes people refer to this as negative pressure, or a vacuum. And the reason they're saying that is because they're saying, well, relative to 760, relative to this number, 757 is 3 points lower. And so in that sense, it's negative. So if you actually want to compare them to each other, you'd say, well, 757 minus 760 is negative 3. And that would be a negative number. But for the time being, I'm just going to leave it in the numbers we have, which is 757. Now, let's say that I open this door. This opening is now open. If I open up this opening, what will happen? Well, we have all this extra space down here I circled, but I'm just going to remove this for the time being-- all this extra space. And molecules, of course, are being knocked around all the time. So these collisions are happening always. And some molecules are going to get knocked perfectly so that they actually move into the jar. Let's say it goes in like this. So you're going to get some molecules that go in. And in fact, you might have some molecules that get knocked right out. So it's going to happen constantly. But overall, what's going to be the net difference? Well, let's say I leave this and I walk away and do my own thing for a minute and come back. I'm going to notice that there are actually extra molecules on the inside of my jar, because there's more space, less crowding in my jar because of all that extra volume I created. So over time, there's going to be a few extra molecules in my jar. And maybe I got lucky, and this one's an oxygen molecule. So I've got extra molecules on the inside. And these molecules-- so actually, that would be, I guess, the next step, is that air molecules move in. And these molecules are now going to do what molecules do, which is kind of bounce off of each other. So they start bouncing off of each other. And all of a sudden, now you've got-- let's say this guy collides over here as well, and maybe there's some bouncing and this collides over here. So now you've got-- because you've got six molecules on the inside and the same volume, the pressure on the inside has gone up. So pressure has gone up on the inside of the jar, simply because there are more molecules in there now. So even though you had more volume initially, you've kind of filled it up with more molecules. So the pressure goes up, let's say to 760 millimeters of mercury. So now it's gone back up. So this is my new pressure. And this all happened-- this whole kind of series of events happened because I decided to move the floor. Now, what would happen if I decide to move it back? Let's say I decide to go back to the original floor size. And I get rid of this lower line, and I raise the floor back up. And so now it looks something like this. Well, now the volume-- this is kind of the new first step, what's going to happen. The volume has gone down. That's obvious, because I just moved the floor purposefully. And I've got six molecules in my jar. And they're thrashing around, bumping into each other. But they've got less space to do it in. So the pressure is going to go up because there are more collisions. They're bumping into each other more. So the pressure is going to go up. Pressure is going to go up now to, let's say, 763 millimeters of mercury. Because it was 760. And at this point, let's say this is closed up. And so the pressure on the inside is 763 millimeters of mercury. Let me erase this. And that's because, again, you have more molecules, but you reduced the volume. So then the pressure on the inside is actually now higher than the outside pressure. I mean, the outside pressure is always going to be around 760. And that's because the atmosphere is just enormous, right? So the movement of a few molecules this way or that way is really not going to change the amount of collisions that are happening in the atmosphere. That's always going to stay the same. And so if I was to open this up-- open this door up-- then some molecules, of course, are going to be bouncing around, bouncing around. And some of these things might kind of bounce out. So some molecules might kind of bounce out. And overall, again, on the whole, you're going to have more molecules bouncing out than bouncing in because you have more collisions happening on the inside. And, again, when I say more collisions, in your mind, I want you to think of higher pressure. So if there's higher pressure on the inside and more collisions happening on the inside, you're going to have more things bouncing off each other, and molecules are going to be sent outside. So the next step I could write in would be air molecules. Air molecules move out. So the final point is that if air molecules are moving out-- let's say just by random chance, this oxygen molecule happened to be the one that got sent away. So this one kind of got knocked out. Then you have-- let me try to erase all this to clear it up-- then you have five molecules, again, on the inside. And you have the same volume that we initially started out with. So the pressure on the inside goes back to what it was in the first place. The pressure falls to 760. And the reason that I say exactly 760 is because this process in step three will continue until the number of collisions on the inside and outside of the jar are equal. So this is kind of the process-- and actually, I forgot to mention. When we were back at 763, sometimes people call this positive pressure for the same reason they called it negative before. Because all they're doing is they're comparing 763 to atmospheric pressure, which is 760, and saying, wow, that's a plus 3. That's a little bit positive. And so when you compare things relatively, you use words like "positive" and "negative." But if you're using just the total number in kind of absolute terms, then you would stick to 757 or 763. Now, what does all of this has to do with us? What does a jar and an opening have to do with human beings? Well, let me just show you that by simply changing my drawing a little bit, you'll see what this has to do with us. Now, instead of having all the molecules inside the jar-- I know that you know that they're there-- I can actually erase all this. And maybe I can change the shape of this a little bit to help you see what this could be. So let's say I make that like this and start drawing in like that. I'm going to keep all of this kind of the same in terms of the way it looks. Maybe like that. And you can see now, instead of a jar, what I'm creating for you are a pair of lungs. So this is a pair of lungs, left and right. This'll be right and this'll be left. And it'll look something like this. And this one might go up like that around that cardiac notch, and go like this. And then we have, of course, the opening-- which, if instead of calling it an opening, I can call it a mouth, this would be my mouth. And I could erase the word "opening" completely. And I think you'll start seeing how this is basically what happens in our body. So our head represents the opening of this. And this could be the nose. And this could be the head-- kind of a flat head I've drawn here. But you get the idea, I think. So there's your nose and there's your ear. And basically, air is coming in the mouth and going into the lungs and back out of the lungs. And what we call this process is "inhalation." So when you increase the volume, we call this "inhaling." So if you've ever wondered exactly what happens when you inhale air, there it is. And when you close up the lungs and air molecules move out, we call that "exhaling." Actually, I should probably try to make it look the same. They're both equally important. So I'll draw them the same way. Exhaling. And now you can see how inhaling and exhaling happen. So with every breath, this is the process. You kind of subtly change the volume, and all of a sudden, the pressure changes. Air moves in and out.