Pssst... we made flashcards to help you review the content in this episode! Find them on the free Crash Course App! Download it here for Apple Devices: apple.co/3d4eyZo Download it here for Android Devices: bit.ly/2SrDulJ
We were watching this in class and the teacher pause it right after the "They almost never behave themselves," and she just looks at us and goes, "Can't imagine what that's like."
At 5:37 - decreasing the number of miles decreases the volume, but in the case of a balloon the pressure actually goes up because pressure is related to curvature (this is why it's hardest to blow up a balloon when you're starting it and then it gets easier).
The fact that this video is 5 years old and that im going to university now and still use these as an aid in studying physics goes a long way to show how well made and timeless these videos are, cheers for that
In a series of experiments with his friend, Richard Towneley, Power discovered the relationship between the pressure and volume of a gas that later became known as Boyle's law. This relationship was outlined in "Experimental Philosophy." However, many may argue nevertheless that Boyle, after discussing the theory with Towneley and reading a pre-publication manuscript of "Experimental Philosophy" cited the hypothesis as the sole work of Richard Towneley. Boyle's mention of the theory preceded the publication of "Experimental Philosophy" by one year, which, combined with Boyle's promotion of the idea and his significant status as an aristocratic scientist, ensured the theory would be known as "Boyle's Law." [5]
I love Crash Course! Just wondering... think maybe you could make them less crashy coursey? You know, pause for breath between words now and again. I would love to see these episode lengths go up to the 22-23 minute mark so that we can allow students to have more internal processing while the video is still playing in class. ( for example, show more experiments, maps, illustrations, practical demonstrations, real world applications). It doesn't have to be Thoughtbubble (I know your contract and collaborations with them are limited and specific), but just maybe some other way of illustrating and expounding on whatever the lesson of the day is. Just a thought. Wonderful work you and your brother do! Huge fan, keep it up!
That would be so much work and this is free education. I think this fast method is kinda cool, quick information with colors and little animations that compare things like the cation animation to help you remember if you're particularly interested you simply do your own research.
This is an excellent episode of CC. Great job Hank and all of the CC team. Took me months to get my head round this at degree level. Wishing I'd seen this sooner.
3:05ish is where he starts talking about the science :) You're welcome. Everything else is cool too, but when studying, it can be helpful to know exactly what you need to know
See, them doing a physics crashcourse is easier said then done. They would need to teach a bunch of advance math, which not many of the viewers actually have that mathematical background knowledge.
Richard smith Then why not do a mathematics course? I'm in AAT H (Advanced Algebra Trigonometry Honors), and I would love help on that subject. I currently have a C, so I actually need it.
Vixen TheFox i would also love a mathematics crash course, not that i'm in college but i find it incredibly interesting. the thing is that math is so incredibly broad i don't know how they would manage to do a "mathematics" crash course.
I love that can experiment, that's just amazing. Especially since, from what I understood, since the atom in the can slowed down so much the air outside the can just busted through. The very air you're feeling broke though metal because inside the metal was too calm.
You have no idea how much you have helped me! You helped me pass A&P, and now in Physics! You rock, and I love your teaching style. Thanks for really helping me out!!!
At my first job, I used a bead blaster to blast some aluminium. This involves a vacuum chamber with thick rubber gloves sticking into it. When I first started using it, I was very surprised at how easy it was to move my arms despite the thick rubber gloves. Before then, I 'knew' that air was there, and that it had mass, but experiencing lack of air really changed my perception of the stuff that always surrounds us!
Can you please make a Crash Course Physics playlist??? PLEASE! You guys explain everything so well, and physics is one of the most confusing things ever.
This is my first time watching a video on this channel but it was really helpful and enjoyable ! Subscribed ! I absolutely love his character and his way of teaching. ♡
"You can remember the Ideal Gas Equation because it looks like Pervnert." Don't remember what cheesy-ass science video that was from, but I busted up laughing when I saw that.
something I never quite understood: If we imagine a closed container filled with 1 mol of a molecular gas and these molecules then split into 2 smaller molecules each, thus raising the number of gas particles from 1 to 2 moles - the ideal gas equation would suggest that the pressure of the whole system would increase. However: if we look at a single molecule it seems that the temperature must drop. One heavy molecule at speed x produces two lighter molecules which - due to conservation of momentum - should still have the same speed. but since their mass drops the average kinetic energy per particle (and thus temperature) should drop considerably. Also: while it is true that we do have more collisions at the same time due to the increased number of particles, the particles also got lighter by that amount. Is the solution simply that (excluding energy given to or taken out of the system due to the endothermic/exothermic nature of the reaction itself) temperature will drop and pressure stays constant?
Who want's to know where the ideal gas law comes from? A gas exerts pressure on the walls of a contain er due to the collisions of the gas molecules with the walls. We start with a single molecule or atom of mass, m, moving backwards and forwards with a velocity, V=(Vx,Vy,Vz) between two walls separated by a distance, L. Every time the molecule hits the wall it bounces back, reversing the x-component of its momentum. Its momentum P=(Px,Py,Pz) therefore changes by: ΔPx=−2mVx The time between two collisions with the same wall is how long it takes to traverse the box twice and get back to the same wall: Δt=2L/Vx Using Newton’s second law, the force by the molecule acting on the wall is: Fx=−ΔPx/Δt=2mVx/(2L/Vx)=m(Vx)^2/L To get the overall gas pressure P on one wall, we need to sum together the contributions due to N molecules in a cubic container of side, L, and take account of the fact that molecules move with varying speeds by taking an average value for (Vx)^2: P=Force/Area =ΣFxL2=Nm/L^3 =Nm/V where we have replaced L^3 with V, the volume of the gas. In practice we don’t measure or consider the average velocity in one specific direction, but only the average speed in any direction (Vrms=√ is the average or root-mean-square (rms) speed of the molecules). These are related in a simple way Vrms^2 = ++ and since there is no preferred direction Vrms^2=3=3=3 hence finally we get P=NmVrms^2/3V from which we see clearly that the pressure is determined directly by the random kinetic energy of the gas molecules. If we rearrange this trivially to read: PV = 2N/3×mVrms^2/2 we begin to see how the ideal gas law arises - we have already got PV on the left hand side and we have something proportional to the average kinetic energy on the right hand side. If we compare the ideal gas law: PV =NkT to the expression we have just derived we see the direct relation between the temperature and the average kinetic energy (1/2)mVrms^2 per molecules of a gas. The average Kinetic Energy, , of a gas molecule is: =(1/2)mVrms^2=(3/2)kT Therefore: PV = (2/3)N x (3/2)kT PV = NkT = nRT
You know, I would probably find chemistry really interesting if college did not force me to learn it and use my future career and thousands of dollars in tuition as what felt like a hostage.
This was a nice recap of my school material. I thought I've forgotten it already since I study Architecture at my university, but no I remember quite a bit. And thanks to shows like this will not be able to forget at all. ;)
Yeah, I know about that part. I was actually talking about the way it's presented and where in the syllabus. It doesn't really "fit" where it's put because it's like a blob of Physics in a Chemistry class. But I think that's because we try to teach the sciences as if they were discrete subjects and fail to make the necessary connections between them.
Indeed there is; it's more an issue for what the symbol means. For example, if I say P V = n k_{b} T, and you tried substituting in the number of moles for 'n', you'd quickly find that your answer is off by two dozen orders of magnitude. I guess the cause of confusion becomes apparent when you work in physical chemistry (or chemical physics), when you have physicists to deal (k_{b} as your constant) and chemists (R as the constant). Inconsistent notation is confusing!
Fun fact! Scientist have not been able to reach 0 kelvin, they believe it may not be achievable as they believe it is really difficult to make a particle not move at all. Lowest temperature reached is around 1 kelvin.
A lot of the reason why any organism fails to function at high temperature is that high temperatures make proteins denature (meaning they lose their shape and stop working). Human proteins are very sensitive, because we're used to a constant internal temperature; some bacteria have extremely heat-tolerant proteins, but if you keep raising the temperature, eventually everything will die. :)
I really want to thank you. My science teacher is horrible and can't explain anything at all. I have learned nothing all year but somehow managed to get good test scores (mostly by guessing). I am going to be in a much harder class next year because according to my scores, I have learned more than the rest of his students. This channel has really helped me understand at least the basic facts
Air pressure outside the container increases. Pressurised aircraft do not maintain a sea level pressure - it's more like 3000m altitude pressure IIRC. The amount of gas inside your water bottle doesn't change, neither does the temperature (greatly), or the ideal gas constant. So as the pressure outside the bottle increases, and as your water bottle is a pretty poor pressure vessel, the pressure inside also has to increase, which means the volume drops - it deflates.
depends if you are adding or subtracting material (ie gas) from the volume. Otherwise (in a closed system) it stays the same. Good test is pumping up a tire. pressure, volume, and mol change. Calculate the change in Temperature.
In all my time in school and university, we never used kilopascals, but rather hectopascals (1 hPa = 100 Pa) or just pascals. It's also the unit barometers use, next to bars or millibars.
Some one who knows things on RUclips? I never thought I would see the day. I salute you sir. We must spread our knowledge to everyone. The world is collapsing into idiocy...
>"I personally hate the fact we have multiple units for the same measurement" I agree. In the manual of all motorcycles* I ever had, the tire pressure is in Pa. But on all the gauges at all gas stations** I have been to, the scale is in bar, and often also psi. *Japanese **German I should take my label maker and stick "1bar=100kPa" on gauges at gas stations for the people who didn't google it yet. ^^
I believe it's because chemistry likes to deal with changes. Whether that be a chemical change or just a physical change. I've had the ideal gas law in all of my physics and chemistry courses though. The part of the law that deals with work is more towards physics.
That can being crushed was really surprising. I was totally expecting the crushing action to take place over the course of 30 seconds or so, not on the order of milliseconds!
Pssst... we made flashcards to help you review the content in this episode! Find them on the free Crash Course App!
Download it here for Apple Devices: apple.co/3d4eyZo
Download it here for Android Devices: bit.ly/2SrDulJ
I hope we can have a Mac version too, that will be really helpful as well, but I will try it out on my phone!
A chemist froze himself at-273C. Everyone said he was crazy. But he was 0K
+Lane Messier Nice. c:
I'm sorry to ruin your joke but -273C isn't 0K
+Stop throwing fridges at me
Ice crame is best tasty on that temperatour :-D
Stop throwing fridges at me Are you sure? I thought that you added 273 to a Celsius measurement to get the Kelvin measurement.
It's actually -273.15C
We were watching this in class and the teacher pause it right after the "They almost never behave themselves," and she just looks at us and goes, "Can't imagine what that's like."
+alexiane250 Throwin shade
+alexiane250 LOL. That's perfect.
Us teachers are savage
alexiane250 omg xD
you have a great teacher
At 5:37 - decreasing the number of miles decreases the volume, but in the case of a balloon the pressure actually goes up because pressure is related to curvature (this is why it's hardest to blow up a balloon when you're starting it and then it gets easier).
The fact that this video is 5 years old and that im going to university now and still use these as an aid in studying physics goes a long way to show how well made and timeless these videos are, cheers for that
If I had a dollar for every time I had a test tomorrow and Crash Course saved my butt ...
TobyKid Major
I would be richer than Bill Gates
I’d be the owner of every cent in earth
On
I'd be eating pancakes by then
PV=nRT, or as I remember it, "PerVneRT".
You sir, are a genius.
I'd just like to say that I used this in my physics exam over xmas & got an A. Thank you.
Combat King 0 yea that what my teacher said
I love that equation...now i use it as an ammunition and shell the warmists XD
Shell the warmists? Are you really on this channel and against climate change?
Animations are done by us - Thought Café :)
Hank: DO YOU FEEL IT? ARE YOU DOING THIS?!
Me: I'M DOING IT! :D
On Henry Power's wiki page, it says:
"Written by Hank Green, saviour of impoverished high school children."
Well played, Hank.
hmm I don't see it
0:19 *waving my arms around*
mom: *walks in*
me:
mom:
me:
mom:
me: science *continues flapping*
mom: *walks away*
Regan Reynolds omg LoL 😂😂😂😂🤣🤣🤣🤣
@@pattys.6799 sem
This is the content I subscribe for
legit me right before i read this
😂😂😂😂
Anyone else struggling in Chem rn lmao
Me!!! I have a test tomorrow and I'm not sleeping tonight.
+Cameron Joseph Yep
I am because I have a year of work to catch up on + do another year at the same time all in six months.
Lucy Hunt Good Luck to you!
yup. watching this video the night before my final just trying g to understand lol
I did shake my hands around. And I did feel it
Me too! Haha.
The funny thing is I would do that when I was younger but I nor anyone else knew what I was doing
I'm really feeling it.
u feelin it now mr.krabbs?
😂 Idiots
Did anyone else wave their hands around when Hank did? XD
I did
Me too..!!
I did lol!
LOL! I did
You all are weird
ppl here in 2024 🙌
In eight years of chemistry I have never seen the can experiment, and that made me really happy to see something so simple but so new to me
Exams got me watching 46 crash course chemistry vids after finishing all of world history and economics.
life got me learning 24/7 regardless of it being the schoolyear or not faster than you study for exams
2:58 *immediately opens wikipedia and checks*
In a series of experiments with his friend, Richard Towneley, Power discovered the relationship between the pressure and volume of a gas that later became known as Boyle's law. This relationship was outlined in "Experimental Philosophy." However, many may argue nevertheless that Boyle, after discussing the theory with Towneley and reading a pre-publication manuscript of "Experimental Philosophy" cited the hypothesis as the sole work of Richard Towneley. Boyle's mention of the theory preceded the publication of "Experimental Philosophy" by one year, which, combined with Boyle's promotion of the idea and his significant status as an aristocratic scientist, ensured the theory would be known as "Boyle's Law." [5]
I like that you broke down each portion of the ideal gas law equation. Keep up the good work :)
I love Crash Course! Just wondering... think maybe you could make them less crashy coursey? You know, pause for breath between words now and again. I would love to see these episode lengths go up to the 22-23 minute mark so that we can allow students to have more internal processing while the video is still playing in class. ( for example, show more experiments, maps, illustrations, practical demonstrations, real world applications). It doesn't have to be Thoughtbubble (I know your contract and collaborations with them are limited and specific), but just maybe some other way of illustrating and expounding on whatever the lesson of the day is.
Just a thought. Wonderful work you and your brother do! Huge fan, keep it up!
That would be so much work and this is free education. I think this fast method is kinda cool, quick information with colors and little animations that compare things like the cation animation to help you remember if you're particularly interested you simply do your own research.
Joseph Swanner You could see khanacademy. They have a free course of Math, Science (Chemistry too!).
Change the playback speed to .75 or .5
If they did that they wouldn't need to employ teachers; we could all watch crash course lol. Works for me.
This is an excellent episode of CC. Great job Hank and all of the CC team. Took me months to get my head round this at degree level. Wishing I'd seen this sooner.
I'm so glad nobody decide to enter my room when I was watching 0:20
jortjuuuuuh Porn would have been easier to explain..
jortjuuuuuh 2 11 you can see Henry powers showing a middle finger to bolye and townleey....
I am onto you CrashCourse and Thought Café
3:05ish is where he starts talking about the science :) You're welcome. Everything else is cool too, but when studying, it can be helpful to know exactly what you need to know
Thanks
+horsecrazy2266 You're the best
EMNstar Thanks haha :)
thanks bro
Tanmay Deshpande no problem aha
there's also Gay-Lussac's law of pressure and temperature :) in which pressure is directly proportional to temperature (P/T = K)
Why don't you guys have physics crashcourse
See, them doing a physics crashcourse is easier said then done. They would need to teach a bunch of advance math, which not many of the viewers actually have that mathematical background knowledge.
Richard smith Then why not do a mathematics course? I'm in AAT H (Advanced Algebra Trigonometry Honors), and I would love help on that subject. I currently have a C, so I actually need it.
I would love to see that.
Vixen TheFox i would also love a mathematics crash course, not that i'm in college but i find it incredibly interesting. the thing is that math is so incredibly broad i don't know how they would manage to do a "mathematics" crash course.
Richard smith There is algebra based physics which is very simple. It's not like crash course really goes into the higher level chemistry anyways.
such an amazing job at teaching chemistry, keep up the great work!
Studying for my chemistry final, and I have never gotten Gases until now. My class would be so less boring with Hank Green teaching.
Thanks for the jargon!
STP=0°C 100kPa
n at STP=22,4 L
ABSOLUTE ZERO=0 K=-273,15°C
Bananas=Chom choms
you can actually see the number of views for this video going up during the exam period :p
blackbirdie Cheaters be cheatin
In the midst of trying to feel the air, I bashed my elbow on the radiator
+Alisha Padaruth (AlishThePanini) you should put your hand in front of a fan
so you really did feel the gas (get it the radiator)
omg I love this.
He's really great at explaining things.
The energy and his enthusiasm.
I'm a fan.
thanks a lot :)
2:58 thank you, you have probably helped thousands of students from that, and thank you for your videos which help millions.
I love that can experiment, that's just amazing. Especially since, from what I understood, since the atom in the can slowed down so much the air outside the can just busted through. The very air you're feeling broke though metal because inside the metal was too calm.
You have no idea how much you have helped me! You helped me pass A&P, and now in Physics! You rock, and I love your teaching style. Thanks for really helping me out!!!
Actually, I believe the study of making yourself look cool while waving your hands around is called martial arts. (joke)
At my first job, I used a bead blaster to blast some aluminium. This involves a vacuum chamber with thick rubber gloves sticking into it. When I first started using it, I was very surprised at how easy it was to move my arms despite the thick rubber gloves.
Before then, I 'knew' that air was there, and that it had mass, but experiencing lack of air really changed my perception of the stuff that always surrounds us!
Don't be confused! The Universal Gas Constant can also be .0821 (L*atm)/(mol*K)
That's what I was taught.
Yes
That's because you're using ATM, it really depends on the units involved
Can you please make a Crash Course Physics playlist??? PLEASE!
You guys explain everything so well, and physics is one of the most confusing things ever.
I love the can crush experiment! I learned about in physics, of all things. How sad that college chemistry did not show me this.
crash coursing my way through 1st yr chemistry...
baby hank is so cute
Guys at 4:25 his mac book runs out of battery LMAO!!!!!!!!!!!!!!!!!!
LOL
I love you so much Hank. My chemistry teacher explained this for 3 hours and I didn't understand it at all.
Who went to Henry Power's Wikipedia page?
ngjo3y I did!
+ngjo3y Mee TOO!!!
I did as well!
i thougt to go but too much of work for me!
Meee
"The bad news is, they almost never behave themselves."
Damn that's true.
I got finals in two weeks and this is how I study for it.
same bro
"You can't look cool while you're feeling it. But you can feel it." ... That pretty much goes for all the feels.
Teachers be assigning this vid
Wish my chem lecturer was as enthusiastic as you, if he was i wouldn't be here days before the exam trying to re learn everything from the semester.
Thank you so much for this video series because it's helping me study so much and the things I memorized actually click and make sense now
There are 3 different "R's". It depends on the pressure units. You use .0821 when you're using "atmospheres", 8.31 for kPa, and 63.1 for mm Hg.
Whoa this really helped me. I had been so curious about this but my teachers won't explain it to me at school. Thanks a lot!
Summarized three weeks of our Gases Unit🙏
0:09
"It's everywhere!"
*lets go of balloon
*balloon releases gas
Hank in his mind: i have achieved _humor_
Hank Green the Sci Fiend, one of my favorite scientists.
Thank you for breaking down scientific theory in laymen's terms!
when you're already studying for chemistry on the first day of school
This is my first time watching a video on this channel but it was really helpful and enjoyable ! Subscribed ! I absolutely love his character and his way of teaching. ♡
"You can feel it if you wave your arms around" Me: *smiles* * waves arms* *knocks my phone that I'm watching this on out of my hand*
I'd like to say I still appreciate whomever adjusted the volume of the into to not be so loud relative to the rest of the video. I notice this often.
"You can remember the Ideal Gas Equation because it looks like Pervnert."
Don't remember what cheesy-ass science video that was from, but I busted up laughing when I saw that.
Did the can demo today in class! Then we watched a video of the same thing happening to an oil drum. Really cool.
Ap Chem problems
much love to hank green he brings the joy to chemistry , which is usually made lifeless by universities
I love seeing the green in his hair, knowing he's using a green screen.
Amy LPS Productions he isnt
Out of every episode I've watched on RUclips this one explains the Ideal Gas Law the best
Awesome.. The government should pay you for this
something I never quite understood: If we imagine a closed container filled with 1 mol of a molecular gas and these molecules then split into 2 smaller molecules each, thus raising the number of gas particles from 1 to 2 moles - the ideal gas equation would suggest that the pressure of the whole system would increase. However: if we look at a single molecule it seems that the temperature must drop. One heavy molecule at speed x produces two lighter molecules which - due to conservation of momentum - should still have the same speed. but since their mass drops the average kinetic energy per particle (and thus temperature) should drop considerably. Also: while it is true that we do have more collisions at the same time due to the increased number of particles, the particles also got lighter by that amount. Is the solution simply that (excluding energy given to or taken out of the system due to the endothermic/exothermic nature of the reaction itself) temperature will drop and pressure stays constant?
Thumbs up if you waved your hands at 0:20...
I didn't so i dislike
dont ask for likes
In school to be a respiratory therapist, so gas laws are very close to my heart. Good vid
Who want's to know where the ideal gas law comes from?
A gas exerts pressure on the walls of a contain
er due to the collisions of the gas molecules
with the walls. We start with a single molecule or atom of mass, m, moving backwards and forwards with a velocity, V=(Vx,Vy,Vz) between two walls separated by a distance, L.
Every time the molecule hits the wall it bounces back, reversing the x-component
of its momentum. Its momentum P=(Px,Py,Pz) therefore changes by:
ΔPx=−2mVx
The time between two collisions with the same wall is how long it takes to traverse the box twice and get back to the same wall:
Δt=2L/Vx
Using Newton’s second law, the force by the molecule acting on the wall is:
Fx=−ΔPx/Δt=2mVx/(2L/Vx)=m(Vx)^2/L
To get the overall gas pressure P on one wall, we need to sum together the contributions due to N molecules in a cubic container of side, L, and take account of the fact that molecules move with varying speeds by taking an average value for (Vx)^2:
P=Force/Area
=ΣFxL2=Nm/L^3
=Nm/V
where we have replaced L^3 with V, the volume of the gas.
In practice we don’t measure or consider the average velocity in one specific direction, but only the average speed in any direction (Vrms=√ is the average or root-mean-square (rms) speed of the molecules). These are related in a simple way Vrms^2 = ++ and since there is no preferred direction Vrms^2=3=3=3 hence finally we get P=NmVrms^2/3V from which we see clearly that the pressure is determined directly by the random kinetic energy of the gas molecules. If we rearrange this trivially to read: PV = 2N/3×mVrms^2/2
we begin to see how the ideal gas law arises - we have already got
PV on the left hand side and we have something proportional to the average kinetic energy on the right hand side.
If we compare the ideal gas law: PV =NkT to the expression we have just derived we see the direct relation between the temperature and the average kinetic energy (1/2)mVrms^2 per molecules of a gas. The average Kinetic Energy, , of a gas molecule is: =(1/2)mVrms^2=(3/2)kT
Therefore:
PV = (2/3)N x (3/2)kT
PV = NkT = nRT
You know, I would probably find chemistry really interesting if college did not force me to learn it and use my future career and thousands of dollars in tuition as what felt like a hostage.
This was a nice recap of my school material.
I thought I've forgotten it already since I study Architecture at my university, but no I remember quite a bit.
And thanks to shows like this will not be able to forget at all. ;)
When you have the ap chem exam in two days but still need assurance so you check crash course.
Your chemistry series truthfully covers the majority of thermodynamics in an introductory physics class
ur awesomeee!!! crash course physics?
Thank you!
The words "Jargon Fun Time" only appear on the annotation if you mouse over it,
Yeah, I know about that part. I was actually talking about the way it's presented and where in the syllabus. It doesn't really "fit" where it's put because it's like a blob of Physics in a Chemistry class. But I think that's because we try to teach the sciences as if they were discrete subjects and fail to make the necessary connections between them.
why don't you post some experiment videos
Indeed there is; it's more an issue for what the symbol means. For example, if I say P V = n k_{b} T, and you tried substituting in the number of moles for 'n', you'd quickly find that your answer is off by two dozen orders of magnitude.
I guess the cause of confusion becomes apparent when you work in physical chemistry (or chemical physics), when you have physicists to deal (k_{b} as your constant) and chemists (R as the constant). Inconsistent notation is confusing!
Fun fact! Scientist have not been able to reach 0 kelvin, they believe it may not be achievable as they believe it is really difficult to make a particle not move at all. Lowest temperature reached is around 1 kelvin.
Oh right! Thanks for the correction XD
3rd law of thermodynamics - you cannot reach absolute zero in a finite number of operations
Oh! So that's the third law, I knew of the first three but not the fourth XD Thanks.
It's 2019 and I'm looking at Hank's outfit in this video and how young he looks and...my brain is breaking.
Studying for the AP Chem exam like...
+Kali Elaine same lol
Hell
A lot of the reason why any organism fails to function at high temperature is that high temperatures make proteins denature (meaning they lose their shape and stop working). Human proteins are very sensitive, because we're used to a constant internal temperature; some bacteria have extremely heat-tolerant proteins, but if you keep raising the temperature, eventually everything will die. :)
How to calculate 1/volume(L^-1) from volume (L)
Lucy Hunt Wow
Lucy Hunt lol
Finally something I haven't learned yet at high school, loved it. And I'm glad you'll go further in the next video.
I really want to thank you. My science teacher is horrible and can't explain anything at all. I have learned nothing all year but somehow managed to get good test scores (mostly by guessing). I am going to be in a much harder class next year because according to my scores, I have learned more than the rest of his students. This channel has really helped me understand at least the basic facts
It is very impressive if you consider that air molecules are hitting the can so hard that it crushes the can.
I remember when I first saw the crushing soda can thing- SO AWESOME.
The most valuable information I gathered from this video is that Hank's IP address is 184.166.87.227.
Air pressure outside the container increases. Pressurised aircraft do not maintain a sea level pressure - it's more like 3000m altitude pressure IIRC. The amount of gas inside your water bottle doesn't change, neither does the temperature (greatly), or the ideal gas constant. So as the pressure outside the bottle increases, and as your water bottle is a pretty poor pressure vessel, the pressure inside also has to increase, which means the volume drops - it deflates.
Man, just like a submarine
I look forward to these more than I look forward to school.
this is for human phisiology i just didnt get how more pressure means less volume and vise versa.. now I do ! thank you crash course
Who is watching in 2022
depends if you are adding or subtracting material (ie gas) from the volume. Otherwise (in a closed system) it stays the same.
Good test is pumping up a tire. pressure, volume, and mol change. Calculate the change in Temperature.
In all my time in school and university, we never used kilopascals, but rather hectopascals (1 hPa = 100 Pa) or just pascals. It's also the unit barometers use, next to bars or millibars.
Some one who knows things on RUclips? I never thought I would see the day. I salute you sir. We must spread our knowledge to everyone. The world is collapsing into idiocy...
>"I personally hate the fact we have multiple units for the same measurement"
I agree. In the manual of all motorcycles* I ever had, the tire pressure is in Pa. But on all the gauges at all gas stations** I have been to, the scale is in bar, and often also psi.
*Japanese
**German
I should take my label maker and stick "1bar=100kPa" on gauges at gas stations for the people who didn't google it yet. ^^
I believe it's because chemistry likes to deal with changes. Whether that be a chemical change or just a physical change. I've had the ideal gas law in all of my physics and chemistry courses though. The part of the law that deals with work is more towards physics.
That can being crushed was really surprising. I was totally expecting the crushing action to take place over the course of 30 seconds or so, not on the order of milliseconds!