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
Literally crying tears of joy. I have a HORRIBLE chemistry teacher, who does not teach us (he just goes through extremely complicated notes and uploads extensively long videos), but expects everyone to master the materials. Tomorrow is our test on Kinetics and Equilibrium and THANK GOD FOR CRASH COURSE (and Hank) BECAUSE IT HAS TAUGHT ME MORE IN
These videos are a great review for my chemistry tests. I'm taking my second chemistry class (for science majors) as a summer course, so we are going through this information rapidly. I had to take it in the summer so that I would be able to take my MCAT at the end of my junior year. These videos have help me review, realize, discover, and remember very often. Thank you Hank and everyone else over there at Crash Couse!
Before I started learning chemistry I did a reaction with my friends where we put Lye into a bottle then add aluminum to it screw the cap on and it explodes we thought it was cool... but know I enjoy it even more because I actually know what's going on the aluminium acts as a catalyst and when you drop it in it produces hydrogen gas and steam pretty cool thank you Hank :D
I once watched this series for fun. I once again watched this series for fun. Probably a few more times to help understand certain things during my first university level chemistry class, did pass. Now I'm at the point of breaking down because the "orders" thing was explained by graphs and calculus. Hank Green saves the day, AGAIN.
I have a small bone to pick. The chemical reaction rate can be predicted by theory. There are variety of approaches out there, but Stephen Klippenstein and DG Truhlar of Argonne Nat'l Lab has written a variety of papers on the topic with various coauthors. See: The Journal of physical chemistry 100 (31), 12771-12800; Chemical reviews 106 (11), 4518-4584
This dude is saving my life right now. My chem professor is so monotoned I fall asleep almost every day. I don't feel so afraid of my test tomorrow now.
Amazing, as always! Thank you for these crash course videos, they really do help clear a lot of things up (and they're quite fun). P.S. at 4:19 I think there's a typo, shouldn't it be "Amount of H2" instead of "Hz"?
Hi Hank, I've been reading Six Easy Pieces by Feynman and he also states that atoms "bang into each other" but it is my understanding that it is an interaction of the forces between atoms which drives their movement and that nothing ever actually touches. I understand that the language of the quantum world is in some cases inherently equivocal, but I was hoping for clarification on this topic. Thank you, Andrew
lulublondy But why does he hope they sold funnel cakes in chemistry class? (I would understand why you would want a dessert in school, but why funnel cakes specifically?)
A catalyst actually provides an alternative pathway for the reaction with a lower activation energy, thus more molecules and particles have an energy greater than or equal to the activation energy, speeding up the reaction.
For the people that are saying this is easy he is explaining the basic concepts so the student can understand and keep improving on there own, this is simple quick and easy thats why its called crash course
I think this is the first episode I have understood without having to go back and watch it. I feel this is because I am finally understanding Chemistry, thanks guys :)
When both exponents are 0, the concentration terms both become 1. This simplifies the rate equation to simply k, a constant. So no matter how much of each reactant you start with, the rate will always be the same. An example is the reaction H2 + Cl2 --> 2HCl (hydrogen gas + chlorine gas => hydrogen chloride gas).
I see that many people have a problem with Reaction Rate Law.Rate Law links reaction rate with concentrations (or pressures) of reactants.A reaction can be written as ---- aA + bB ----> cC + dDThe coefficients(a, b, c and d above) of a balanced equation tell us in what ratio the substances react or are produced.The powers of '[A]' and '[B]' in the rate law expression i.e. 'n' and 'm' does not mean 'a' and 'b' i.e. the ratio in which reactants react rather the power is the relation between concentration of reactant and the rate of reaction. In the reaction at 5:12 , if the concentration of H2 is doubled than the rate of reaction(how fast reaction will occur) is doubled. If concentration of reaction is tripled than the rate of reaction is tripled.And if the concentration of NO is doubled the rate of reaction becomes 8 times. If the concentration of NO is tripled the rate of reaction becomes 27 times.So , in case of H2 the relation between concentration and rate of reaction gives 'm'='1'........[H2]^1.Similarly in case of NO the relation between concentration and rate of reaction gives 'n'='3'.........[NO]^3.Finally , we can say that order of reaction = n + m = 3+1 = 4. So this type of reaction is called fourth order.If in a reaction increasing the concentration (like doubling or tripling) does not increase the rate of reaction than the value of 'n or m' their is 0.Order of reaction is decided by the exponential powers of all the reactants.
At 8:09' in describing the role of a catalyst, the common expression "lowers the activation energy" is used. A better description is that a different mechanism is provided through the catalyst and the activation energy of that pathway is lower than that of the uncatalysed reaction.
It is still suggested to Read your text book . There are many equation stuff that were hard to explain in this short vid . After all this is just a crash course.
Great lesson overall. A small problem at 3:45' when describing the form of the rate equation. It is explicitly stated that only the reactants are included. When looking at overall reactions (macroscopic scale) there is no a priori reason to exclude products or catalysts in the rate law. It is common to have only reactants, and in teaching we tend to stick with this paradigm, but it is not the law.. A rate law that has a product with a positive reaction order will be "self-catalysing".
Strictly speaking, catalysts don't lower activation energies, but provide additional pathways that have lower activation energies. Because the apparent (observed) activation energy
Great way to prepare yourself for college level chemistry before the semester starts. CrashCourse, you guys really do need to add a Crash Course Physics section!
It helped me understand the collision theory better, but the formula part just went over my head. Only hw practice will help me understand that at this point.
Catalysts, change the reaction mechanism; it does not lower the activation energy. The new reaction mechanism has a lower activation energy so it requires less energy, so it looks like activation energy has been lowered but you have not.
The rate law for the reaction at 5:12 is - k[H2][NO]^2 Source : www2.chem.umd.edu/lms/claroline/backends/download.php?url=L0RJU0NVU1NJT04vS2luZXRpY3NXb3Jrc2hlZXQyQW5zLnBkZg%3D%3D&cidReset=true&cidReq=CHEM271
This video is perfect it gave me a great conceptual understanding of kinetic energy. The only thing I'm still unclear about afterwards is how to determine the exponential value of the reactants concentrations in the rate laws after performing the reactions experimentally and determining the rates of the reactions.
I really like these video series! But I have to point out a small mistake (chemical kinetics is my research field :). In the three steps converting NO + H2 to N2 + H2O at 8:03, step 1 (NO + H2 -> H2O + N) is actually the rate limiting step--it's very endothermic. That's one reason that once you make NO it's pretty hard to get rid of. But in general, great job with these videos!
7:00 Hank states that most reactions aren't in equiblirum because the reverse reaction's activition requires high activation. "Why? Because, remember, reactions take place in steps". What is the relationship between the high activation of the reverse reaction and reactions taking place in steps?
At 4:30, you said that to double the hydrogen you raise the exponent to the power of 1. However, raising anything to the power of 1 leaves it the same. Can you please explain this?
I dunno about the speed of light bit, but the extra energy just gets transferred to the product molecules as kinetic energy (for non-c speed reactions). so if the molecules have to hit at 10 mph to react, 1 is travelling straight at the other at 7 mph the other at 8, then the products would have enough energy to give 5mph between them (roughly, ask a maths person for the accurate answer) for motion.You'd have to ask a physicist (probably a theoretical kind) for the other bit.
Out of curiosity Hank, do you have any degrees ? I'd assume that you have a degree in chemistry or some form of scientific degree with how well you can explain concepts :)
You make learning somewhat boring things very fun! Thank you for that! I also thank you for the little section center at the end of all of your videos! Thank You!
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
good luck to everyone watching this the day before the test!
2019
Thx bro
*Day of the test
Thanks bro🙏🙏
🤝
Literally crying tears of joy. I have a HORRIBLE chemistry teacher, who does not teach us (he just goes through extremely complicated notes and uploads extensively long videos), but expects everyone to master the materials. Tomorrow is our test on Kinetics and Equilibrium and THANK GOD FOR CRASH COURSE (and Hank) BECAUSE IT HAS TAUGHT ME MORE IN
Shout-out to Ms. Frizzle for winning the demolition derby
you won the comment section
She probably cheated. It's a magic school bus after all.
Man, if crash course didn't exist, I would not be passing my chemistry class.
more like i would be passing out during chemistry class
I would like to thank Crash Course and coffee for my education...
These videos are a great review for my chemistry tests. I'm taking my second chemistry class (for science majors) as a summer course, so we are going through this information rapidly. I had to take it in the summer so that I would be able to take my MCAT at the end of my junior year. These videos have help me review, realize, discover, and remember very often. Thank you Hank and everyone else over there at Crash Couse!
This literally helped me understand kinetics more than my 3 months chemistry course at MSU lol.
Before I started learning chemistry I did a reaction with my friends where we put Lye into a bottle then add aluminum to it screw the cap on and it explodes we thought it was cool... but know I enjoy it even more because I actually know what's going on the aluminium acts as a catalyst and when you drop it in it produces hydrogen gas and steam pretty cool thank you Hank :D
“It’s kinda intense, but we can handle it. Check it out.”
Basically what I live by
WHY DID I CHOOSE CHEMISTRY IM SO CONFUSED
I love science. ; - ; * ^ *
me 2
How is 0.060 is half of 0.012?
0.0060*
@@wasiangie hi
😂😂😂😂I missed that introduction sound. I haven’t watched a video for school from this channel in a long time. So happy to be back.
This video just summed up my last 3 chem lectures in less than ten minutes and made more sense doing it.
this took cramming to another level
Who wants to have a crying session?
Fun AND intellectual all while teaching us the basics of kinetics? WHAT IS THIS BLACK MAGIC?!
no majiks r involved, just some people who know what gets us
It is the wondrous magic of Hank Green.
Also chemistry is f***ing awesome.
Yes of course, can`t you see the dark mark?
This counts as studying for my chemistry exam next week, right?
Thank you for explaining concepts in such simple and beautiful ways!
I once watched this series for fun. I once again watched this series for fun. Probably a few more times to help understand certain things during my first university level chemistry class, did pass. Now I'm at the point of breaking down because the "orders" thing was explained by graphs and calculus. Hank Green saves the day, AGAIN.
Who cares what grade you're in. Knowledge is knowledge, and grade (In this case) is just a number.
But if you're not old enough, you can't buy a bunch of bookcases and a Lamborghini to put in your garage.
dang if you play the video at half the speed Hank will sound as if he is totally drunk :)
+Ziyad Mohamed amazing
+Ziyad Mohamed That is brilliant! Much better way to watch the video my teacher assigned.
+Ziyad Mohamed lollll tru!
lol
Even the theme music sounds drunk
He summarized the whole chapter of my book in just 10 mins. Wow!
Hank Green....
....Bless you.
How does he have the lung capacity for this?
dat sweet sweet editing
who knows who cares, i don't
He's mastered biology
I had to teach this earlier, collision analogies and all - the day after the news of Paul Walker's fate became widespread.
It wasn't easy
@6:30 the lightbulb just came on! Thank you Green Bros. and Co.!
I have a small bone to pick. The chemical reaction rate can be predicted by theory. There are variety of approaches out there, but Stephen Klippenstein and DG Truhlar of Argonne Nat'l Lab has written a variety of papers on the topic with various coauthors. See: The Journal of physical chemistry 100 (31), 12771-12800; Chemical reviews 106 (11), 4518-4584
This is also relevant for college chemistry and I'm overwhelmingly thankful it exists! Thanks guys!
This dude is saving my life right now. My chem professor is so monotoned I fall asleep almost every day. I don't feel so afraid of my test tomorrow now.
this was the most sexual first 3 minutes of a crash course yet
Hahaha genius..It got pretty gay at 2:15 though lol.
I know right, "So if chemical reactions only work when particles band into each other good and hard" lololololololol
i thought nobody noticed it
I thought I was the only one who noticed 😂
1Poiuytgfdsa1 Um.. biology has like 5 videos about reproduction, including human reproduction
This helped very much! Thanks crash course❤ From India
Amazing, as always! Thank you for these crash course videos, they really do help clear a lot of things up (and they're quite fun).
P.S. at 4:19 I think there's a typo, shouldn't it be "Amount of H2" instead of "Hz"?
I love this guy so much his teachings are 😍😍😍 I wish their was cashcourse math
There is crash course statistics
I have a test in AP Chem tomorrow! This helped me a lot! Thanks!
Only if Crash course Knew about 10 min mark .
I would have 0 in chemistry without Hank.... Thank you ! I love you and appreciate your work.
You saved my ass. This was the one thing that was killing my chem grade.
Hi Hank,
I've been reading Six Easy Pieces by Feynman and he also states that atoms "bang into each other" but it is my understanding that it is an interaction of the forces between atoms which drives their movement and that nothing ever actually touches.
I understand that the language of the quantum world is in some cases inherently equivocal, but I was hoping for clarification on this topic.
Thank you,
Andrew
Dang-it! Now I want funnel cakes!
Me too! D=
lulublondy But why does he hope they sold funnel cakes in chemistry class?
(I would understand why you would want a dessert in school, but why funnel cakes specifically?)
coolcatho13 Funnel cakes are sold at demolition derbies and he was comparing a demolition derby w/ chemistry class.
the words used to describe kinetics have changed my view on chemical reactions forever.
Cattle-lists, I geddit
"If you paid attention" I feel called out 😭
A catalyst actually provides an alternative pathway for the reaction with a lower activation energy, thus more molecules and particles have an energy greater than or equal to the activation energy, speeding up the reaction.
LOVE the breaking bad reference / You are amazing for including it :)
just wanted to say crash course both chemistry and economics r real lifesavers.
For the people that are saying this is easy he is explaining the basic concepts so the student can understand and keep improving on there own, this is simple quick and easy thats why its called crash course
I think this is the first episode I have understood without having to go back and watch it.
I feel this is because I am finally understanding Chemistry, thanks guys :)
crash course is a blessing we do not deserve
When both exponents are 0, the concentration terms both become 1. This simplifies the rate equation to simply k, a constant. So no matter how much of each reactant you start with, the rate will always be the same. An example is the reaction H2 + Cl2 --> 2HCl (hydrogen gas + chlorine gas => hydrogen chloride gas).
I see that many people have a problem with Reaction Rate Law.Rate Law links reaction rate with concentrations (or pressures) of reactants.A reaction can be written as ---- aA + bB ----> cC + dDThe coefficients(a, b, c and d above) of a balanced equation tell us in what ratio the substances react or are produced.The powers of '[A]' and '[B]' in the rate law expression i.e. 'n' and 'm' does not mean 'a' and 'b' i.e. the ratio in which reactants react rather the power is the relation between concentration of reactant and the rate of reaction. In the reaction at 5:12 , if the concentration of H2 is doubled than the rate of reaction(how fast reaction will occur) is doubled. If concentration of reaction is tripled than the rate of reaction is tripled.And if the concentration of NO is doubled the rate of reaction becomes 8 times. If the concentration of NO is tripled the rate of reaction becomes 27 times.So , in case of H2 the relation between concentration and rate of reaction gives 'm'='1'........[H2]^1.Similarly in case of NO the relation between concentration and rate of reaction gives 'n'='3'.........[NO]^3.Finally , we can say that order of reaction = n + m = 3+1 = 4. So this type of reaction is called fourth order.If in a reaction increasing the concentration (like doubling or tripling) does not increase the rate of reaction than the value of 'n or m' their is 0.Order of reaction is decided by the exponential powers of all the reactants.
If anybody wants some help regarding Chemistry, Physics or Maths you can ask me on mohitcooper@gmail.comI am happy to help.
At 8:09' in describing the role of a catalyst, the common expression "lowers the activation energy" is used. A better description is that a different mechanism is provided through the catalyst and the activation energy of that pathway is lower than that of the uncatalysed reaction.
It is still suggested to Read your text book . There are many equation stuff that were hard to explain in this short vid . After all this is just a crash course.
I cannot believe they came back and added chapter to a 9 year old video.
Hank could be an auctioneer.
I laud you for speaking strictly. We wouldn't want to teach that the world is flat
Great lesson overall. A small problem at 3:45' when describing the form of the rate equation. It is explicitly stated that only the reactants are included. When looking at overall reactions (macroscopic scale) there is no a priori reason to exclude products or catalysts in the rate law. It is common to have only reactants, and in teaching we tend to stick with this paradigm, but it is not the law.. A rate law that has a product with a positive reaction order will be "self-catalysing".
Was the winner of the demolition derby a reference to "the magic school bus"?
Omg, I didn't even see that
Nice video.
Can anyone recommend me another best TH-cam channels to learn Chemistry?
Kinetics, the bread and butter of chemical engineering.
I read a chapter of an Analytical Chem textbook on Kinetics, yet this video was more informative. Well done.
Thank you so much! This is DEFINITELY the crutch I need to survive Chemistry!
Strictly speaking, catalysts don't lower activation energies, but provide additional pathways that have lower activation energies. Because the apparent (observed) activation energy
4:28 Amount of "Hz"? It should be H2.
Ya I think ur right.
ya
Good catch.
i see Our Heisenberg in 4:09 and appreciate it, thanks thought cafe!!
Ms. Frizzle as a demolition derby champion...... YES
Great way to prepare yourself for college level chemistry before the semester starts. CrashCourse, you guys really do need to add a Crash Course Physics section!
It helped me understand the collision theory better, but the formula part just went over my head. Only hw practice will help me understand that at this point.
Haha, Sweet Tooth cameo. Somebody's been playing Twisted Metal.
Kommandant7 I was wondering who else noticed that!
Catalysts, change the reaction mechanism; it does not lower the activation energy. The new reaction mechanism has a lower activation energy so it requires less energy, so it looks like activation energy has been lowered but you have not.
studying this at school right now ! i love it when crash course aligns with my school syllabus :)
The rate law for the reaction at 5:12 is -
k[H2][NO]^2
Source : www2.chem.umd.edu/lms/claroline/backends/download.php?url=L0RJU0NVU1NJT04vS2luZXRpY3NXb3Jrc2hlZXQyQW5zLnBkZg%3D%3D&cidReset=true&cidReq=CHEM271
Ms. Frizzle beat Sweet Tooth from Twisted Metal 😂😂
+Background Hero Media Of course she did, she has a magic school bus. Seems like cheating really.
+Background Hero Media "It's time to take chances, make mistakes, shut up and bleed!"
+Duke Travers Lol 😅
Magic School Bus is a win button in any Demo Derby since it can transform into anything you need. She could change it into a tank and wreck everybody.
the bus still can easily take a car down
Wish this went more in depth ;-; Is there an AP version?
Lol AP
Bozeman Science is a youtube channel that has videos on AP chemistry. It goes into more detail.
Do you find it at all ironic that you spelled illiterates wrong?
You are awesome as usual!! Thank you for the lesson. Love learning on TH-cam.
Morning tea and chemistry. I feel like I should write a song about watching crash course.
why is no one mentioning the many sexual jokes that can be made from this
AnimeArtista Atoms are banging .
AnimeArtista Just how hard do they have to bang into each other?
I'm quoting all those for a paper I'm doing for my chemistry class on kinetics
Jay Newton good luck :)
atoms and molecules need to bang hard and good
this is literally the only helpful resource i have found for kinetics. thank you!
This video is perfect it gave me a great conceptual understanding of kinetic energy. The only thing I'm still unclear about afterwards is how to determine the exponential value of the reactants concentrations in the rate laws after performing the reactions experimentally and determining the rates of the reactions.
If only they would sell funnel cakes before the AP chem exam i have tomorrow :(
I really like these video series! But I have to point out a small mistake (chemical kinetics is my research field :). In the three steps converting NO + H2 to N2 + H2O at 8:03, step 1 (NO + H2 -> H2O + N) is actually the rate limiting step--it's very endothermic. That's one reason that once you make NO it's pretty hard to get rid of. But in general, great job with these videos!
I love you Hank Green, I love you so much 😭 I have an AP Chem final this Monday and I am dyinggggggg
I like your history lessons the most.
7:00 Hank states that most reactions aren't in equiblirum because the reverse reaction's activition requires high activation. "Why? Because, remember, reactions take place in steps".
What is the relationship between the high activation of the reverse reaction and reactions taking place in steps?
Does this mean the forward reaction takes less energy than the reverse reactions, because it takes place in steps?
Products usually have lower energy than reactants. Thus, to go back to being reactants they need more energy than it took to become the products.
At 4:30, you said that to double the hydrogen you raise the exponent to the power of 1. However, raising anything to the power of 1 leaves it the same. Can you please explain this?
I'm shocked you went with funnel cake instead of fair corndogs, Hank!
Also, nice Equilibirium reference.
Chem midterm tomorrow = CrashCourse tonight!
I feel like talking about catalysts in this episode would have been important and relevant
I dunno about the speed of light bit, but the extra energy just gets transferred to the product molecules as kinetic energy (for non-c speed reactions). so if the molecules have to hit at 10 mph to react, 1 is travelling straight at the other at 7 mph the other at 8, then the products would have enough energy to give 5mph between them (roughly, ask a maths person for the accurate answer) for motion.You'd have to ask a physicist (probably a theoretical kind) for the other bit.
you have an amazing talent for teaching, i hope you have the success in life that you earn
Out of curiosity Hank, do you have any degrees ? I'd assume that you have a degree in chemistry or some form of scientific degree with how well you can explain concepts :)
After the rate laws.. i was like " i've never learnt this at school.."
48 hours later i will be taking a chemistry exam. Thanks to crash course for giving me a final tip!
It is the best video on kinetics . Thank you Hank and the team.
could u do an episode about catalysts as most teachers try to fudge the explanation of how they specifically work?
I don't putt facing west exclusively, but in the back on my mind I'm haunted by the notion that I'm sure it's the best way to putt.
Crash Course Physics would be really neat.
Nice Magic School Bus reference.
Demolition Derbys kick butt!
Yes Chemistry is exciting and I came to know it through your lectures only Mr. Hank. Thanks :)
THANK YOU FOR THESE VIDEOS OMG
You make learning somewhat boring things very fun! Thank you for that! I also thank you for the little section center at the end of all of your videos! Thank You!