Chemical Kinetics - Free Formula Sheet: bit.ly/3zYmDjy Direct Link to The Full 53-Minute Video: bit.ly/3vPPUad Chapter 12 - Video Lessons: www.video-tutor.net/chemical-kinetics.html
This guy has taught me more than any of my university professors. He is better than my calculus, physics, and chemistry teachers. Keep it up, God bless you!
Professor Organic Chemistry Tutor, thank you for showing/explaining How to write Rate Law expression for a reaction Mechanism in AP/General Chemistry. Writing the Rate Law reaction for mechanism is not a difficult process, however finding the catalyst and intermediate in the reactions is confusing. I will rewatch and review this material from start to finish. This is an error free video/lecture on TH-cam TV with the Organic Chemistry Tutor.
13:15 there are two NO2's so why is it not third order. when you had 2A + B -> C you did [A]^2 [B], so why dont you also put it to the power of 2 in that one. Thanks
Question: at time 13:20 Since there is one molecule of O3 and 2 molecules of NO2, Shouldn't k= [O3] [NO2]^2? Then the reaction would be first order with respect to O3, second order with respect to NO2 and third order overall?
No, the rule that you are thinking of, about the molecularity and how the coefficients equal the reactant order, only applies to "elementary reactions". It does not apply to this overall reaction because it is a multistep reaction. He says this at 9:05 . The reaction order(s) of an overall reaction that is multistep depends on the rate law of the determining step.
@@keanupie8399 It's been awhile for me, but I think they will usually either give you the rates of each step, or they will simply tell you one of them is the slow step depending on the question.
It would be, except that he adds that the first step is the "slow" step, and the second step is the "fast" step. Since the slow step always determines the speed of the reaction (think "you can't go faster than the slowest person in line"), then you only use what's in the slow step, which, in this case, is just one H2O2. If it's still confusing, go back and check the previous example that he showed, and compare its answer to his first example, which didn't use the "slow" or "fast" rates.
For a multi-step reaction, the slow step (rate limiting/rate determining step) determines the rate of the whole chemical reaction even when your overall reaction has different molar coefficient/s. In other words, stick to the slow step at all times when writing the rate law of the reaction.
I've watched many of your videos, which were free on TH-cam ever since. But now, you have moved your full content to Patreon. I understand that, your time is worth a lotta bucks. But, poor students who were benefited by your videos will no longer be able to gain that benefit anymore. And that's sad.
@@Garret_bruh_homey Yes he has a lot of free stuff. But still, most of his good content is now paid. You won't understand unless you benefited from his great content and now don't. And most of the content the TH-cam has is nowhere close to this man's content in quality. I will reiterate that poor students are missing a great opportunity, that they had before.
I'm just a bit confused. So the coefficients don't matter when determining what type of overall reaction it is? How would you be able to distinguish bimolecular reaction from a unimolecular reaction?
idk if this will help but overall rate law can only be determined experimentally. So like looking at the graphs or tables. so I think concluding the order of each reactant for overall rate law was a mistake. Elementary reaction on the other hand, you can calculate by looking at molecularity. One cannot determine the order of each reactants in overall balanced equation simply by looking at coefficients. Does that help?
the rate of the overall reaction is limited by, and is exactly equal to, the combined rates of all elementary steps up to and including the slowest step in the mechanism, therefore its should be K[H2O2]2
The slow step in elementary reaction is considered to be the rate determining step. It is always the slow step for the basis of overall rxn. The reason why we only have [NO2] in the overall.
what happened to that other fast/slow step video where u had an example of a slow step being in the middle of the reaction? im trying to find that vid and i cant find it did you delete it? in that vid you showed us why the overall order is different from whats in the slow/fast steps, it was rlly helpful, on this one u gloss over it like in 13:18.. why is NO2 not raised to the 2nd power? :(
NO2 isn't raised to the second power because it depends on the slow step of the reaction. Usually at this level they give you all the information about the system in the question . Rate determining step = first slow step
10:20 Sir Why u took only 1st reaction as slow reaction and 2nd one as fast reaction...Please reply sir I am in confusion please And sir I like your teaching sir....Thankyou for this lecture sir....I understood everything except that one thing please sir answer my question sir
Hey he said the first reaction they give you is usually the slow step unless they specify otherwise. At A- level dont bother learning the actually systems they will tell you a you need to know in the question
Should the orders be experimentally determined and not by the coefficients? This is what I’ve learned in rate law. Are we just assuming that the coefficients are the order or reaction? But may show a different order in an experiment? Thanks
I think the "overall" rate law equation is wrong. I think it is supposed to be the exact same as the rate law equation of the slowest elementary step, which includes the catalyst. Please recheck for us, please.
Chemical Kinetics - Free Formula Sheet: bit.ly/3zYmDjy
Direct Link to The Full 53-Minute Video: bit.ly/3vPPUad
Chapter 12 - Video Lessons: www.video-tutor.net/chemical-kinetics.html
@@xshxr 😆😆😆
a dislike for paying money to watch full tutorial goodjob:)
@@xshxr these are the best tutorials on the web, clear, focused, and straight to the point, class, pay a few dollars for them.
wtf wrong with people in the comments if you don't wanna pay just quiet he's been helping people for free
I agree
This guy has taught me more than any of my university professors. He is better than my calculus, physics, and chemistry teachers. Keep it up, God bless you!
This guy is single handedly tutoring the world!
Respect 🙏🏾
My professor literally "taught" us this just last class... needed this! Thanks!
an absolute legend. Got an 87% on my Gen Chem 1 final because of you and an 86% in the class. Now you're getting me through Gen Chem 2!
Lol literally same!!!
I JUST CAME ONTO TH-cam TO FIND HIS VIDEOS ON RXN MECHANISMS my guy u are my savior
The fact that you are keeping up with me by posting these videos as I'm learning this material is perfect. Thank you
I didn't realize he's following perfectly with my course until this comment... dang
hey, I think I remember u did u live in Ottawa at some point?
can i get ur snap
For everyone wondering on why it’s not 2h2o2 for the last one it’s because overall reaction is solely determined on slow process
I was confused at first but thank you for clarifying that!!
Thank you very much!
THANKS!!! Have a chem test tmw and was confused
Isn’t having I in rate equation a violation to one of the conditions? And then replace it using rate formed = rate reversed?
If it is soley determined on slow process, why is there no I-?
The simplicity of these videos along with your clear explanations make them really useful and time-saving.
Thank you!
My class literally started learning about this week. You are savior my dude. Keep up the good work 👍
Biggest coincidence of my life i was literally learning this
Me too
Its algorithm doing its job not a coincidence😌
I'm so glad this man is getting the recognition he deserves 4 mil keep going my boy
Thank you so much
I told my friends about u and advised them to subscribe to ur TH-cam videos.
U are a great help to all of us
Thank u from Nigeria
He is of great help
Your videos boost my understanding in every unit of chemistry,,thumb up and thanks so much🙏🙏
This is perfect timing!!! Just after my teacher taught this and I didn't understand, I found you!!!
Professor Organic Chemistry Tutor, thank you for showing/explaining How to write Rate Law expression for a reaction Mechanism in AP/General Chemistry. Writing the Rate Law reaction for mechanism is not a difficult process, however finding the catalyst and intermediate in the reactions is confusing. I will rewatch and review this material from start to finish. This is an error free video/lecture on TH-cam TV with the Organic Chemistry Tutor.
Lol tell me why this was the perfect timing. I was looking for your explanation on this for so long.
i got an A+ grade in chemistry because of you
Bro you have everything. I love you man, your videos been saving me since Year 1 😭❤️❤️
Since the rate law is determined by the coefficient of the reactants…
Then why is 2H2O2 written as “k[H2O2]^1” instead of “k[H2O2]^2”
That’s what I was thinking
Turns out it’s because we only write what the slow step is. Since the slow step only has H2O2 we only write that since we follow the slow step only
Now does mean also the overall reaction also depends on the slow reaction or what??😢
@@RichardMwaba-g4e exactly that's what he said in the video "The rate will always depend on the slow step"
Its because the rate law is affected by the stoichiometric coefficients only for the elementary reactions, not for the overall reaction
13:15 there are two NO2's so why is it not third order. when you had 2A + B -> C you did [A]^2 [B], so why dont you also put it to the power of 2 in that one. Thanks
I swear I don't have the money you asking for the full video but you helping me alot
thank you so much, u save my university life
Illiasu from Ghana I love ur tuition wholeheartedly
You helped me a lot more God bless you my brother love your style of teaching ❤️👍🏿
You’re a life saver may god bless you more
Ty so much. Your video literally answered everything in my pre-lab!
my exam for my g12 chem is tomorrow!!! ill be back when I'm in Uni!
This channel has helped me out with my chemistry class. Thank you very much!
Thank you! I was lost on this!
God bless u bro
In my reference book and txt book difficult to understand but in your 18Min video i understood whole again God bless u
Kobby from Ghana
My best tutor ever🙌💕
Hey Gloria, check out my TH-cam channel.
definitely the best video on this concept, thank you
Thank you professor
I really appreciate you are a good tutor
My best tutor🎉
Why are you so good at teaching.
the last thing I had trouble with one day before the final. thank you!!!
thank you so much for this pretty good tutorial ❤❤...your way of teaching is really amazing
crazy how this dude taught me in 18 mins what my chem teacher cant do in 1 hr.... literally no explanation on the slides 😔
Good God we are just about to cover this. Thank you
You are awesome 👍🎉 organic chemistry tutor!!!
I love you so much ❤❤❤🎉🎉🎉🎉
Many Thank U sir::: ! Outstanding social services appreciated. Love you from Sri Lanka ❤❤❤❤
Thank you 😀
and God bless you.
You're highly Good in Chemistry.
You are so amazing man. Best teacher ever
Question: at time 13:20
Since there is one molecule of O3 and 2 molecules of NO2, Shouldn't k= [O3] [NO2]^2?
Then the reaction would be first order with respect to O3, second order with respect to NO2 and third order overall?
So you only look at the rate determining step when writing rate law. The rate determining step will al always be the slow step.
No, the rule that you are thinking of, about the molecularity and how the coefficients equal the reactant order, only applies to "elementary reactions". It does not apply to this overall reaction because it is a multistep reaction. He says this at 9:05 . The reaction order(s) of an overall reaction that is multistep depends on the rate law of the determining step.
@@kingpyrrhusofepirus6686 how do we know which is the slow step?
@@keanupie8399 It's been awhile for me, but I think they will usually either give you the rates of each step, or they will simply tell you one of them is the slow step depending on the question.
@@kingpyrrhusofepirus6686 thank you!
You are blessed ❤❤❤❤❤❤
You are the best from S.Sudan
That's the youngest country , right???
I'm ✨🇵🇭Filipino🇵🇭✨ btw😌🤩
this guy needs a medal
NOCl2 is the intermediate.
Overall rxn mechanism:
2NOCl2 + Cl2➡️ 2NOCl2
Rate law equation
R=K[NOCl2][NO]
Overall rate law
R=K[NO]
Question for the last example wouldn’t the rate constant be= k[H2O2]^2?
That's what I would've thought to
It would be, except that he adds that the first step is the "slow" step, and the second step is the "fast" step. Since the slow step always determines the speed of the reaction (think "you can't go faster than the slowest person in line"), then you only use what's in the slow step, which, in this case, is just one H2O2. If it's still confusing, go back and check the previous example that he showed, and compare its answer to his first example, which didn't use the "slow" or "fast" rates.
For a multi-step reaction, the slow step (rate limiting/rate determining step) determines the rate of the whole chemical reaction even when your overall reaction has different molar coefficient/s. In other words, stick to the slow step at all times when writing the rate law of the reaction.
@@prestonrossi7597 thank u bro
@@gerryaraujo7852 thank you bro
Are you guys really making it a competition to be first when his vids drop?😂
Love in the Air...
i love u benjamin
@@antwondickbutt5986 Don't get you bro
@@Spectrojamz 😔😔
@@antwondickbutt5986 😂 You're acting funny.. You know?
@@Spectrojamz what is the funny about how I act
You never failed in teaching students...
All of his videos helps me a lot
I've watched many of your videos, which were free on TH-cam ever since. But now, you have moved your full content to Patreon. I understand that, your time is worth a lotta bucks. But, poor students who were benefited by your videos will no longer be able to gain that benefit anymore. And that's sad.
Correct
Yes it's very sad
Yes, specifically because as students is difficult to get money because college is expensive 💔😥💔
He still has plenty of free videos on here. And the internet is abundant with free resources. This guilting and moralizing isn’t appropriate.
@@Garret_bruh_homey Yes he has a lot of free stuff. But still, most of his good content is now paid. You won't understand unless you benefited from his great content and now don't. And most of the content the TH-cam has is nowhere close to this man's content in quality. I will reiterate that poor students are missing a great opportunity, that they had before.
you must be a teacher or something because you know exactly what we're learning in the time we're learning it
Damn right!!!
fr
I don't know how I thank u from ethiopia
your a life saver man and u make learning fun
Thank you so much for this! It was very clear!
This video was perfect
You always save me!
I'm just a bit confused. So the coefficients don't matter when determining what type of overall reaction it is? How would you be able to distinguish bimolecular reaction from a unimolecular reaction?
idk if this will help but overall rate law can only be determined experimentally. So like looking at the graphs or tables. so I think concluding the order of each reactant for overall rate law was a mistake. Elementary reaction on the other hand, you can calculate by looking at molecularity. One cannot determine the order of each reactants in overall balanced equation simply by looking at coefficients. Does that help?
@@na-kumlee6317 Thank you!
Only reason I’m passing Chem 2 right now
Thank you for this. Really needed it
the rate of the overall reaction is limited by, and is exactly equal to, the combined rates
of all elementary steps up to and including the slowest step in the mechanism, therefore its should be K[H2O2]2
love you man!
Thank you for the video! I was struggling with this!
another excellent video
18:03 this contradicts Khan Academy. They included catalysts in the overall rate law
khan academy is correct. He probably made a mistake
@@shimshonbalakhani5446 so would the overall rate law be rate=k[H202][I^-]
same here it contradicts my book
I love you. More than you will ever know.
Thanks man, Helped alot.
In 13:20 wouldn't it be Fast Rate = K [ NO3 ] [ NO2 ] rather than Rate = K [ O3 ] [ NO2 ]?
Idek why I'm watching this, idk wtf this is because I solely clicked on this video to hear their voice 😭✋🏻
If you realize it ...his voice same as SHAWN MENDES
shouldn't [NO2] in the overall rate be [NO2]^2 ? since it has 2 NO2 in the equation?
The slow step in elementary reaction is considered to be the rate determining step. It is always the slow step for the basis of overall rxn. The reason why we only have [NO2] in the overall.
@@teacherdanz3794 ohh right right
@@teacherdanz3794 is the first step always the slow step?
@@kjay5587 yes
Euclidean Algorithm please!!
Thank you so much🌹🌹
Thank you for this❤️
THANK YOU MAN!
Thanks sooo much😍🌻✨
I just learned what my teacher couldn’t teach me in a whole semester 😂
That peepy ad got me spooked for life
what happened to that other fast/slow step video where u had an example of a slow step being in the middle of the reaction? im trying to find that vid and i cant find it did you delete it? in that vid you showed us why the overall order is different from whats in the slow/fast steps, it was rlly helpful, on this one u gloss over it like in 13:18.. why is NO2 not raised to the 2nd power? :(
He's forcing you to pay for the longer videos now on Patreon.
NO2 isn't raised to the second power because it depends on the slow step of the reaction. Usually at this level they give you all the information about the system in the question . Rate determining step = first slow step
thank you very much God bless you
I’m soooo confused on why he did [h2o2] [i^-] instead of [h2o2] [no2] for 17:27
also confused on why the IO and I canceled out instead of h2o2
really thanu full to you☺
Perfect timing !!!]
10:20 Sir Why u took only 1st reaction as slow reaction and 2nd one as fast reaction...Please reply sir I am in confusion please
And sir I like your teaching sir....Thankyou for this lecture sir....I understood everything except that one thing please sir answer my question sir
Hey he said the first reaction they give you is usually the slow step unless they specify otherwise. At A- level dont bother learning the actually systems they will tell you a you need to know in the question
@@kxkxsxi6305 Oh.....okay Thank you Now its clear for me
Why are the stoichiometric number not considered in rate expression? E.g 2H2 + O2 = 2H2O
Rate for H20 = [H20] = ½[H2]²[O2]
Very helpful. thanks!
at 12:47 why is NO2 not raised to the power of 2 in the rate law?
Should the orders be experimentally determined and not by the coefficients? This is what I’ve learned in rate law. Are we just assuming that the coefficients are the order or reaction? But may show a different order in an experiment?
Thanks
I believe in elementary reactions, the coefficients correspond to the order, although they are normally determined experimentally
in the overall reaction, why didnt you raise the rate overall for NO2 to the power 2? maybe i missed out on something
For the first example why is it [NO2] for the rate law instead of [NO2]^(2)?
How can you identify the the slow and fast reactions?
It will be given, you are not required to identify
Understandable
I think the "overall" rate law equation is wrong. I think it is supposed to be the exact same as the rate law equation of the slowest elementary step, which includes the catalyst. Please recheck for us, please.
Pay attention stop looking at the comments
Thank you!
Thank you soo much
Wait at the end....why the rate equation doesn't become "rate=k [H2O2]^2" but only to the power of 1??
Yes I have also noticed, because the coefecient of the overall reaction is #2
I think it’s simply because we’re to consider the slow reaction, and not the overall equation.
@@quyumkehinde2683 on the contrary we are only supposed to see the slow reaction . I feel you meant slow but typed fast .
@@aadygoel4837 Exactly! Thank you.
@@quyumkehinde2683 but that is the overall reaction?
Thanks this helps