4.3. Chemical Kinetics

[@lonelymoon000]

Informative at its best. Try to include 0:00 so that the timestamps can be included as chapters inside the video. ------ OUTLINE 0:00 Introduction 4:19 Reaction rates 11:00 Rate law 13:02 Determining the rate law: isolation method 20:28 Determining the rate law: integrated rate laws 31:02 Half-life 53:23 Collision Theory 1:01:49 Transition-State Theory 1:05:43 Effect of temperature on reaction rates: the Arrhenius equation 1:11:20 Reaction mechanisms 1:19:02 Pre-equilibrium method 1:21:26 Steady-state approximation 1:31:21 Special mechanisms: Lindemann mechanism 1:39:51 Special mechanisms: Radical chain mechanisms

[@johnr4906]

I watched all you videos and got an A in Physical chem one, thank you.

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[@joeloduntan]

❤️

[@carloconstantino4762]

Where have you been all my life. This is one of the best explanations i have seen for chemical kinetics

[@KostyaGL]

The best explanation of kinetics I've seen, thank you so much

[@MrsLoolis]

Your lecture was extremely helpful and great made. Thanks :) Greetings from Poland!

[@arijitdutta5573]

I was just impressed with the way you have tought..Please upload more videos..Love your videos very much.

[@DavidEssien-nn7qb]

I love your voice. It's pretty nice and clear. I love your video too. Thank you for sharing your knowledge

[@momodoukasowe3832]

Thanks for the lecture. Watching all the way from The Gambia.

[@Gero_Nimo123]

Thank for your lecture videos. Very helpful in reviewing for licensure examination. I am now a licensed chemist here in the Philippines.

[@muhindojimmy8552]

Thanks alot madam....Sarah..i really appreciate ur effort towards enlighting my knowledge on chemical kinetics. May God bless you abundantly.....

[@wendychen4452]

These videos all are very useful and helpful, could you please upload more videos. Thanks!

[@wy2894]

This is really helpful! Thank you very much Sarah!

[@ammarparmr]

Fantastic lectures Well explained They are impressive and when I'd knew that there are made 4 years ago with this quality, I did not find a proper word to describe it. Thank you so much You're an excellent tutor You don't just have knowledge, you know how to deliver it as well 👏👏

[@Faendal91]

Do you have any videos using the Michaelis Mention theory to confirm enzyme kinetics? Great video btw!

[@sodaikabiodun2793]

I cant thank you enough. You just made my life simple

[@James-Pookulathel]

You are the boss Ma'am.....Thank you so much.....

[@AMITKUMAR-nf8in]

wow... it was very good... why have u stopped making videos?

[@muhindojimmy8552]

How do u generally obtain R² in determining the order of reaction....

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Thank you very much, your videos are helping me so much!

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[@MbekezeliKubheka]

hey can you please add videos explaining first order parallel reactions

[@caesarwiratama3303]

Very nice and clear explanation. Thanks a lot

[@mohammedabudaqqa8385]

WOW! what a great explanation! many thanks to you for these great videos 😍

[@amilawanasinghe7107]

Thanks a lot for the nice and simple explanations! :)

[@mimic5121]

Thank you... you're a life saver.

[@cdorman11]

'Kay?

[@konstantinosdivanis4213]

Excellent lesson!Thank you very much

[@kipmaru4290]

Please a lecture on rheology

[@PankajKumar-xh6oq]

Really that's awesome to learn from you ... applaud you 👍

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we need more of your videos, please

[@pegaseii]

Thank you for this! ♥

[@kishorekumarr6569]

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[@tomon7605]

Great and friendly lecture for non-native speaker of English. Many thanks.

[@thewhitelotus7667]

Thank you!

[@PankajKumar-xh6oq]

Mam .. is there any video of you on exothermic and endothermic reaction

[@thefarellanalysis3496]

You are one hell of a damsel, beauty and brains, quite hard to find these days 😊

[@mainestate727]

Thank you very much maám! Nice Explainations.

[@sizweduba328]

for the second order integrated law isn't suppose to be 1/[A]t=Kt - 1/[A]o

[@waedsarmigo2123]

Thank you it's very useful Put more videos about physical chemistry 2 please

[@sjjadmortdha5889]

هل يمكن تحويل الترجمة للغة العربية رجاءاً

[@marvellnelson9141]

Dont understand where you have y= - 0.0076 where did this number came from? help, please.

[@mihip619]

Yeah don't understand it either. When I calculate the slope I get -0.00389. Not sure what I'm doing wrong?

[@hariwpedits1526]

4 yrs ago ?

[@htv5485]

legendary...

[@boat7944]

29:15 maybe kdt(not kt)?

[@SarahMaySibugTorres]

Oops, my mistake! Yes, it should be dt! I think mentally I got ahead of myself and had the integrated form in mind :) Thanks very much for pointing this out :)

[@reanchern7]

Love your lectures. Will there be more coming?

[@hazratullahhisham]

please make more videos

[@stimulantdaimamld2099]

great

[@md.morshedurrahman5940]

Excellent lecture. Thank you

[@zephaniahgreenwell8151]

"Kay..."

[@ntombiyomuzinyathi5731]

Hey Sarah under steady state approx why did you choose HOCL as the intermediate why not HOI or H2O as the intermediates or why not write all of them and say there are 2 intermediates and 1 catalyst also, when writing the rate expression when not told which one is the slow step are we supposed to write any expression in which the intermediate is involved

[@SarahMaySibugTorres]

Hello! Good question! Based on Problem 4.3.4., Step 2 was given as the "slow" or rate determining step, so we wrote down the rate of that step as the overall reaction rate. It just so happens that HOCl is the only intermediate that appears in the reaction rate expression, so we did a steady-state approximation to solve for an expression for HOCl. We could have also written a steady-state approximation expression for the other intermediates, but that for HOCl is the most useful for us in the problem. Alternatively for a more general approach... if we don't know which is the slow step, we can write down the rate of the reaction in more general terms, like the concentration change of product with time, either Cl- or OI- (or we can write it in terms of reactant too, but add a negative sign). If we use Cl-, we get: (eq. 1) Rate = d[Cl-]/dt= k2[I-][HOCl] (same if we knew that step 2 was the slowest step!) OR, if we use OI-, we get: (eq. 2) Rate= d[OI-]/dt=k3[HOI][OH-] - k-3[OI-] (note that we're assuming H2O is in very large excess, so its concentration is considered to be more or less constant) If we use the rate of OI-, we'll have to write the steady state approximation for HOI since it appears in the expression. Interestingly, if we plug an expression for HOI into eq. 2, it just simplifies to eq. 1. So using the change in concentration of either product with time as the overall rate of reaction should yield the same results. I hope this helps! :)

[@pawankumar-ng8du]

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[@tantntn2813]

OK

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[@Stardusk.]

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[@Stardusk.]

As a man before your machine with aditions, and functions while declines of your bad tooling. The machine is only as good as the machiner. Organic before mechanical. Your failures coming to whisper in your ear. Thanks girl stem person thing for this video. Try weaker.

[@esoto1386]

thank you!