thank you so much! helped immensely. you don't even understand how much it did! You are very thorough with every step thank you again from the bottom of my heart!!!
@vegassDJ I just watched it. Although I generally don't like hearing the sound of my own voice, it sounds particularly awful here. I think i may have been sick that day. Thanks for the suggestion!
shouldn't the observes rate law be k [H2]^2 [NO]^2 ? If so, the derived rate law of k_2 [H2] [NO]^2 isn't consistent because the ^2 is absent from the [H] concentration
Thank you alot :) It really helped me, I have asked a question but there is no one could answer me clealy which is " Whats does K rate constant exactly represent??" I hope Yours or any one answer me. And thank you in advance .
this is called the steady-state approximation, right? thank you so much for your videos!! keep them going because they really help me. you teach way better than my professors :)
Hi ! Your video really helped a lot (: However I was hoping you could clarify a question I have - why is it that for the intermediate steps , the powers of the reactants are the same as the coefficients, but when we are looking at the overall balanced equation the powers for the initial reactants are not necessarily the same as the coefficients . I hope my question doesn't confuse you ! ): sorry and thanks a bunch (:
for my problem I had to find the overall chemical equation and a rate was given to me. How would I determine if the reaction mechanism is scientifically valid? Or is there a vid I can watch?
i have a mechanism that is Cl2(g) (equilibrium arrows) 2Cl(g) (and other steps) I need Cl by itself as the intermediate for another step... i end up with k1/k-1[Cl2]=[Cl]^2 .... How can I get Cl by itself to put it into rate2=k3[Cl][CHCl] where Cl is the intermediate in the equation
Thank you very much for explaining this. It was the exact example from the ebbing book and was having issues with it. They really can't explain shit in that book. I think they try to make it seem complex for job security... this is just high school algebra with elements, at best. Cheers.
nevermind, i see what i did wrong. i used the coefficient of a non-elementary reaction as an exponent. H2 is unimolecular, so its exponent should be 1, not 2 (its coefficient)
The world needs more teachers like you...love how you stated the conditions and explained it, such clarity is seriously lacking in schools today.
A decade later, you're still making students feel much better about exam topics. Props to you!!!
Thanks for your kind words, and thanks for watching! 😀
Explained it waay better than my AP chem teacher...Thanks!
thank you so much! helped immensely. you don't even understand how much it did! You are very thorough with every step thank you again from the bottom of my heart!!!
Hello!
The world needs more people like you. Thanks for the videos.
Explained way better than my chem prof... have an exam in 2 days!!! thank you so much!!!!
you are not a hero you are the hero. god bless you, my brother
So, I just watched all the videos in your "Chemical Kinetics" playlist........Thank You! I understand this stuff waaaay more now! Thank you!!!!!!!!!
Watched the entire chem kinetics playlist... understand it now great job and thanks
Are the steps always given? If not, how can you determine by yourself when the step is fast or slow? Thank you.
@vegassDJ I just watched it. Although I generally don't like hearing the sound of my own voice, it sounds particularly awful here. I think i may have been sick that day. Thanks for the suggestion!
Even after 6 years, this is helpful. Thank you :)
Must a fast first elementary reaction be an equilibrium one? Could you have a full forward arrow on the first fast rxn?
I'm glad I watched this before my university chem 2 final otherwise I don't think I would have ever learned it as well.
This was so helpful! Thank you so much for your help. I love the step by step explanation. I can't thank you enough!! :D
Wait why isn’t the [H2] squared in the final rate equation if the H2 in the overall equation has a 2 coefficient?
That only applies to ELEMENTARY reactions (reactions with only one step). If you have a multi-step reaction, it is a different story.
very helpful, thank you!!!
You're very welcome! Many thanks for watching and commenting 😀
Thanks for helping me lessen my chances of failing my Chem 115 midterm tomorrow
Is this the pre-equilibrium method?
Thank you so much! You teach better than my AP Chem. teacher!
I am here in may 25 2024.......from Ethiopia
great videos!!!! your videos should get wayyyy more views, trust me they are really helpful
Thank you so much! This was incredibly helpful
Great video! Very helpful and explained the concepts well. Thank you!
shouldn't the observes rate law be k [H2]^2 [NO]^2 ? If so, the derived rate law of
k_2 [H2] [NO]^2 isn't consistent because the ^2 is absent from the [H] concentration
An amazing explanation, thank you.
You're very welcome! 😃
That was very helpful! I wish my teacher had said this.
Thank you alot :) It really helped me, I have asked a question but there is no one could answer me clealy which is " Whats does K rate constant exactly represent??" I hope Yours or any one answer me. And thank you in advance .
You're a boss. 'Meek Mill - I'm a Boss (Ft. Rick Ross)' Is now the theme tune to your life.
this video helped me a lot. thanks
You are a genius bro. Keep up the good work
This helped a lot. Thank you very much.
You're very welcome! Many thanks for watching and commenting 😀
BLESS YOUR SOUL. SAVED MY LIFE
thank you so much! i have a final coming up and this was so helpful
Dude this is amazing thank you so much brother!
You're very welcome! Thanks for your kind words 😀
Thank You
You're very welcome! Many thanks for watching and commenting 😀
thank you so much it was so confusing but it's clear now to me
this is called the steady-state approximation, right? thank you so much for your videos!! keep them going because they really help me. you teach way better than my professors :)
I'm really grateful for the help. Thank you!
thanks for the video and help! this video was very clear and went step by step!
Hi ! Your video really helped a lot (:
However I was hoping you could clarify a question I have - why is it that for the intermediate steps , the powers of the reactants are the same as the coefficients, but when we are looking at the overall balanced equation the powers for the initial reactants are not necessarily the same as the coefficients . I hope my question doesn't confuse you ! ): sorry and thanks a bunch (:
That was sooooo cleaaaaarrrr and easy to understand!!!
Thanks, it helped me a lot👍👍👍👍
You're very welcome!
Thank you very much...very usefull videos !
thank you so much. you are awesome teacher.
hi! why is it that k-3 is usually ignored?
That was beautifully done. Thank you
for my problem I had to find the overall chemical equation and a rate was given to me. How would I determine if the reaction mechanism is scientifically valid? Or is there a vid I can watch?
So helpful thank you
thank you! amazing!
REALLY helpful! Thanks a lot, brother. Best wishes and God bless :)
can you explain more in detail why the [NO] is squared?
Reviewing for my AP chem test lol thank you so much
thank u very much helped a ton
great video, thanks
Very helpful
So helpful, thank you so much!
i have a mechanism that is Cl2(g) (equilibrium arrows) 2Cl(g) (and other steps) I need Cl by itself as the intermediate for another step... i end up with k1/k-1[Cl2]=[Cl]^2 .... How can I get Cl by itself to put it into rate2=k3[Cl][CHCl] where Cl is the intermediate in the equation
that was an amazing vid dude. thanks
Thank you very much for explaining this. It was the exact example from the ebbing book and was having issues with it. They really can't explain shit in that book. I think they try to make it seem complex for job security... this is just high school algebra with elements, at best.
Cheers.
excellant video thank you!
-Khalissi
But since k1 is equal to k-1, since equilibrium can't you just cancel the division since it would be equal to one???
Thanks a lot!!!! Really helpful
That was a great help, thx!
Wow, great video dude.
thanks from nepal!!!!
10 billion % helpful
Very cool!
THANK YOU SO MUCH
So helpful!! Thanks so much!
God bless you
Life-saver!!!!!!!!!
Thank you so much for this!
Love you man
That helped me SO much omg!
Thanks alot!!!
thanks twin
This is exactly what I needed! thanks! :-D
Thank. You. Very. Much.
Amazing thanks
Thank you so much!
how about the 2 h2? why didn't you account for k3?
helpful, thanks
thank you ben
This was amazing.
You just made something that put me on my ass yesterday seem so simple in 10 minutes. You are a God.
excellent!!!
how we will come to know that which reaction is fast or slow
DDH channel
Give your Mom for the answer
I think they are usually given to you during the test or quiz. If its not, you probably have to determine it experimentally.
how do you determine which is K1 K2 K3?
why Didn't you write k3 and k2 in the expression?
Since k is equal and opposite k-1 can't you just simplify (k1/k-1) to a negative sign?
In that first step, k_1 is not equal to k_-1. Rather k_1 * [NO]^2 = k_-1 * [N_2O_2].
@@BensChemVideos Thanks!
@@alexawermuth558 you bet! Thank you for watching and asking a question!
Thanks sir
nevermind, i see what i did wrong. i used the coefficient of a non-elementary reaction as an exponent. H2 is unimolecular, so its exponent should be 1, not 2 (its coefficient)
why isnt k3 used?
You didn't account for the consumption of N2O2 in step 2...
Thanks bruv
You're very welcome! Thanks for watching! 😀
At 3:18, how did you know that the k was k2??
AWESOME!
Thankyou so much :))
Fantastisch!
:) Great help
what about third step???