It depends on the question. So if the REACTANTS turning into PRODUCT is an endothermic reaction then adding heat will shift it towards the right(because the reactants require heat to react) BUT if the PRODUCT turning back into the REACTANT is endothermic that means adding heat will shift it to the left (because the products require heat to form back into the original reactants)
This is by far the greatest explanation of this principle. Instead of just saying it moves to the left or right, you explained the conceptual reasoning behind it...for me, it makes it a hell of a world of difference. Thanks again, and keep it up!
Never would I have thought that something that caused me so much pain and turmoil could make complete sense after 8min from a random stranger on the internet..... God speed my friend.....
Just taking a moment to appreciate you and your work. You have literally answered all my questions and relieved all my doubts from the beginning of high school to the end of my university path. I could never thank you enough.
This video is by far the best and more clear explanation. After watching several videos and becoming even more confused; I now fully understand the concept of equilibrium and what side it favours depending on the change. Thank you
English isn't even my mother tongue, but this helped me a lot more than any other video I saw! Your way to explain things is awesome, thank you very much :)
if only my teacher could teach as well as you could, my whole class would have covered the whole curriculum in two weeks - with room to spare! But no .. teachers these days are so lazy and only know to read from the textbook.
This is so helpful! I've been studying for 2 weeks for my chemistry final and a problem like this appeared in the final packet. You explain chemistry very simple that is easy to follow, thanks!
This video is by far the most amazing one I've seen on Le Chatelier's principle. Thank you so much for all the great reasonings and explanations. I was having some issues with the change in temperature part but you made it all very clear to me. Thank you so much sir, you're a great teacher!
more product was produced during equilibrium of the reaction so it needs to shift to reactants to offset the production of products. i know this is a old question but just incase someone else was wondering.
this helped a lot, i have been having A LOT of struggle with my chemistry class this year and this is gonna help me for my test coming up, thank you :)
Thank you for this helpful explanation! I've watched so many other videos, read my textbook on this concept and I didn't fully understand it until now.
Dear Sir, this is my first time to write a comment on any RU-vid video. First of all, I would say I like your method of teaching, knowledgeable, clear and to the point. Secondly, I would like to correct your understanding of adding inert into the system. When we add inerts into reactor at constant system pressure, the partial pressure of reacting species decreases and as a result we get few moles of ammonia on the product side. For reference, I would suggest reading Sandler, S. (2006). Chemical, biochemical, and engineering thermodynamics, chapter 13, pp 720-722. Further, I have also simulated the case study of production of ammonia by adding inert material into the system using a process simulator. My results are in agreement with the book i.e. decrease in formation of ammonia by adding an inert material or dilutent at constant system pressure. Thanks.
I love your videos, you're helping me pass Chem 2, so thank you so much!!! But as a double major (with French) I'd have to say I'm pretty sure its pronounced as Shat-lee-A, not Shat-uh-lee-A, or even pronouncing the first E in Chatelier at all. Regardless, you're the man, thank you so much. Just got distracted by that that and had to mention it. Keep up the awesome work, hundreds of chemistry grades depend on it!
