I love your style of teaching. Soo much better than my chem teacher, who introduces something to us, barely explains, and expects us to be able to take a quiz on it the next day. >.>
You just explained something to me in 7 minutes that I would have not understood had my chemistry teacher taught it to me. It was very helpful, thank you!
my ap bio teacher made us watch your videos as assignments and i'm still using your videos for years later in my college courses... you have helped me in my journey as a science major tremendously!! thank you.
You literally make everything so clear! Im currently studying for the MCAT and your videos have made the process so much smoother! Thank you Mr Anderson!
3:17 am march 18, 2021 mid pandemic. Hello to the future students reading this comment. Its hard but youll learn it like he did and I did. Anyways tryna imagine life post pandemic wonder what that will be like. Anyways future student gotta go Back go studying
@@humzamuhammad2426hey, welcome to the future, the pandemic heavily damaged the very fabric of our society, yet through perseverance and a sense of community, civilisation has once again healed itself and resorted to assigning kids chemistry homework!
This goes hand in hand with the fact that when enthalpy is endothermic (delta H is greater than 0), then when it has a lot of temp it’s spontaneous (goes to the right) and when it lowers temp, it goes to the left is non spontaneous.
In any reaction where it is reversible and we have reactant and products and equilibrium is reached, if there is ever a stress factor involved like increase/ decrease temperature, increase/ decrease pressure there is going to be a new equilibrium will be established. Increasing yield by concentration when we want more product we raise the concentration of the reactants to shift reaction towards the right and vice versa.
Thanks so much! I have a chem test on this stuff tomorrow and I'm racking my brain over these shifting concepts. That definitely cleared things up!!!!!
Great vid sir! Just a little comment. If you're taking a test and it doesn't give you the energy flow (positive or negative) then what Mr Anderson was using there is called enthalpy. So basically, for the reversible process of turning hydrogen and nitrogen gas into ammonia, on the forward reactants side, there are 4 mol of gas while on the forward products side, there are only two, so during the process heat was released. Also, catalyst doesn't shift the equilibrium. With a one way reaction, it helps making the reaction go to completion faster. But, in a two way reaction, it makes the reaction reach equilibrium more quickly.
bozeman you should teach math from the ground up all the way to pre-calculus, i would watch that more than chemistry and biology, dont know about everybody else
Hey Great video however, with the reaction of N2O4 to 2NO2 when you increase pressure or decrease volume why would the reaction shift right first and then go to the side of fewer moles? I thought that it would shift left to reactants first and stay there till the volume would allow the product of nitrogen dioxide to form? A little confused
Holy Moly, thanks you so very much! I'm taking General Chemistry 2 in the summer and my professor just threw this on to us and expected us to know it by the next day... I salute you for making my science journey possible. THANK YOU! Also do yu have a video on how to memorize the acids/bases ?! I confuse them all..
When more of a reactant or is added, will the new equilibrium have a different Kc (equilibrium constant) than our original reaction? Or will it remain constant?
Thank you so much Mr. Anderson...this helped me greatly :D Btw, I also like your process of teaching: very straight forward, yet simple enough to apply and follow along :).
Thank you so much. For everything I am one of your fans. I wish that you enjoy your year off and keep doing this excellent thing. I could try to translate your videos to Spanish, let me know if you are okay with that!
Mr Anderson, does adding or removing solids and liquids from a reaction (which involves them) actually affect the concentrations and thus the equilibrium? One of my textbooks says that it 'does not shift the equilibrium' because you 'cannot change the concentration of a pure liquid or solid as they are 100% pure'. Another book says that it does affect the equilibrium position, which is quite different to what the first book says.
it does not affects the equilibrium as the solids and pure liquids donot change with time. they remain constant during the course of a chemical reaction.
+Tejas Chandrasekar : If in a classroom of 40 students, 10 students are asleep (and are hence 'unresponsive' or 'unreactive' to the teacher), will their removal from class make a difference to how the class is being conducted? Not much! Similarly when molecules of a solid, where the atoms cannot react much because they are bonded very tightly to each other, are removed from the reaction, it makes no significant difference. A similar argument can be made for addition of solids as well. Perhaps this blog chemistrified.wordpress.com will help you in visualizing the Le Chatelier's principle a little better. Hope it helps!
After we place a stress on the reaction (by removing/adding reactants) and allowing that reaction to come to a new equilibrium, does the new equilibrium still have the same equilibrium constant? Afterall, it is referring to the same chemical equation.
Yes, since for a given reaction, at a temperature, Kc stays the same. The only thing that changes is Q. When the equilibrium is thrown off, the value of Q will change (in other words, Q no longer equals to Kc). According to Le Chatelier's principle, the reaction will shift in the direction that restore the equation: Q = Kc.
Mr Andreson, how can I find out if a reaction is endothermic or exothermic by using Le Chatelier's principle? I've been given the reaction N_2O_4 = 2N0_2.
Not sure if you still need an answer, but I'll give it a try. Usually, if the question asks how increasing/decreasing temperature affects the equilibrium of a reaction, you will also be given the energy diagram or delta H or some qualitative measure to figure out if the reaction is endo- or exothermic. An example of qualitative measure (word description) is the beaker gets hotter or colder after a while. If exothermic, delta H < 0, the beaker will get warmer (since heat is releasing to the surrounding), reactants are higher in energy than products (meaning in the energy diagram, if energy increases on the positive y-axis, the position of reactants will be higher than that of products). If endothermic, delta H > 0, beaker will get colder (since heat or energy is absorbed from the surrounding to supply the reaction), reactants are lower in energy than products (the position of reactants will be lower than that of the products).
Guys, please help me out: Let's say the Reactants have less moles than the Products. When we decrease the pressure, why do the Reactants with FEWER MOLES move towards the Products with MORE MOLES? i don't understand... what makes the system shift to the right??
Yes, because remember, when you INCREASE the pressure - the equilibrium shifts to the side with fewer molecules of gas, basically because it can expand, produce more molecules to hit the walls of the container. If you decrease the pressure the equilibrium will move in such a way that the pressure increases again. It can do that by producing more molecules. In this case, the position of equilibrium will move towards the right-hand side of the reaction.
+metalguitar311 : let's try to think of it with a physical analogy. If we're in a room full of boys and girls looking to get married by meeting up with each other and we add more boys to the room, there is greater chance that those girls who weren't finding a match earlier may now find a better suited match and hence land up marrying. Thus, the number of couples increases, but the number of girls left single decreases. In the example you've stated, treat NH3 like the couples (increases), H2 like the boys (added more) and N2 like the girls (number of molecules left behind without reaction decreases). You may also perhaps understand a little better by reading up about this on my blog chemistrified.wordpress.com/2016/04/02/le-chateliers-principle/ where i've tried to explain in a little more detail. Hope this helps!
how is there more heat on the right side (ammonia) if its exothermic ? exothermic reactions lose heat, making the ammonia colder, and endothermic reactions would make the products warmer, so why would it shift to the left if theres more heat already on the reactants? Im sorry, i know you're right, im just confused
I think you swapped the concepts of exothermic and endothermic reactions. Exothermic reaction means that the reactants are higher in energy (if you look at the energy diagram), products are lower in energy, and heat is released along with the products (meaning heat is a 'product', delta H < 0, and the surrounding gains heat). If the exothermic reaction happens in a beaker, when you wrap your hand around the beaker after some time, you will feel your hand gets warmer, not colder. On the other hand, endothermic reaction means that reactants are lower in energy, products are higher in energy, and you must input energy (by increasing temperature, etc.) for the reaction to happen. In this case, heat is a 'reactant', delta H > 0, and the surrounding loses heat (as the endothermic reaction "steals" the input/surrounding heat to supply its own reaction), and you will feel the beaker gets colder. I hope this clears things up!
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I love your style of teaching. Soo much better than my chem teacher, who introduces something to us, barely explains, and expects us to be able to take a quiz on it the next day. >.>
Sounds like a lot of teachers... Very few like this guy!
Sandra Gonzalez lol, my teacher doesn't know how to teach either, to top it off we have a quiz on the same day he teaches us a new topic...
my teacher acts like were stupid when we ask questions!! im not a chemist how would i know the answer. love this guy
mine does the same but then refuses to answer questions on it or go through it again come exams.
Our*, not "Are". What english class do you have by the way?
mr Anderson we are indebted to you
Why are the best teachers always on RUclips?
You just explained something to me in 7 minutes that I would have not understood had my chemistry teacher taught it to me. It was very helpful, thank you!
my ap bio teacher made us watch your videos as assignments and i'm still using your videos for years later in my college courses... you have helped me in my journey as a science major tremendously!! thank you.
same!!
Wherever you work, Sir, whatever you get paid, you should get a raise. Thank you so much for all the efforts you put into your yt channel :-)
Bruh you just saved our LIVES!!!!!!!!!! Test today! Learned more in a five min video than 5 class periods
You literally make everything so clear! Im currently studying for the MCAT and your videos have made the process so much smoother! Thank you Mr Anderson!
Your chem videos are almost exactly in unison with my ap chem class. Thank you
jus saying eli manning best qb ever now stfu
it is Tom Brady
You explain the concepts very clearly and your animations really help in visualizing the concepts. Thank you for being such a great educator!
OMG I love this man.. I needed to know this for my chemistry lab tomorrow :D
Even in college, your videos are still as helpful as ever! Thank you so much!
thanks vro its 9pm and im doing chem hwk
3:17 am march 18, 2021 mid pandemic. Hello to the future students reading this comment. Its hard but youll learn it like he did and I did. Anyways tryna imagine life post pandemic wonder what that will be like. Anyways future student gotta go
Back go studying
@@humzamuhammad2426hey, welcome to the future, the pandemic heavily damaged the very fabric of our society, yet through perseverance and a sense of community, civilisation has once again healed itself and resorted to assigning kids chemistry homework!
When you showed the actual implications with percent yields that made it all so much more clear.
you are among the best teachers for ever
This video from when I was still in 5th grade is now very usefull. Thank you very much 💗
This goes hand in hand with the fact that when enthalpy is endothermic (delta H is greater than 0), then when it has a lot of temp it’s spontaneous (goes to the right) and when it lowers temp, it goes to the left is non spontaneous.
Thank you man. I hadn't understood this in more than two years. Thank you *cries*
In any reaction where it is reversible and we have reactant and products and equilibrium is reached, if there is ever a stress factor involved like increase/ decrease temperature, increase/ decrease pressure there is going to be a new equilibrium will be established. Increasing yield by concentration when we want more product we raise the concentration of the reactants to shift reaction towards the right and vice versa.
this is my new favourite channel.
Saving my life all the way from High School Ap Bio up until now in Chem 2 in college...thx chief.
I enjoyed you video. You explained the topic simply and thoroughly. Thank You.
We’re deeply grateful for your help
Thank You, the visual diagrams help a lot. It actually makes sense.
oh my God this is awesome everything start to click. i have been stuck on this for a week and thats studying it everyday
You're the best! Thank you for making this video and the other chemistry and biology videos. They're all very helpful!
simple and straight foward. i only know of the temp and pressure part. knowing the concentration helps also.
Thank you, Mr. Anderson. Always helpful, since AP Bio to General Chemistry 1 & 2.
Thanks so much! I have a chem test on this stuff tomorrow and I'm racking my brain over these shifting concepts. That definitely cleared things up!!!!!
I think I now know how to make my slides. Thanks Mr Anderson
I like your channel and you have been a tremendous help in my success. Please continue on. Thank you!
THANKS SO MUCH! I was so confused. i take AP Chemistry and i was so confused about Le Chatelier. Thanks for spelling it out for me.
Great vid sir!
Just a little comment. If you're taking a test and it doesn't give you the energy flow (positive or negative) then what Mr Anderson was using there is called enthalpy. So basically, for the reversible process of turning hydrogen and nitrogen gas into ammonia, on the forward reactants side, there are 4 mol of gas while on the forward products side, there are only two, so during the process heat was released.
Also, catalyst doesn't shift the equilibrium. With a one way reaction, it helps making the reaction go to completion faster. But, in a two way reaction, it makes the reaction reach equilibrium more quickly.
@Anuveer Saini [Student] Hey, are you talking about the catalyst or enthalpy?
Max Nguyen I’m talking about the Enthalpy. Is it always exothermic if there are less moles on the product side than the reactant side? Let me know.
@@anuveersaini7860 Hey, Yes.
Max Nguyen and that only applies to gases, right?
@@anuveersaini7860 Hey, yes :D
Keep going
I wished all our doctor like you 😪
Very easy to follow, thank you!!!
bozeman you should teach math from the ground up all the way to pre-calculus, i would watch that more than chemistry and biology, dont know about everybody else
Thank you so much all your lectures are really helpful.
I should have watched this 5 years ago, thank you for the help.
You are so good. Such great explanations. Love it
Wah! Wonderfully explained! Thank you very very much!
This helped me so much! you explain everything so well! thank you!
Thank you so much for a wonderful lecture.
Wow sir !!!! impressive teaching style ☺tq sir
Hey Great video however, with the reaction of N2O4 to 2NO2 when you increase pressure or decrease volume why would the reaction shift right first and then go to the side of fewer moles? I thought that it would shift left to reactants first and stay there till the volume would allow the product of nitrogen dioxide to form? A little confused
I love your videos so much. Thank you!
Far superior than my professor's explanation.
Thank you SO much! This video was super helpful!
thank you , i learned a lot :D I couldn't understand to my teacher, so I found you, and it was AWESOME! ;D
your the reason I understand chem... thank you so much
But you don't understand english!!!! You're* ezpz
This was very helpful you did such a great job at explaining it thank you so much!
Holy Moly, thanks you so very much! I'm taking General Chemistry 2 in the summer and my professor just threw this on to us and expected us to know it by the next day... I salute you for making my science journey possible. THANK YOU! Also do yu have a video on how to memorize the acids/bases ?! I confuse them all..
Navneet Kaur there are others but I don't think he has one
lol, thank you for your reply. i actually understand it now and i passed my chem 2. now taking organic chemistry. FUN STUFF!
wow! How is it going one year later?? Hopefully well :)
When more of a reactant or is added, will the new equilibrium have a different Kc (equilibrium constant) than our original reaction? Or will it remain constant?
Kc depends on Temperature
Perfect explanation :) Thanks a million
Any videos explaining how to determine Q#'s of different elements? Thank you Mr. Anderson for being super duper awesome! :)
thank u so much sir love ur way of teaching
this was life changing. thanks a lot
My teacher should not be teaching chemistry so thank you for this video !!!!
Thank you so much Mr. Anderson...this helped me greatly :D
Btw, I also like your process of teaching: very straight forward, yet simple enough to apply and follow along :).
Thank you so much. For everything I am one of your fans. I wish that you enjoy your year off and keep doing this excellent thing. I could try to translate your videos to Spanish,
let me know if you are okay with that!
Thank you, this was so helpful!
Mr Anderson, does adding or removing solids and liquids from a reaction (which involves them) actually affect the concentrations and thus the equilibrium?
One of my textbooks says that it 'does not shift the equilibrium' because you 'cannot change the concentration of a pure liquid or solid as they are 100% pure'.
Another book says that it does affect the equilibrium position, which is quite different to what the first book says.
it does not affects the equilibrium as the solids and pure liquids donot change with time. they remain constant during the course of a chemical reaction.
+Tejas Chandrasekar : If in a classroom of 40 students, 10 students are asleep (and are hence 'unresponsive' or 'unreactive' to the teacher), will their removal from class make a difference to how the class is being conducted? Not much! Similarly when molecules of a solid, where the atoms cannot react much because they are bonded very tightly to each other, are removed from the reaction, it makes no significant difference. A similar argument can be made for addition of solids as well.
Perhaps this blog chemistrified.wordpress.com will help you in visualizing the Le Chatelier's principle a little better. Hope it helps!
@@tejasshyam Already understood the concept but still like your example :D
Thank you, this was very helpful.
how can I ask you questions mr anderson about other topics that you haven't yet uploaded videos about 'em
Wow. This video is amazing.
To all the chemistry god's you are one of the best.
Anyone here cause all there classes are online now?
OG_DanTheMan literally me taking notes on this for my Chem class rn
Loved the video..Thanks Sir!!
Great video. Thank you.
this was so helpful. thanks.
After we place a stress on the reaction (by removing/adding reactants) and allowing that reaction to come to a new equilibrium, does the new equilibrium still have the same equilibrium constant? Afterall, it is referring to the same chemical equation.
Yes, since for a given reaction, at a temperature, Kc stays the same. The only thing that changes is Q. When the equilibrium is thrown off, the value of Q will change (in other words, Q no longer equals to Kc). According to Le Chatelier's principle, the reaction will shift in the direction that restore the equation: Q = Kc.
Wish you made all these videos last year :(
Am I the only one here who has a great AP Chem teacher?
I had a good one
Sir, You are the best. Regards from India. My Chemistry teacher sucks !!!! :D
Great explanation
Could you add examples of application that would have been helpful. Thanks
about to take my ap chem exam! thank you!!
Is the value of K in the new equilibrium going to be the same for the same temperature, or will there be a new K value?
Thank you so much!
Your stuff is good for the general concept but i think it would be more effective if you showed difficult examples. Good video though
Thanks for saving me. My chemistry teacher wont even know this..
Are you using Lemay's textbook?
Yes.
Mr Andreson, how can I find out if a reaction is endothermic or exothermic by using Le Chatelier's principle? I've been given the reaction N_2O_4 = 2N0_2.
Not sure if you still need an answer, but I'll give it a try. Usually, if the question asks how increasing/decreasing temperature affects the equilibrium of a reaction, you will also be given the energy diagram or delta H or some qualitative measure to figure out if the reaction is endo- or exothermic. An example of qualitative measure (word description) is the beaker gets hotter or colder after a while. If exothermic, delta H < 0, the beaker will get warmer (since heat is releasing to the surrounding), reactants are higher in energy than products (meaning in the energy diagram, if energy increases on the positive y-axis, the position of reactants will be higher than that of products). If endothermic, delta H > 0, beaker will get colder (since heat or energy is absorbed from the surrounding to supply the reaction), reactants are lower in energy than products (the position of reactants will be lower than that of the products).
This basically saved my whole exam
great video
i literally thought of creating a second account to like it twice
Guys, please help me out:
Let's say the Reactants have less moles than the Products. When we decrease the pressure, why do the Reactants with FEWER MOLES move towards the Products with MORE MOLES? i don't understand... what makes the system shift to the right??
Yes, because remember, when you INCREASE the pressure - the equilibrium shifts to the side with fewer molecules of gas, basically because it can expand, produce more molecules to hit the walls of the container. If you decrease the pressure the equilibrium will move in such a way that the pressure increases again. It can do that by producing more molecules. In this case, the position of equilibrium will move towards the right-hand side of the reaction.
It was helpful, thank you...
If you add more H2, I get why the NH3 would increase to balance, but why does the N2 need to change?
+metalguitar311 : let's try to think of it with a physical analogy. If we're in a room full of boys and girls looking to get married by meeting up with each other and we add more boys to the room, there is greater chance that those girls who weren't finding a match earlier may now find a better suited match and hence land up marrying. Thus, the number of couples increases, but the number of girls left single decreases. In the example you've stated, treat NH3 like the couples (increases), H2 like the boys (added more) and N2 like the girls (number of molecules left behind without reaction decreases). You may also perhaps understand a little better by reading up about this on my blog chemistrified.wordpress.com/2016/04/02/le-chateliers-principle/ where i've tried to explain in a little more detail. Hope this helps!
Thanks :D Really love the video you made :) I survived CHEMISTRY ;D
You are an angel
You are great! Thanks
that's helpful❤
does anyone know what table is he using ?
So helpful...... Thank you
how is there more heat on the right side (ammonia) if its exothermic ? exothermic reactions lose heat, making the ammonia colder, and endothermic reactions would make the products warmer, so why would it shift to the left if theres more heat already on the reactants?
Im sorry, i know you're right, im just confused
I think you swapped the concepts of exothermic and endothermic reactions. Exothermic reaction means that the reactants are higher in energy (if you look at the energy diagram), products are lower in energy, and heat is released along with the products (meaning heat is a 'product', delta H < 0, and the surrounding gains heat). If the exothermic reaction happens in a beaker, when you wrap your hand around the beaker after some time, you will feel your hand gets warmer, not colder. On the other hand, endothermic reaction means that reactants are lower in energy, products are higher in energy, and you must input energy (by increasing temperature, etc.) for the reaction to happen. In this case, heat is a 'reactant', delta H > 0, and the surrounding loses heat (as the endothermic reaction "steals" the input/surrounding heat to supply its own reaction), and you will feel the beaker gets colder. I hope this clears things up!
good video!
Thnk you for helping me pass gen chem
Really noice video thank you.
amazing!! thanks a lot!!!
What is opening song?
Alexandra Backfisch darude sandstorm