Great video! It is a bit misleading at the very end though. As mentioned, reactions will shift the exothermic direction when cooled and the endothermic direction when heated, but this does NOT always mean it will shift left for exo and right for endo. This one does because the forward reaction is endothermic.
Does this apply only if there is enough limiting reactant available to form more product? Or does the principle itself imply that there is always available reactant because there is always product being decomposed? In a sense, making the concept of "limiting" reactant null?
When there is a reversible reaction in equilibrium, you don't have to worry about the concept of limiting reactant as the reaction won't go to completion anyway.
Love the vid, but aren’t the endo/exo directions reversed here? You apply thermal energy, so in order for the solution to cool down, shouldn’t it go in the exothermic direction? Exothermic means to release thermal energy. Isn’t that how it would cool down…and Vice versa, if it’s cooled it needs thermal energy so it should go in the endothermic direction?
Releasing thermal energy means that the surroundings (which include the water that the chemicals are dissolved in) warms up. So if a reaction goes in the exothermic direction, the surroundings warm up. Endothermic reactions take in thermal energy (and, importantly, change it into chemical energy, which we cannot actually measure) from the surroundings, so the surroundings cool down. So if I heat up a reversible reaction, it tries to oppose that - thermal energy is taken from the solution I am heating and converted into chemical energy - that is an andothermic reaction.
@@richardhiggins6471 We are in agreement. At least to me, we’re saying the same thing. I think the frame of reference regarding the expressions “it tries to cool down” and, “it tries to warm up” is the cause of confusion. What the “it” is is the crux of the issue. I took the “it” to mean the reaction and not the environment…so if the reaction is trying to “cool down”, it would do so by moving in the direction that would release energy, thus exhibit an exothermic process. Do I have this wrong?
So if we put the test tube in a hot bath(adding heat) and the reaction turned blue that means that the heat was added as a reactant(endothermic) meaning too much reactant now, so it needs to shift to the right to get rid of the excess reactant and rebranded? Or am I looking at this wrong? Or does this mean since it's shifting the heat from reactant side to the product side it is technically getting rid of the heat(cooling down). A separate question- does that mean a reaction can be exothemic and endothermic depending on if you are adding heat or taking away heat? I feel like my teacher made it seem that a reaction can be 1 or the other.
You can think of heat as a reactant (not technically correct, but it works as a way of predicting what happens to the equilibrium). Add heat, the equilibrium shifts to reduce the heat but going in the endothermic direction. In answer to your second question, no. You can add heat to any reaction, whether it is exo- or endothermic. The most important thing about a reversible reaction is, if it is exothermic in one direction, it is endothermic in the other.
HELP, question: I'm looking for a reaction where you start with color (any color is ok) and after a certain time, it becomes colorless. If possible I would like to do it with non-harmful chemicals, because it's going to be an experiment for primary school kids. -Start with a color (already set up in the container, if possible use non-harmful chemicals or natural products) -Add H2O and it becomes colorless -If possible, change the time it takes to become colorless based on the concentration of the initial chemicals/products -Use natural products or non-harmful chemicals, as it is an experiment for kids, primary school students. Thank you very much.
When we say "an endothermic reaction takes heat in", what we really mean is " an endothermic reaction takes heat energy from the surroundings (which includes the water that the chemicals are dissolved in) and changes it into chemical energy that is stored in the products. By changing heat energy into chemical energy, the system cools down.
You are not dumb - that was a very intelligent question showing that you are thinking about the topic, rather than just accepting something you have read or heard. I had to answer exactly the same question with my Year 12 class yesterday. This is an A level topic as well as GCSE, so it is considered to be a difficult subject to get your head around.
The fumes from concentrated HCl are unpleasant and in an ideal world I would have done it in a fume cupboard, but it would have been much harder to film and you wouldn't have heard me speak over the noise of the extractor fan!
ahaha all other vids just say "equilibrium shifts to left/right", without explaining what this means. only explanation ive seen which wasn't a waste of time
Its a reversible reaction, so there is no one product but instead there are two, one will be from the exothermic side and one from the endothermic side, they are producing the product at the same rate hence you don't see a constant color change and the two products will be COCl4 and CO(H2O)6, so basically the one in the center is a mixture of the two PS: I hope I am right, this is what I have learnt so far
@@richardhiggins6471 hey ,i am so sorry for asking but I have a chem 30 lab report due in 4 hours and I need the materials used in this in exact or close quantity. Can you please help me?
@@okiedokie4582 I cannot recall exact amounts, but it was one spatula of hydrated cobalt chloride (check the Hazcard about this) dissolved in the absolute minimum of distilled water (maybe 2-3 ml, a saturated solution). Then, to get the purple mixture in the middle I added concentrated hydrochloric acid (corrosive) drppwise from a pipette until I achieved the purple colour.
No-one forced you to watch it, did they? If you already understand it, brilliant, and if you don't, well, some people enjoy learning and understanding stuff.
![Baby Kia - GLOVES & DRACS (BLACK AF1s) [Official Music Video]](http://i.ytimg.com/vi/ajm8LeB0qQk/mqdefault.jpg)
this is a must watch video for those who are studying this concept.
i agree
definetly
Great video! It is a bit misleading at the very end though. As mentioned, reactions will shift the exothermic direction when cooled and the endothermic direction when heated, but this does NOT always mean it will shift left for exo and right for endo. This one does because the forward reaction is endothermic.
This is so helpful and actually helped me understand the concept better! Thank you so much!!!
Thank you, sir! Sadly, our teacher didn't show us the chatelier principle irl, so it was hard to understand the concept. You've saved a life!
ur videos are way more informative than all the others i've come across!!!!!!
this explains the concept so well, thank you!
Great !! You made me this concept clear through your practical
thank you so much for this.. really helpful for students like me who have no access to a school laboratory during online classes :)
What a GREAT video! I had such a hard time reading the concept and seeing this makes it so clear. Thank you!
informative video, well explained, and to make everything perfect the nice deep voice.
Thanks a lot !
Best demonstration! 🌷❤️
a big thumbs up for you... i understood really clearly now with thehelp of experiments
thanks a lot sir!
Mrs. Crosby sent me here, very cool and educational, had super fun with this video
Nice demonstration 👍🙏
so glad i stumbled across this, in y11 my chem teacher is so bad and this is perfect to finally understand
Super!
thanks!
im helping my brother out but I had no clue what it's principle was!
Thanks man
Thanks a lot.
You are welcome.
Hey what an excellent demonstration! :)
Great one, I understand it very well 😊😊
Very helpful! Thanks!
❤
Who puts a dislike to this video?? It's very nicely made and narrated and to the point.
Thankyou so muchh sir it war really really helpfull
LOVE THIS VIDEO ❤❤❤❤
I can't believe, the way ur explained.
Not all heros wear capes
fantastic
thank you. i finally understood.
Best video ever!
I really love this video. Thanks a lot sir!
this makes so much sense
thank you sir🫡
Decent vid!
Does this apply only if there is enough limiting reactant available to form more product? Or does the principle itself imply that there is always available reactant because there is always product being decomposed? In a sense, making the concept of "limiting" reactant null?
When there is a reversible reaction in equilibrium, you don't have to worry about the concept of limiting reactant as the reaction won't go to completion anyway.
Love the vid, but aren’t the endo/exo directions reversed here? You apply thermal energy, so in order for the solution to cool down, shouldn’t it go in the exothermic direction? Exothermic means to release thermal energy. Isn’t that how it would cool down…and Vice versa, if it’s cooled it needs thermal energy so it should go in the endothermic direction?
Releasing thermal energy means that the surroundings (which include the water that the chemicals are dissolved in) warms up. So if a reaction goes in the exothermic direction, the surroundings warm up. Endothermic reactions take in thermal energy (and, importantly, change it into chemical energy, which we cannot actually measure) from the surroundings, so the surroundings cool down. So if I heat up a reversible reaction, it tries to oppose that - thermal energy is taken from the solution I am heating and converted into chemical energy - that is an andothermic reaction.
@@richardhiggins6471 We are in agreement. At least to me, we’re saying the same thing. I think the frame of reference regarding the expressions “it tries to cool down” and, “it tries to warm up” is the cause of confusion. What the “it” is is the crux of the issue. I took the “it” to mean the reaction and not the environment…so if the reaction is trying to “cool down”, it would do so by moving in the direction that would release energy, thus exhibit an exothermic process. Do I have this wrong?
So if we put the test tube in a hot bath(adding heat) and the reaction turned blue that means that the heat was added as a reactant(endothermic) meaning too much reactant now, so it needs to shift to the right to get rid of the excess reactant and rebranded? Or am I looking at this wrong? Or does this mean since it's shifting the heat from reactant side to the product side it is technically getting rid of the heat(cooling down). A separate question- does that mean a reaction can be exothemic and endothermic depending on if you are adding heat or taking away heat? I feel like my teacher made it seem that a reaction can be 1 or the other.
You can think of heat as a reactant (not technically correct, but it works as a way of predicting what happens to the equilibrium). Add heat, the equilibrium shifts to reduce the heat but going in the endothermic direction. In answer to your second question, no. You can add heat to any reaction, whether it is exo- or endothermic. The most important thing about a reversible reaction is, if it is exothermic in one direction, it is endothermic in the other.
HELP, question:
I'm looking for a reaction where you start with color (any color is ok) and after a certain time, it becomes colorless. If possible I would like to do it with non-harmful chemicals, because it's going to be an experiment for primary school kids.
-Start with a color (already set up in the container, if possible use non-harmful chemicals or natural products)
-Add H2O and it becomes colorless
-If possible, change the time it takes to become colorless based on the concentration of the initial chemicals/products
-Use natural products or non-harmful chemicals, as it is an experiment for kids, primary school students.
Thank you very much.
Reverse titration of acetic acid and NaOH using phenolphthalein
5:27 I though endothermic was taking heat in, if it's trying to cool wouldn't it be exothermic instead?
When we say "an endothermic reaction takes heat in", what we really mean is " an endothermic reaction takes heat energy from the surroundings (which includes the water that the chemicals are dissolved in) and changes it into chemical energy that is stored in the products. By changing heat energy into chemical energy, the system cools down.
Thanks. I'm so dumb. Excuse me for that.
You are not dumb - that was a very intelligent question showing that you are thinking about the topic, rather than just accepting something you have read or heard. I had to answer exactly the same question with my Year 12 class yesterday. This is an A level topic as well as GCSE, so it is considered to be a difficult subject to get your head around.
Thanks for the words of encouragement. There's hope for me after all.
This reaction is endothermic in general, right?
Tq sir
damnn i didnt know his name is prounced so fancy. my teacher says it as 'lee-chat-lee-ar". I've been deceived
Confused
good
HI GUYS
hi lad
abid ahad
@@fennprx7187 fenn prx
@@abidahad7242 406 Heysham Rd, Heysham, Morecambe LA3 2BJ
@@fennprx7187 thats not my address u donut
I am 100% sure that he is a doctor ( by seeing his handwriting )🤪🤪🤪
HaHa!
Why didn’t you do this in a fumehood? My teacher had directed me to do that.
The fumes from concentrated HCl are unpleasant and in an ideal world I would have done it in a fume cupboard, but it would have been much harder to film and you wouldn't have heard me speak over the noise of the extractor fan!
he risked his life for the video
Very brave not wearing gloves
ahaha all other vids just say "equilibrium shifts to left/right", without explaining what this means. only explanation ive seen which wasn't a waste of time
Which solution of middle
I don't understand your question. Please can you try to rephrase it?
Its a reversible reaction, so there is no one product but instead there are two, one will be from the exothermic side and one from the endothermic side, they are producing the product at the same rate hence you don't see a constant color change and the two products will be COCl4 and CO(H2O)6, so basically the one in the center is a mixture of the two
PS: I hope I am right, this is what I have learnt so far
@@richardhiggins6471 hey ,i am so sorry for asking but I have a chem 30 lab report due in 4 hours and I need the materials used in this in exact or close quantity. Can you please help me?
@@okiedokie4582 I cannot recall exact amounts, but it was one spatula of hydrated cobalt chloride (check the Hazcard about this) dissolved in the absolute minimum of distilled water (maybe 2-3 ml, a saturated solution). Then, to get the purple mixture in the middle I added concentrated hydrochloric acid (corrosive) drppwise from a pipette until I achieved the purple colour.
@@richardhiggins6471 Thank you so much, you just saved my lab report. Thank you :)
U hlakile
This is so boring
No-one forced you to watch it, did they? If you already understand it, brilliant, and if you don't, well, some people enjoy learning and understanding stuff.
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