No it doesn't. Only the concentration of reactants and products. If it's >1 that means there are more products than reactants. We also say that the equilibrium lies on the right. When its
Thank you soooooo much!!! I love the way you simplify complex concepts and I love the stimulations! I think everyone should watch your videos and benefit from them!!!
Thank you for helping me through chemistry's difficult concepts. I feel hopeful even when things are hazy in class as I know I can look up the concept on your channel and find clarity! Cheers to you for sharing your knowledge and gift as a teacher!
i've been watching your videos since my first intro. chem class a 1.5 years ago. i'm in chem 2 now and you are still doing god's work (i'm atheist btw). can't thank you enough for this invaluable resource, sir
I watch your videos all the time, and I would just like to thank you for taking the time to post them. You are an excellent teacher, easy to follow and understand. Once again thank you so much!
Products/reactants Equilibrium constant uses molarity so before you set up the equation you need to balance the equation, find the molarity of each product and reactant. Then you set up an equation that multiplies the molarity of all the products with exponents that are the coefficients in the reaction. This has to be over the molarity of the reactants multiplied together with exponents that are the coefficients. Should look like this: (C)^c(D)^d ----------------- (A)^a(B)^b If Keq < 1 it favors reactants in the left direction. If Keq > 1 it favors products in the right direction. By the way solids and liquids are not in the equation.
Equilibrium constant (K) is equal to (C)^c x (D)^d / (A)^a x (B)^b. There is an invisible multiplication sign in the middle, so you have to multiple the molarities/concentrations of the products and divide that over by the molarities/concentrations of the reactants to get K. (And you get molarity by using C = n/V)
Actually I didn't get u yarrr. How can u explain so nicely... Equilibrium constant was a doubt in my mind for 6 years.. U just cleared in a 6 min.... But u r lilbit fast.. I watched at 0.75X .. it was so helpful... Love u bro 😎. From INDIA 🇮🇳
In equilibrium constant the reaction is reversible hence the double arrows, meaning reactants can be products and products can be reactants. But we try to figure out if we have one more than the other by our constant K. Constant K measures out if we have more reactants or if we have more products at equilibrium. K represents the concentration of our products over our reactants. K>>1 reactant to product, K
I already knew how to solve it,but the question that was annoying me was that what is k constant and what does its value represent,thanks very much sir,definitely subscribing👍👍👍👍
depends on the forward reaction, if its exothermic (which is the case for most reactions) then clearly if u increase the temperature the equilibrium will favor the endothermic reaction (which is the backward reaction) which increases the reactants, making the K value lower. i hope that was helpful!!
Great video! I wonder why the temperature has an impact on what will be produced more, the reactant or the product, and therefore, what the K value is. What role does temperature play in the way that at one moment the product can be produced more than the reactant (thus, favoring the forward reaction)? Conversely, how does a lower temperature of the same reaction make it favor the reverse reaction?
Bavley Guerguis I am not a very bright student. It would mean a lot if someone else were to explain it to me. I'm not able to comprehend from internet sources
How can we solve units of concentration for the followinv reaction? I have tried so hard on it but couldn't understand that how do we get moldm‐³ as its answer. When nitrogen reacts with hydrogen to form ammonia, the equilibrium mixture contains 0.31 mol dm‐³ and 0.50 mol dm‐³ of nitrogen and hydrogen respectively. If the Kc is 0.50 mol‐²dm⁶, what is the equilibrium concentration of NH3?
Thank you very much. You say if Kc is greater than 1, it moves from reactants to the products side. And if the Kc is less than 1, it moves products to reactants. My question is when can we have the equilibrium mixture for an appreciable concentration of both reactants and products ?
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This guy is single-handedly keeping my GPA in equilibrium.
K
+MegaCadette55 HAHA
LOL, dude said "1.0" lmaoo
Lol I wish I could be as creative as u guys in comments
This thread 😆
you were there for me when no one else was
Lol
Omg yes
I commented this in undergrad and as a now medical student I can honestly say you are still there for me when no one else is
Steffy Martinez queen
@@soccerismylife514 ohh how cute
How can he explain things so fast but so well?! Keep up the amazing work Mr Andersen you're the best!
One thing missing: solid and liquid exceptions.
Was just looking for this to confirm it's real, should be higher in the comments
solid and liquid should not be included in the equilibrium because only gas has pressure.
Others should know👍
@@Kim-mu7gw This is what I was looking for thank you!!!
@@Kim-mu7gw wait what about aq?
love this guy's teaching, especially his concise yet detailed explanations. thanks Paul.
Thank you Mr. Andersen, your videos are wonderful!
Does Kc value tell about the reaction rate???
No it doesn't. Only the concentration of reactants and products. If it's >1 that means there are more products than reactants. We also say that the equilibrium lies on the right. When its
@@thisisnotmyfinalform7856 No, it doesn't. It tells us whether we'll have more products or more reactants when we reach equilibrium.
Thank you soooooo much!!! I love the way you simplify complex concepts and I love the stimulations! I think everyone should watch your videos and benefit from them!!!
Perfect. Just what I needed to share with my students while teaching from home. Thank you for all you do!
Thank you for helping me through chemistry's difficult concepts. I feel hopeful even when things are hazy in class as I know I can look up the concept on your channel and find clarity! Cheers to you for sharing your knowledge and gift as a teacher!
Wow thanx for a beautiful lecture. Never knew the meaning of K value. No chemistry book has shown such simplified meaning.
First your videos helped me with AP biology as a senior in high school. Now they're helping me with chemistry in college. I love these.
i've been watching your videos since my first intro. chem class a 1.5 years ago. i'm in chem 2 now and you are still doing god's work (i'm atheist btw). can't thank you enough for this invaluable resource, sir
I watch your videos all the time, and I would just like to thank you for taking the time to post them. You are an excellent teacher, easy to follow and understand. Once again thank you so much!
dude i fucking love you
Thank you sir. Simple, effective, insightful and fun. Just what education should be.
Thank you! K>1,P>R,arrow points to the right indicating a right shift while K
hi
I wish he would have covered how to calculate the equilibrium constant...
me too man, me too
Products/reactants
Equilibrium constant uses molarity so before you set up the equation you need to balance the equation, find the molarity of each product and reactant. Then you set up an equation that multiplies the molarity of all the products with exponents that are the coefficients in the reaction. This has to be over the molarity of the reactants multiplied together with exponents that are the coefficients. Should look like this:
(C)^c(D)^d
-----------------
(A)^a(B)^b
If Keq < 1 it favors reactants in the left direction. If Keq > 1 it favors products in the right direction.
By the way solids and liquids are not in the equation.
Bro I a mega test tomorrow and hace to learn this in 4 hours
@@frodobaggins7227 the molarity, Why multiply without adding up?
can you please explain it for me
Equilibrium constant (K) is equal to (C)^c x (D)^d / (A)^a x (B)^b. There is an invisible multiplication sign in the middle, so you have to multiple the molarities/concentrations of the products and divide that over by the molarities/concentrations of the reactants to get K. (And you get molarity by using C = n/V)
u r the goat & teach sm better than my teacher thank u sir
Actually I didn't get u yarrr. How can u explain so nicely... Equilibrium constant was a doubt in my mind for 6 years.. U just cleared in a 6 min.... But u r lilbit fast.. I watched at 0.75X .. it was so helpful... Love u bro 😎. From INDIA 🇮🇳
you are super helpful man bless you and all the generations that come behind you!
Mr. Andersen saving my but again. First in high school now in my senior year of college.
oh my! thank you sm! hoping it will help me in my prelim exam in cellular and molecular biology!! taking the test in a few! ❤️🔥
You sir are a gentleman and a scholar
Thank you Mr. ANderson...I have watched your videos lately and I really learned a lot
Very helpful! I learned this a week ago and completely forgot the concept. After watching this video however, I was able to jog my memory!
Daym every problem I have in chem and physics this guy has already done it
You teach very well. I like your teaching
am finally getting smething BOZEMAN yuh the best...thkz alot
+Anthony okpara or that your just dumb and took this guy for u to actually get something and get you to use one of your brain cell on
Of course that was helpful...thanks! You are the best, Andersen..
In equilibrium constant the reaction is reversible hence the double arrows, meaning reactants can be products and products can be reactants. But we try to figure out if we have one more than the other by our constant K. Constant K measures out if we have more reactants or if we have more products at equilibrium. K represents the concentration of our products over our reactants. K>>1 reactant to product, K
Thank you so much I really needed this 🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻
Thanks! You make the whole thing very understandable.
You're helping me get a degree!
Thank you for the videos! Really clarified important concepts!
Thank you soo much sir, this video was beautifully explained. God Bless !!!!
Thanks Mr.Andersen this is really helpful
Didn't take chemistry yet, but still understood it. Thanks for the extra knowledge!
you just practically save my life
The song in the beginning of the video is so cool!
I already knew how to solve it,but the question that was annoying me was that what is k constant and what does its value represent,thanks very much sir,definitely subscribing👍👍👍👍
I am poor human being desperate to pass his a level chemistry, but this guy gives me a hope.
THANK YOU SOO MUCH I LOVE YOUR VIDEOS THEY ARE SUPER HELPFUL
you explain WAYYY better than my chem teacher
Your videos are so helpful! Thanks so much! Keep up the good work.
Very very helpful thanks... And very easy language....
Thanks so much, got Chem sac tomorrow and I finally understand the concept :)
this guy proceeds to explain in 6 minutes what my professor failed to explain in 4 hours
Wish they had TH-cam videos when I was in college taking chemistry.
Fantastically explained!
It was really helpful. keep going!
Thanks a lot for your clear explanation!
4:26 Why does the increase in temperature decrease the K value?
depends on the forward reaction, if its exothermic (which is the case for most reactions) then clearly if u increase the temperature the equilibrium will favor the endothermic reaction (which is the backward reaction) which increases the reactants, making the K value lower.
i hope that was helpful!!
The illustrations are very helpful for me. It would be helpful if they just called it the equilibrium ratio constant.
Time to review ... Thank you for your video.
Thank you Mr. Anderson
excellent.... splendid explanation
Great video! I wonder why the temperature has an impact on what will be produced more, the reactant or the product, and therefore, what the K value is. What role does temperature play in the way that at one moment the product can be produced more than the reactant (thus, favoring the forward reaction)? Conversely, how does a lower temperature of the same reaction make it favor the reverse reaction?
mr anderson can you do more practiced questions and examples please???
Tkkk.....very must sir.
Love from Manipur
So is the K value the same as Log K? Like when modeling in the GWB, each reaction has Log K values at different temperatures
Thank you soooooooooo much. U r an amazing teacher.
4:03 You said "standard temperature and pressure", but then the box said 25 degrees Celsius, which is room temperature. Which did you intend?
overall the chemical reaction's entourage
Thank you very much for this helpful video!
Wow thanks! That was so helpful!
can someone help me... if the product I have in the reaction is in (aq) aqueous state, should I leave it out when calculating for Kp?
Syazlina Aasim yes, you only use the gaseous stuff in your calculations :)
Bavley Guerguis Do you mind explaining?
Michael Malize could you please explain
Bavley Guerguis I am not a very bright student. It would mean a lot if someone else were to explain it to me. I'm not able to comprehend from internet sources
and here I am a college junior coming back to this yet again
Thank you so much sir.😍😍😍😍😍💟
man this was soooo helpful! thanks!!
thank you so much!!! you are a great teacher!!!!
Thank you sooooo much, great videos
Very helpful. Great job, and thank you!
I have an upcoming report for this topic and thnks god that you creaed this video. 😇
CO2 (g) + H2O (l) H2CO3 (aq)
Calculate the equilibrium constant using the following concentrations [H2CO3] = 7.75 x 10-4 M and [CO2] = 5.65 x 10-1 M
Love this. Thank you
Thanks a lot ✨ it really helped!!!
How can we solve units of concentration for the followinv reaction? I have tried so hard on it but couldn't understand that how do we get moldm‐³ as its answer. When nitrogen reacts with hydrogen to form ammonia, the equilibrium mixture contains 0.31 mol dm‐³ and 0.50 mol dm‐³ of nitrogen and hydrogen respectively. If the Kc is 0.50 mol‐²dm⁶, what is the equilibrium concentration of NH3?
is it the same if it ask you to writ an equation for equilibrium constant for forward reaction
this was just beautiful!!!
Thank you very much.
You say if Kc is greater than 1, it moves from reactants to the products side. And if the Kc is less than 1, it moves products to reactants. My question is when can we have the equilibrium mixture for an appreciable concentration of both reactants and products ?
Thanx it helps in my AIIMS questions
it was so helpful thank you so much:)
It was very helpful sir.
This was so helpful!!
Thank you so much :)
At 3 min, the expression should be aA + bB cC + dD (missing PLUS sign on RHS)
Great video, very well explained
Somehow my chemistry teacher was able to teach me this is 27 minutes, and I only understood about 20% of what he said
Damn this sure was helpful thanks brother
That was superhelpful :) Thanks!
can you do a video on how to find the equilibrium constant in electrolysis
This is helpful, thank you!
What if I'm asked to solve for the Kc and Kp and the given is only the molarities of all the substance given at a certain temperature?
Very helpful, thank you
And phosgene is made by simply let them sit togheter or ignite the mixture?
Excellent. Thank you
thanks mr.Anderson , it was os usefull
That was VERY helpful thx.
It was helpful 🙏
So helpful, thanks!
thanks a million times
this guy is awesome