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!
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)
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!
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
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
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 🇮🇳
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👍👍👍👍
Always enjoy these videos. I am still confused on one thing. At nine minutes during an ICE table the change in H2O is shown as .038 mols. The initial value is zero and the equilibrium value is .138. So why is the change not .138?
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?
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 ?
Nice video, but it did not answer the fundamental questions regarding equilibrium constant: 1. why is it calculates the way it is and 2. for what does the value stand for? 1. So equilibrium constant is calculated with the formula K = ([C]^c * [D]^d) : ([A]^a * [B]^b) Why is it calculated like this? Why is it not calculated like this: K = (c*[C] * d*[D]) : (a*[A] * b*[B]) or like this K = (c*[C] + d*[D]) : (a*[A] + b*[B]) or like this K = ([C]^c + [D]^d) : ([A]^a + [B]^b) or just like this K = ([C] + [D]) : ([A] + [B]) ? Why does it have to be like it is, and why would these other calculations not good enough when determinating the ratio between the starting compounds of the reaction and the product compounds of the reaction? 2. The value of K is not the concentration ratio between the starting compounds of the reaction and the product compounds of the reaction, because that would be calculated just with a simple formula: K = ([C] + [D]) : ([A] + [B]) So, why is K calculated like it is, and what does it's number really stand for?
uh didnt you watch the video? concentrations in products / concentration in reactants but make sure you multiply them and properly exponentiate them to their coefficient. those values will be given in a problem or determined experimentally. you asked this 2 years ago so i doubt you give a rats ass about the answer now
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?
Hi, I just have one doubt: why do we multiply ( the products by the products and the reactants by the reactants) instead of adding, when calculating the equilibrium constant?
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!!
If a reaction has a very low K value, would that mean that the reaction at that temperature is non spontaneous as there are very few products. Also, if the k value is very large, would that mean that the reaction is spontaneous as there are many products?
I don't know why use concentrations for this, I think molar fractions would be better. If there is an equal amount of products and reactants, but there molar masses aren't equal, then k won't be equal to one, but it should.
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
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?
How can he explain things so fast but so well?! Keep up the amazing work Mr Andersen you're the best!
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!!!
love this guy's teaching, especially his concise yet detailed explanations. thanks Paul.
Wow thanx for a beautiful lecture. Never knew the meaning of K value. No chemistry book has shown such simplified meaning.
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!
Perfect. Just what I needed to share with my students while teaching from home. Thank you for all you do!
dude i fucking love you
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 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)
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!
Thank you! K>1,P>R,arrow points to the right indicating a right shift while K
hi
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
Thank you sir. Simple, effective, insightful and fun. Just what education should be.
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
Mr. Andersen saving my but again. First in high school now in my senior year of college.
you are super helpful man bless you and all the generations that come behind you!
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're helping me get a degree!
u r the goat & teach sm better than my teacher thank u sir
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!
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
I am poor human being desperate to pass his a level chemistry, but this guy gives me a hope.
Didn't take chemistry yet, but still understood it. Thanks for the extra knowledge!
Daym every problem I have in chem and physics this guy has already done it
you explain WAYYY better than my chem teacher
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
Thank you for the videos! Really clarified important concepts!
The illustrations are very helpful for me. It would be helpful if they just called it the equilibrium ratio constant.
The song in the beginning of the video is so cool!
Wish they had TH-cam videos when I was in college taking chemistry.
At 3 min, the expression should be aA + bB cC + dD (missing PLUS sign on RHS)
You teach very well. I like your teaching
Of course that was helpful...thanks! You are the best, Andersen..
Thanks! You make the whole thing very understandable.
Thank you so much I really needed this 🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻
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
this guy proceeds to explain in 6 minutes what my professor failed to explain in 4 hours
Very very helpful thanks... And very easy language....
Thanks Mr.Andersen this is really helpful
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👍👍👍👍
mr anderson can you do more practiced questions and examples please???
Always enjoy these videos. I am still confused on one thing. At nine minutes during an ICE table the change in H2O is shown as .038 mols. The initial value is zero and the equilibrium value is .138. So why is the change not .138?
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?
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 ?
Time to review ... Thank you for your video.
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
and here I am a college junior coming back to this yet again
It was really helpful. keep going!
Nice video, but it did not answer the fundamental questions regarding equilibrium constant:
1. why is it calculates the way it is and
2. for what does the value stand for?
1. So equilibrium constant is calculated with the formula
K = ([C]^c * [D]^d) : ([A]^a * [B]^b)
Why is it calculated like this? Why is it not calculated like this:
K = (c*[C] * d*[D]) : (a*[A] * b*[B])
or like this
K = (c*[C] + d*[D]) : (a*[A] + b*[B])
or like this
K = ([C]^c + [D]^d) : ([A]^a + [B]^b)
or just like this
K = ([C] + [D]) : ([A] + [B]) ?
Why does it have to be like it is, and why would these other calculations not good enough when determinating the ratio between the starting compounds of the reaction and the product compounds of the reaction?
2. The value of K is not the concentration ratio between the starting compounds of the reaction and the product compounds of the reaction, because that would be calculated just with a simple formula:
K = ([C] + [D]) : ([A] + [B])
So, why is K calculated like it is, and what does it's number really stand for?
Thank you sooooo much, great videos
you just practically save my life
THANK YOU SOO MUCH I LOVE YOUR VIDEOS THEY ARE SUPER HELPFUL
Your videos are so helpful! Thanks so much! Keep up the good work.
Thanks so much, got Chem sac tomorrow and I finally understand the concept :)
Thank you Mr. Anderson
Thanks a lot for your clear explanation!
can you do a video on how to find the equilibrium constant in electrolysis
Fantastically explained!
how did you get the numerical value of the constant?
+Krystel Shayne Lantano I would like that as well :) Did you find the answer?
+Krystel Shayne Lantano you use the concentrations, or you can get it experimentally, i think
uh didnt you watch the video? concentrations in products / concentration in reactants but make sure you multiply them and properly exponentiate them to their coefficient. those values will be given in a problem or determined experimentally. you asked this 2 years ago so i doubt you give a rats ass about the answer now
@@CoDRagna I care
@@chrisfrost7945 great point!
Excellent. Thank you
is it the same if it ask you to writ an equation for equilibrium constant for forward reaction
Thank you soooooooooo much. U r an amazing teacher.
You went through very well the meaning of k, but you didn't go through how you got to value eg what did you calculate eg what were the concentrations?
Love this. Thank you
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 for this helpful video!
Wow thanks! That was so helpful!
Hi, I just have one doubt: why do we multiply ( the products by the products and the reactants by the reactants) instead of adding, when calculating the equilibrium constant?
What software are you using to create your vids???
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!!
excellent.... splendid explanation
it was so helpful thank you so much:)
If a reaction has a very low K value, would that mean that the reaction at that temperature is non spontaneous as there are very few products. Also, if the k value is very large, would that mean that the reaction is spontaneous as there are many products?
Very helpful. Great job, and thank you!
thank you so much!!! you are a great teacher!!!!
That was VERY helpful thx.
is k value given to us on the exam because I cannot find it on my periodic table
So, we can't calculate for K? It would always be given to us?
thanks a million times
I don't know why use concentrations for this, I think molar fractions would be better. If there is an equal amount of products and reactants, but there molar masses aren't equal, then k won't be equal to one, but it should.
this guy is awesome
Thanks a lot ✨ it really helped!!!
Thank you so much sir.😍😍😍😍😍💟
Very helpful, thank you
Thanx it helps in my AIIMS questions
at 3.37 Is H2O taken into account for this equation? I thought this is only for gases and aqueous ?
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?
I get this. But what's the proof that _K_ stays the same?
thank you! it feels like you did it all on one breath though!
What’s the difference between kp and kc
why does only temperature affect k, and not pressure, concentation etc?
Tkkk.....very must sir.
Love from Manipur
And phosgene is made by simply let them sit togheter or ignite the mixture?
I have an upcoming report for this topic and thnks god that you creaed this video. 😇