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
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
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!!
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 🇮🇳
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 ?
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?
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?
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?
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?
thank you so much but i have a question! we dont write the liquids and solids in the equation becuz it doesnt affect the concentration but what about aqueous substances? do we include them in the equation? does it affect the concentration
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.
+2ndintelligentWorld no it wouldn't be because the number is way below 1. (1.0 x 10^-30=.0000000000000000000000000000001) That means there would be more reactants because the products aren't forming, so it would be to the left.
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?
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
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👍👍👍👍
how do you know the concentration of the substances that youre putting into the K value equation ? is this information usually given ? (high school chemistry btw)
Can anyone help me understand why "there are 2 moles of water" in the equation which says 2H2O - I thought this meant there were 2 molecules of water (and moles is like 6 x 10^23)
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?
if the reaction is endothermic and you increase temperature, the equilibrium will shift to the right and create higher [products] so therefore a higher Keq. If the reaction is exothermic then increasing the temperature will shift the equlibrium left, and so it will decrease Keq
i legit asked my teacher what K actually is, like what does it mean and why we use it. her reply, "we already covered it in class. i suggest you go over the chapter again!!!!" I wanted to throw something at her istg
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?
Thank you Mr. Andersen, your videos are wonderful!
Does Kc value tell about the reaction rate???
@@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.
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.
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!
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!
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 soo much sir, this video was beautifully explained. God Bless !!!!
dude i fucking love you
Thank you! K>1,P>R,arrow points to the right indicating a right shift while K
hi
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 sir. Simple, effective, insightful and fun. Just what education should be.
Mr. Andersen saving my but again. First in high school now in my senior year of college.
this guy proceeds to explain in 6 minutes what my professor failed to explain in 4 hours
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
u r the goat & teach sm better than my teacher thank u sir
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
Daym every problem I have in chem and physics this guy has already done it
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!!
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! ❤️🔥
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
you explain WAYYY better than my chem teacher
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 anderson can you do more practiced questions and examples please???
God damn. How did he explain like that in 6 minutes
You teach very well. I like your teaching
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!
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.
Thank you so much I really needed this 🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻
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 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 ?
and here I am a college junior coming back to this yet again
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?
You're helping me get a degree!
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?
Didn't take chemistry yet, but still understood it. Thanks for the extra knowledge!
can you do a video on how to find the equilibrium constant in electrolysis
And phosgene is made by simply let them sit togheter or ignite the mixture?
Of course that was helpful...thanks! You are the best, Andersen..
Thank you for the videos! Really clarified important concepts!
at 3.37 Is H2O taken into account for this equation? I thought this is only for gases and aqueous ?
You sir are a gentleman and a scholar
At 3 min, the expression should be aA + bB cC + dD (missing PLUS sign on RHS)
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?
is k value given to us on the exam because I cannot find it on my periodic table
Thanks! You make the whole thing very understandable.
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?
So, we can't calculate for K? It would always be given to us?
is it the same if it ask you to writ an equation for equilibrium constant for forward reaction
Wish they had TH-cam videos when I was in college taking chemistry.
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?
What if there are solids or liquid in products and reactants . Do I have to put their concentrations in the equation ?
The song in the beginning of the video is so cool!
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?
thank you so much but i have a question! we dont write the liquids and solids in the equation becuz it doesnt affect the concentration but what about aqueous substances? do we include them in the equation? does it affect the concentration
Thanks Mr.Andersen this is really helpful
Somehow my chemistry teacher was able to teach me this is 27 minutes, and I only understood about 20% of what he said
How does temperature affect the equilibrium constant?
Your videos are so helpful! Thanks so much! Keep up the good work.
how do you know which side is the product and which side is the reactant?
why does only temperature affect k, and not pressure, concentation etc?
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.
Thanks so much, got Chem sac tomorrow and I finally understand the concept :)
5:05 I think you mean shift towards to the right not left. this confused me massively
+2ndintelligentWorld no it wouldn't be because the number is way below 1. (1.0 x 10^-30=.0000000000000000000000000000001) That means there would be more reactants because the products aren't forming, so it would be to the left.
+Yonas Meshesha i think i put 30 zeros in there. it should be 29 zeros and the 1
Does it matter if the concentrations are in mM as opposed to M?
THANK YOU SOO MUCH I LOVE YOUR VIDEOS THEY ARE SUPER HELPFUL
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?
I get this. But what's the proof that _K_ stays the same?
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!
The illustrations are very helpful for me. It would be helpful if they just called it the equilibrium ratio constant.
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👍👍👍👍
how do you know the concentration of the substances that youre putting into the K value equation ? is this information usually given ? (high school chemistry btw)
concentration is always given in the question
It was really helpful. keep going!
What software are you using to create your vids???
Can anyone help me understand why "there are 2 moles of water" in the equation which says 2H2O - I thought this meant there were 2 molecules of water (and moles is like 6 x 10^23)
Do you have a note version of this?
Very very helpful thanks... And very easy language....
But how do you derive the number k?
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?
What’s the difference between kp and kc
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
you just practically save my life
So is Kc proportional to Temp. Or is it inversely proportional? Can anyone explain this to me?
Mathias T it depends on if the reaction is exothermic or endothermic
if the reaction is endothermic and you increase temperature, the equilibrium will shift to the right and create higher [products] so therefore a higher Keq. If the reaction is exothermic then increasing the temperature will shift the equlibrium left, and so it will decrease Keq
i legit asked my teacher what K actually is, like what does it mean and why we use it. her reply, "we already covered it in class. i suggest you go over the chapter again!!!!" I wanted to throw something at her istg
Guy's , i know we should except liquids and solids but how about the aquas ?
When Kc isn't equally to 1,then it means the system isn't in equil.state then why the constant is called EQUILIBRIUM constant.
How do you get those K values
how do you make your simulations?
Time to review ... Thank you for your video.
Thanks a lot for your clear explanation!
Thank you so much sir.😍😍😍😍😍💟