ALERT ⚠️ , dear upcoming juniors u will find confusion when sir will tell about dependency of Rate constant and equilibrium constant , PAY ATTENTION Kf and Kb are different from Keq /Kc and Kp , it should eventually get clear by itself till video 7 , but still if it doesn't read the notes again and put emphasis on difference between RATE CONSTANT , AND EQUILIBRIUM CONSTANT ( which is ratio of Kf/Kb)
Dependency of Kc / Kp on catalyst/inhibitors: For catalyst, Kf and Kb both increase so Kf/Kb=Keq=constant For inhibitors, Kf and Kb both decrease so Kf/Kb=Keq=constant Keq is always constant kyuki jitna Kf badha ya ghata utna hi Kb badha ya ghata....toh un dono ka ratio is constant
Those who were confused ( I too was :) ) regarding equilbrium constatn depends on catalyst or not pls understand this - 1) Kc & Kp Are Eqm constants Which are independent of Catalyst and they are essentially a ratio of Kf : Kb. 2) However Kf and Kb are independent, Catalyst = Increase in rate = Kf Or Kb incresed. However there ration is independent of catalyst, Hope this helps
Sach me sir, mujhe 2 saal se phase or state me difference samjh ni aa raha tha par Ap to bahut acha padhate ho mujhe aapse ummed thi ki aap ek na ek lecture me jarur bataoge, and it happened in this lecture. Even I was expecting it in colloids 😊
All the liquid contents are miscible and thus they are not pure liquid understand it carefully that acetic acid, ester, alcohol and the water all are miscible also understand that equilibrium constant correctly is defined on the basis of activity and also, active mass is not same as concentration of that species Note that for concentration purposes we use activity to get a correct equilibrium constant and for partial pressure purposes we use fugacity to get a correct equilibrium constant Understand it that what we write as the expression of equilibrium constant involving concentrations aur partial pressure of species involved is just and approximation of equilibrium constant derived thermodynamically from activities and fugacity of species involved Please someone reading this go through the references as it will be very helpful in understanding the derivations of ionic equilibrium and why activity of pure substances is substituted one (even though that is not exactly unity but for practical purposes it is very very close to unity) Equilibrium constant is a dimensionless quantity when we have to standardize it, see NCERT of equilibrium: Box of "Units of Equilibrium Constant" refer to law of mass action statement which is in use en.wikipedia.org/wiki/Law_of_mass_action#Modern_statement_of_the_law to understand the term activity refer en.wikipedia.org/wiki/Thermodynamic_activity to understand the term activity refer en.wikipedia.org/wiki/Fugacity to understand why the current expression of equilibrium is an approximation of Modern statement chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Physical_Properties_of_Matter/Solutions_and_Mixtures/Nonideal_Solutions/Activities_and_their_Effects_on_Equilibria#:~:text=The%20Derivation%20of%20Mass%20Action%20Expressions,-Given%20all%20of&text=It%20should%20be%20noted%20that,by%20the%20standard%20state%20concentration.
you are in iit bhu, so i don't think youll need this, but, here is why.... concentration=n/Vol .... ∆Vol is nearly zero cause the liquid volume of container is fixed...but there is ∆n, change in moles of the species, so concentration is changing that's why we have to account that.... in of solvent ∆n is nearly zero , [solvent] is fixed....
Here it is not acting as a solvent, but it is also itself getting dissociated to H+ and OH-Active Mass 1 is taken in case H20 is in excess(acting as solvent)
All the liquid contents are miscible and thus they are not pure liquid understand it carefully that acetic acid, ester, alcohol and the water all are miscible also understand that equilibrium constant correctly is defined on the basis of activity and also, active mass is not same as concentration of that species Note that for concentration purposes we use activity to get a correct equilibrium constant and for partial pressure purposes we use fugacity to get a correct equilibrium constant Understand it that what we write as the expression of equilibrium constant involving concentrations aur partial pressure of species involved is just and approximation of equilibrium constant derived thermodynamically from activities and fugacity of species involved Please someone reading this go through the references as it will be very helpful in understanding the derivations of ionic equilibrium and why activity of pure substances is substituted one (even though that is not exactly unity but for practical purposes it is very very close to unity)
Equilibrium constant is a dimensionless quantity when we have to standardize it, see NCERT of equilibrium: Box of "Units of Equilibrium Constant" refer to law of mass action statement which is in use en.wikipedia.org/wiki/Law_of_mass_action#Modern_statement_of_the_law to understand the term activity refer en.wikipedia.org/wiki/Thermodynamic_activity to understand the term activity refer en.wikipedia.org/wiki/Fugacity to understand why the current expression of equilibrium is an approximation of Modern statement chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Physical_Properties_of_Matter/Solutions_and_Mixtures/Nonideal_Solutions/Activities_and_their_Effects_on_Equilibria#:~:text=The%20Derivation%20of%20Mass%20Action%20Expressions,-Given%20all%20of&text=It%20should%20be%20noted%20that,by%20the%20standard%20state%20concentration.
We said pure liquids always have active mass one. Then Why when H2O is not a solvent, we don't take its active mass 1? According to rule 3 , for a pure liquid active mass should be 1 but according to rule 4, only if it's solvent it should be 1? Does this hold only for water or any pure liquid. I am confused
@@neetusinha8504 both rules are indepedent. If it is a pure liquid it will be 1. If it is a solvent then also it will be 1. I think water is just not considered a pure liquid. You can check a quora post.
@@prismatic-bl8qf why is water not considered a pure liquid here? I got the point that they are independent rules, a pure liquid has active mass 1, a solvent in excess has active mass1. What if we have combinations. Pure liquid is a solvent. Water is generally pure and it is a solvent then its active mass is 1 If water is pure liquid but not a solvent, by rule 3 even its active mass is taken 1 (as u said, independent rules) But in this case why idn't water considered a pure solvent
Catalyst helps in attaining the equilibrium rapidly. So, rate of rxn depends on the catalyst. Kf and Kb are rate constants ,so they are dependent on the catalyst..
16:30 sir you said in previous video that catalyst doesnot affect rate constant and just helps in reaching the equilibrium fast, and here you are saying kf and kb depend on catalyst
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ALERT ⚠️ ,
dear upcoming juniors
u will find confusion when sir will tell about dependency of Rate constant and equilibrium constant , PAY ATTENTION Kf and Kb are different from Keq /Kc and Kp , it should eventually get clear by itself till video 7 , but still if it doesn't read the notes again and put emphasis on difference between RATE CONSTANT , AND EQUILIBRIUM CONSTANT ( which is ratio of Kf/Kb)
Thank you so muchhh
Thank you
thanks buddy ,
Dependency of Kc / Kp on catalyst/inhibitors:
For catalyst, Kf and Kb both increase so Kf/Kb=Keq=constant
For inhibitors, Kf and Kb both decrease so Kf/Kb=Keq=constant
Keq is always constant kyuki jitna Kf badha ya ghata utna hi Kb badha ya ghata....toh un dono ka ratio is constant
TH-cam ko koi jane btaoo ki pw and unacademy k baap bhte h tha, inko leke jaoo koi millions subscribers p
Those who were confused ( I too was :) ) regarding equilbrium constatn depends on catalyst or not pls understand this -
1) Kc & Kp Are Eqm constants Which are independent of Catalyst and they are essentially a ratio of Kf : Kb.
2) However Kf and Kb are independent, Catalyst = Increase in rate = Kf Or Kb incresed. However there ration is independent of catalyst, Hope this helps
Thanks❤🌹🌹🌹
Simple but thanks to you
wrong ,catalyst does not increase the rate of reaction, but it reduce the activation energy of reaction
○TOPICS IN THIS LECTURE:-
→ TYPES OF EQUILIBRIUM
→ LAW OF MASS ACTION
→ ACTIVE MASS AND MORE ABOUT IT
Sach me sir, mujhe 2 saal se phase or state me difference samjh ni aa raha tha par Ap to bahut acha padhate ho mujhe aapse ummed thi ki aap ek na ek lecture me jarur bataoge, and it happened in this lecture. Even I was expecting it in colloids 😊
Best TH-cam coaching
first comment ..btw thanks for all ur efforts
But H2O is in liquid state then why we can't take its active mass 1.rather than that is in excess
Same doubt, did you get it cleared? Please help
@@varadpawar4241 Here it is not acting as a solvent, but it is also itself getting dissociated to H+ and OH-
@@varadpawar4241Active Mass 1 is taken in case H20 is in excess(acting as solvent)
@@hardikaggarwal4510 It is a pure liquid though, so according to third point it's active mass should have been merged with the constant.
All the liquid contents are miscible and thus they are not pure liquid
understand it carefully that acetic acid, ester, alcohol and the water all are miscible
also understand that equilibrium constant correctly is defined on the basis of activity
and also, active mass is not same as concentration of that species
Note that for concentration purposes we use activity to get a correct equilibrium constant
and for partial pressure purposes we use fugacity to get a correct equilibrium constant
Understand it that what we write as the expression of equilibrium constant involving concentrations aur partial pressure of species involved is just and approximation of equilibrium constant derived thermodynamically from activities and fugacity of species involved
Please someone reading this go through the references as it will be very helpful in understanding the derivations of ionic equilibrium and why activity of pure substances is substituted one (even though that is not exactly unity but for practical purposes it is very very close to unity)
Equilibrium constant is a dimensionless quantity when we have to standardize it, see NCERT of equilibrium: Box of "Units of Equilibrium Constant"
refer to law of mass action statement which is in use
en.wikipedia.org/wiki/Law_of_mass_action#Modern_statement_of_the_law
to understand the term activity refer
en.wikipedia.org/wiki/Thermodynamic_activity
to understand the term activity refer
en.wikipedia.org/wiki/Fugacity
to understand why the current expression of equilibrium is an approximation of Modern statement
chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Physical_Properties_of_Matter/Solutions_and_Mixtures/Nonideal_Solutions/Activities_and_their_Effects_on_Equilibria#:~:text=The%20Derivation%20of%20Mass%20Action%20Expressions,-Given%20all%20of&text=It%20should%20be%20noted%20that,by%20the%20standard%20state%20concentration.
sir in the last question u have considered concentration of ester also although it is pure liquid....why????
Yes I was also thinking about it...Guys someone please tell.
it is not pure check the eq again it is written (aq)
you are in iit bhu, so i don't think youll need this, but, here is why.... concentration=n/Vol .... ∆Vol is nearly zero cause the liquid volume of container is fixed...but there is ∆n, change in moles of the species, so concentration is changing that's why we have to account that.... in of solvent ∆n is nearly zero , [solvent] is fixed....
Hello sir,
Could you pls explain that why didn't you considered conc. Of h2o as unity even when it is a pure liquid?
Brother h2o solvent hai BTW video puri dekhni chahiye
Here it is not acting as a solvent, but it is also itself getting dissociated to H+ and OH-Active Mass 1 is taken in case H20 is in excess(acting as solvent)
All the liquid contents are miscible and thus they are not pure liquid
understand it carefully that acetic acid, ester, alcohol and the water all are miscible
also understand that equilibrium constant correctly is defined on the basis of activity
and also, active mass is not same as concentration of that species
Note that for concentration purposes we use activity to get a correct equilibrium constant
and for partial pressure purposes we use fugacity to get a correct equilibrium constant
Understand it that what we write as the expression of equilibrium constant involving concentrations aur partial pressure of species involved is just and approximation of equilibrium constant derived thermodynamically from activities and fugacity of species involved
Please someone reading this go through the references as it will be very helpful in understanding the derivations of ionic equilibrium and why activity of pure substances is substituted one (even though that is not exactly unity but for practical purposes it is very very close to unity)
Equilibrium constant is a dimensionless quantity when we have to standardize it, see NCERT of equilibrium: Box of "Units of Equilibrium Constant"
refer to law of mass action statement which is in use
en.wikipedia.org/wiki/Law_of_mass_action#Modern_statement_of_the_law
to understand the term activity refer
en.wikipedia.org/wiki/Thermodynamic_activity
to understand the term activity refer
en.wikipedia.org/wiki/Fugacity
to understand why the current expression of equilibrium is an approximation of Modern statement
chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Physical_Properties_of_Matter/Solutions_and_Mixtures/Nonideal_Solutions/Activities_and_their_Effects_on_Equilibria#:~:text=The%20Derivation%20of%20Mass%20Action%20Expressions,-Given%20all%20of&text=It%20should%20be%20noted%20that,by%20the%20standard%20state%20concentration.
@@hardikaggarwal4510 bhai kuch bhi h2o nahi tutta h+ and oh- m
We said pure liquids always have active mass one. Then Why when H2O is not a solvent, we don't take its active mass 1? According to rule 3 , for a pure liquid active mass should be 1 but according to rule 4, only if it's solvent it should be 1? Does this hold only for water or any pure liquid. I am confused
Same doubt apka clear ho to btana🙃
bro if we take
[h2o}=1
then we have to take modified const
so for taking {h2o}=1 ,we have to multiply value of [h2o] in kf@@neetusinha8504
@@neetusinha8504 both rules are indepedent. If it is a pure liquid it will be 1. If it is a solvent then also it will be 1. I think water is just not considered a pure liquid. You can check a quora post.
btw dont worry which we have to take as 1 or not since it is usually limited in our questions and by practice you will realise
@@prismatic-bl8qf why is water not considered a pure liquid here? I got the point that they are independent rules, a pure liquid has active mass 1, a solvent in excess has active mass1.
What if we have combinations. Pure liquid is a solvent. Water is generally pure and it is a solvent then its active mass is 1
If water is pure liquid but not a solvent, by rule 3 even its active mass is taken 1 (as u said, independent rules)
But in this case why idn't water considered a pure solvent
Masterpiece
sir , how to find pure liquid in a reaction
it will be given
the same notes he is writing gets copied by allen teachers , even same examples. this stidy material is more than enough for jee advanced.
That's not true. I myself am a student of there, but I study from here also.
12:31 : wow.
Why are stoichiometric coefficient on power.
Why
20:43
30:47 most welcome ❤
16:49 depends on catalyst !?! Pls verify...
Catalyst helps in attaining the equilibrium rapidly.
So, rate of rxn depends on the catalyst.
Kf and Kb are rate constants ,so they are dependent on the catalyst..
Thank you sir
10:59 Isn't this an irreversible reaction???
16:30 sir you said in previous video that catalyst doesnot affect rate constant and just helps in reaching the equilibrium fast, and here you are saying kf and kb depend on catalyst
it was for rate of reaction, not for rate constant 🤦♂🤦♂
in previous video it was said that catalyst does not affect equilibrium constant. rate constant and equilibrium constants are not the same thing
Amazing Sir
17:00
Thanks sir
start 00:00
sep 24; 9:29 PM lecture + notes.
So?
September 23'rd, 5:00 PM lecture + notes XD
@@windows1543 hehe, hope you get your dream college
cool
17:52
25:49
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Mujhe toh ek bhi nhi aya
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