Hi Victor, They have to give you some clue. If it is thermodynamically favorable (spontaneous) it is K>1. If they give you a delta G or Standard Reduction Potential, you can also figure it out. Was there any other information? If it is only the reaction I do not know how to figure it out. Sorry!
Hi Serineh, I am sorry I do not. I would lookfor a junior or senior at your university that is majoring in chemistry and hire them. Often, universities have tutors. Maybe reach out to student services. I hope you find a great tutor! Thanks:)
Hello, sorry to bother you Me and my colleagues are designing a reactor, we wants something simple and easy to make, do u have any thoughts on the system and type of reaction we should work with? We want something simple, affordable and not hazardous
Hi Mohamed, Thank you for your question. I am sorry, this is not my expertise. I think an engineer would be a better support for you. I hope things go well. Thanks!
I still don't understand what is the change which you mentioned in video For example when i have [4] moles of reactant and [2] of product ,[1.5] mol of reactant transform to product and [1.5 ] mol of product transform into reactant or stable is just proportion for example [1.4] mol of reactant transform in product and [0.3] product transform into reactant?
Hi Kcoc, when at equilibrium the rate at which reactant and product convert to one another is the same. When equal rates are achieved (equilibrium) there will be a constant ratio of the amounts of reactant and product. We then put these amounts into the equilibrium expression (products divided by reactants) to get a value. If K< 1 there are more reactants than products at equilibrium (reactant favored), and vice versa. I hope that helps!
Hi Bethany, the only other way is to be given concentrations at equilibrium and plug them into the equilibrium expression to calculate K. Other qualitative clues for product favored: a positive standard reduction potential or a negative Gibb’s free energy (and vice versa for a reactant favored reaction). I hope that helps. Thanks! Please subscribe if you haven’t already!😊
Hi Nolimitderrick:) You will know k>1 if 1. There are more products than reactants at equilibrium or 2. The delta G (Gibbs Free Energy) is negative. You can figure out G if you know H and S. This reaction is exothermic (spontaneous for enthalpy) but becomes more ordered (nonspontaneous for entropy). If you are only given the equation I think you need to google more information to identify that it is product favored. Was more information given in the question? That could give you clues. I hope your class goes well!
I’ve been struggling with equilibrium for the last few weeks, this helped so much!
Hi MusicMelody, I am so glad it was helpful. I hope the rest of your class goes well:) Thanks!
This is my first time watching your videos, I love your energy and you explain everything very clearly !
Hi Krovely, thank you! Welcome to the channel 😊
Thank you so much, it's great to have someone like you explain it ❤️❤️❤️😌
Thanks Michael! I hope your class goes well:)
I have some problems in a textbook asking me if the Keq is= O, > or
Hi Victor, They have to give you some clue. If it is thermodynamically favorable (spontaneous) it is K>1. If they give you a delta G or Standard Reduction Potential, you can also figure it out. Was there any other information? If it is only the reaction I do not know how to figure it out. Sorry!
Youre amazing! Bless you.
Hi Dani, I am so glad it helped. God bless you! :)
I love your videos and they way you explain. It is very helpful. I was wondering if you do private tutoring ?
thank you
Hi Serineh, I am sorry I do not. I would lookfor a junior or senior at your university that is majoring in chemistry and hire them. Often, universities have tutors. Maybe reach out to student services. I hope you find a great tutor! Thanks:)
Hello, sorry to bother you
Me and my colleagues are designing a reactor, we wants something simple and easy to make, do u have any thoughts on the system and type of reaction we should work with? We want something simple, affordable and not hazardous
Hi Mohamed, Thank you for your question. I am sorry, this is not my expertise. I think an engineer would be a better support for you. I hope things go well. Thanks!
I still don't understand what is the change which you mentioned in video
For example when i have [4] moles of reactant and [2] of product ,[1.5] mol of reactant transform to product and [1.5 ] mol of product transform into reactant or stable is just proportion for example [1.4] mol of reactant transform in product and [0.3] product transform into reactant?
Hi Kcoc, when at equilibrium the rate at which reactant and product convert to one another is the same. When equal rates are achieved (equilibrium) there will be a constant ratio of the amounts of reactant and product. We then put these amounts into the equilibrium expression (products divided by reactants) to get a value. If K< 1 there are more reactants than products at equilibrium (reactant favored), and vice versa. I hope that helps!
This is very helpful! Thank you so much for your clear explanation! :)
Hi Trista, I am glad it was helpful! Good luck in you class:)
You taught this so well! Thank you!
Hi Gabby, I'm so glad you think so. Please subscribe if you have not already. Thanks!😊
What if its equal amounts, not product favored or reactant favored? Is it just k=1?
Hi Kate, That means you have both equal rates and equal concentrations. Thanks!
You are a lifesaver. Thank you.
Hi Absolutely, I’m glad it helped! I hope your class goes well😁
Thank you so much, I really like the way you teach!
Hi Suika, I’m so glad my style connects with you. I hope your class goes well!!😊
Thanks you so much for the video
You’re welcome. I hope your class goes well😊
How would you do this if you were not given the K value
Hi Bethany, the only other way is to be given concentrations at equilibrium and plug them into the equilibrium expression to calculate K. Other qualitative clues for product favored: a positive standard reduction potential or a negative Gibb’s free energy (and vice versa for a reactant favored reaction). I hope that helps. Thanks! Please subscribe if you haven’t already!😊
I am also chemistry teacher
Wonderful! Thank you for working with young people and sharing the beauty of chemistry! God bless you in your efforts:)
Hey! maam how are you?!
Thank you so much maam
Lotsssss of love from India🇮🇳
HI Sakshi:) I hope thing are going well. Good job working so hard! I am also sending love from the USA:)
@@OldSchoolChemistry 😀👍
I am struggling so much with acid and bases and your video was the only one that actually made me understand, thank you so so much!
Hi Ana! That makes me so happy. Thank you for sharing with me. I am very proud of your extra work!! You will do great in your class:)
The fact thag she replies every single comment is soooo sweet...mam your teaching is great...
Hi Veena, I so appreciate comments and enjoy interacting with my viewers. I am glad the videos have been helpful. Thank you for commenting!!
fantastic teacher
Hi Curtis, thank you for that vote of confidence:)
We have 2 mols of NH3 and 4 mols of gaseous reactants in the first reaction. How is k >1?
Hi Nolimitderrick:) You will know k>1 if 1. There are more products than reactants at equilibrium or 2. The delta G (Gibbs Free Energy) is negative. You can figure out G if you know H and S. This reaction is exothermic (spontaneous for enthalpy) but becomes more ordered (nonspontaneous for entropy). If you are only given the equation I think you need to google more information to identify that it is product favored. Was more information given in the question? That could give you clues. I hope your class goes well!