Sorry, I'm not sure I understand the question. There's no problem if the equilibrium constant is constant (i.e. doesn't depend on temperature). That will happen if ∆H is 0, as we can see from the van't Hoff equation in this video. At any particular temperature, the equilibrium constant (whether or not it varies with temperature) is just a particular value. That value determines how far the equilibrium lies between reactants and products.
Kind of a silly question but is this equation applicable for all reactions? I'm trying to solve a problem that includes dimerization but the values of Keq are stupidly big and I don't know if there is something wrong with the way I'm trying to solve it. All the others reaction Keq values are reasonable except that one.🤕
Yes, this equation is applicable for any equilibrium reaction. If the K value is very large, it might just mean the "equilibrium" reaction favors the products very strongly. If the reaction is essentially irreversible in the forward direction, the K will be large. (But also, be careful that you are talking about a unitless K when using this equation. The values of K_P or K_c, etc, will be different -- perhaps large or small -- when expressed in different units.)
thats actually brilliantly filmed, im guessing a glass sheet infront of him and then vertically flipping the video.
Good guess!
studio.ruclips.net/user/videoYmvJVkyJbLc
If the K is constant,how the equilibrium would be effected?
Sorry, I'm not sure I understand the question.
There's no problem if the equilibrium constant is constant (i.e. doesn't depend on temperature). That will happen if ∆H is 0, as we can see from the van't Hoff equation in this video.
At any particular temperature, the equilibrium constant (whether or not it varies with temperature) is just a particular value. That value determines how far the equilibrium lies between reactants and products.
Kind of a silly question but is this equation applicable for all reactions? I'm trying to solve a problem that includes dimerization but the values of Keq are stupidly big and I don't know if there is something wrong with the way I'm trying to solve it. All the others reaction Keq values are reasonable except that one.🤕
Yes, this equation is applicable for any equilibrium reaction.
If the K value is very large, it might just mean the "equilibrium" reaction favors the products very strongly. If the reaction is essentially irreversible in the forward direction, the K will be large.
(But also, be careful that you are talking about a unitless K when using this equation. The values of K_P or K_c, etc, will be different -- perhaps large or small -- when expressed in different units.)
@@PhysicalChemistry Thank you for taking the time to answer my question! Your advice is very much appreciated (and helpful!) :)