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K, Kc and Kp: Chemical Engineering Work
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I am a little unclear on the distinction between K, Kc and Kp in chemical equilibria.
I am aware that you can write: Rate = Kc * Conc(A)^a * Conc(B)^b
I also know how to calculate Kc and Kp and that they can be related to each other through the Ideal Gas Equation.
What I am unclear of is whether I can use Kp in the above equation and how that would work. for example, would the following be true?
Rate = Kp * Partial Pressure(A)^a * Partial Pressure(B)^b
Lastly, how does K link to Kp and Kc?
With the Arrhenius Equation we can say: K = A*exp(-Ea/RT)
Would this be equally valid for Kp and Kc?
Thank you for your help and sorry if my thoughts are a little jumbled!
I am aware that you can write: Rate = Kc * Conc(A)^a * Conc(B)^b
I also know how to calculate Kc and Kp and that they can be related to each other through the Ideal Gas Equation.
What I am unclear of is whether I can use Kp in the above equation and how that would work. for example, would the following be true?
Rate = Kp * Partial Pressure(A)^a * Partial Pressure(B)^b
Lastly, how does K link to Kp and Kc?
With the Arrhenius Equation we can say: K = A*exp(-Ea/RT)
Would this be equally valid for Kp and Kc?
Thank you for your help and sorry if my thoughts are a little jumbled!
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#2
I think the first 'kay' you are referring to is k (the rate constant - lower case k) whereas Kc is the equilibrium constant in terms of concentrations ; Kp is the equilibrium constant expressed in terms of partial pressure of gases
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#3
Kc and Kp can be both used for gaseous mixtures. k from the rate equation describes completely different thing, it just happens to use the same letter as a symbol.
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#4
You are mixing up the Rate constant K with equilibrium constant Kc Kp
They are quite different. You cannot put Kc or Kp into the rate equation.
They are quite different. You cannot put Kc or Kp into the rate equation.
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