16 posts • Page 1 of 1
Some of the textbook problems for Outline 1 ask us to refer to Table 5G.2 to find the equilibrium constant for a certain reaction and use it to solve the problem. For each reaction, there is a K value and a Kc value listed in Table 5G.2 and I've noticed that the two values are sometimes different. How do we know when to use K and when to use Kc? Thank you!
Last edited by Samantha Pedersen 2K on Mon Jan 04, 2021 2:44 pm, edited 1 time in total.
In my understanding, K and Kc are almost interchangeable, but K is more general, while Kc is mainly used in the context of comparing concentrations. K can be used to cover both the equilibrium constant of concentrations, Kc, and the equilibrium constant of gas pressures, Kp. Dr. Lavelle with probably explain the difference more in detail in Wednesday's lecture when he explains how to calculate Kp. Hope this helps!
Hello! I think K and Kc are basically the same thing, both representing the equilibrium constant, but Kc is more specific. K can refer to concentration, pressure, etc., while Kc specifically refers to concentration. Hope this helps!
Like what all of the other posts say, they can be used interchangeably and basically are the same thing, but K is more general and Kc is referring to the concentrations. The c subscript is used to specify that the concentration is being used. I think in the next lectures, Dr. Lavelle will talk about other subscripts like p which refers to pressure.
I also agree with the posts above. Since the difference between the two is small, they can basically be considered the same or used interchangeably. Just depends on which specific concentration you need or what the question calls for.
I agree with the statements above but one thing to also keep in mind is that when calculating the equilibrium constant from thermodynamic tables of data (the standard gibbs free energy for example), you have to give K, not Kc.
Who is online
Users browsing this forum: No registered users and 1 guest