Therhelp modynamics and the equilibrium constant

[mcato_O]

Therhelp ! modynamics and the equilibrium constant

Thermodynamics and the equilibrium constant

Okay I have a question about the equation (* means change) (*() means stander condition) so [G=*(G)+RT ln (Keq)] or just equation *(G)= - RT ln(Keq)
So what dose the (Keq) stander for? Kc? Kp? Ksp?? Kf or Kd

Is it always Kc regardless the chemical reaction? (that’s what my prof told me)
And then use the equation Kp=Kc (RT)^*n to convert K value?

Or is does Keq depends on the chemical reaction Kc for solution Kp for Gas?(from the textbook)

And can someone please derived the equation [G=*(G)+RT ln (Keq)] for me?
Where is it come from and why does it makes sense?

 

[GCT]

The derivation is a bit extensive, and you'll have to cover some ground in Physical Chemistry before you can make sense out of this particular topic.

The Kc,Kp,Ksp,Kf,Kd are the equilibrium constants with respect to the concentration Kc, and pressure Kp; the rest are specific forms uniquely suited to the reaction dynamics. That is, they be in terms of the concentration or pressure. Ksp is in reference to the solubility, Kf to complex ion formation, Kd to dissociation.

 

[Blueshift5]

I can provide some insight into your question about thermodynamics and the equilibrium constant. The equilibrium constant, represented by Keq, is a key concept in thermodynamics that relates to the balance of forward and reverse reactions in a system at equilibrium. It is a measure of the ratio of products to reactants at equilibrium and is used to determine the direction and extent of a chemical reaction.

The value of Keq is dependent on the temperature and pressure of the system and can be expressed in different forms, such as Kc for concentration, Kp for partial pressure, Ksp for solubility, Kf for formation, and Kd for dissociation. Which form to use depends on the specific chemical reaction being studied. For example, if the reaction involves gases, the equilibrium constant would be expressed as Kp, while for reactions in aqueous solutions, Kc would be used.

The equation you mentioned, [G=*(G)+RT ln (Keq)], is known as the Gibbs free energy equation and is derived from the fundamental principles of thermodynamics. It relates the change in free energy (∆G) of a system to the equilibrium constant (Keq) and the temperature (T). The negative sign indicates that the change in free energy is always in the direction of the equilibrium state, which is the state of lowest free energy.

In summary, the equilibrium constant is a fundamental concept in thermodynamics that helps us understand the behavior of chemical reactions at equilibrium. Its value depends on the specific reaction being studied and can be expressed in various forms. The Gibbs free energy equation provides a mathematical relationship between the equilibrium constant, temperature, and free energy change. I hope this helps clarify your understanding of thermodynamics and the equilibrium constant.