The Relationship Between K and Kc for Chemical Reaction Equilibrium

What is the relationship between K and K c for the reaction N2(g) + 3H2(g) <--> 2NH3(g)?

Which of the following statements accurately reflects the connection between equilibrium constants K and Kc for the given reaction?

A. K = (RT)^6Kc

B. Kc = (RT)^-2K

C. Kc = (RT)^2K

D. K = (RT)^-2Kc

E. K = (RT)^2Kc

Answer:

The correct answer is option D: K = (RT)^-2Kc

The relationship between equilibrium constants K and Kc for the chemical reaction N2(g) + 3H2(g) <--> 2NH3(g) involves squaring the product of the ideal gas constant (R) and the absolute temperature (T). This relationship is depicted as K = (RT)^2Kc.

Equilibrium constant K is expressed in terms of partial pressures, denoted as Kp, while equilibrium constant Kc is expressed in terms of molar concentrations (mol/L). The ideal gas constant is represented by R and the absolute temperature by T.

This relationship allows us to connect the constants expressed in terms of partial pressures and molar concentrations, providing a method to relate the two equilibrium constants.

By understanding this relationship, we can gain insights into the equilibrium properties of chemical reactions and the factors that influence their balance. For further exploration on absolute temperature, refer to the provided link.