KP=KC (RT) ^∆ng
where ∆ng= difference in gaseous compounds of products and reactants
This is the simplest equation relating KP and KC.

Types of Equilibrium
Equilibrium is a state in which opposing forces or influences are balanced. In the context of chemistry, there are two main types of equilibrium: static equilibrium and dynamic equilibrium.

Static Equilibrium
Static equilibrium refers to a system where the reactions have come to a stop. This means that the concentrations of reactants and products remain constant over time. There are two main types of static equilibrium: stable equilibrium and unstable equilibrium. In stable equilibrium, a system will return to its original state if disturbed. In unstable equilibrium, a small disturbance can cause the system to move away from its original state.

Dynamic Equilibrium
Dynamic equilibrium occurs when the rate of the forward reaction is equal to the rate of the reverse reaction. In dynamic equilibrium, the concentrations of reactants and products are constantly changing, but the overall concentrations remain constant. This type of equilibrium is often seen in reversible reactions.

Relation between KP and KC
The equilibrium constant, K, can be expressed in terms of either partial pressures (KP) or concentrations (KC) depending on the nature of the reaction. For reactions involving gases, KP is used, while for reactions involving aqueous solutions or solids, KC is used. The relationship between KP and KC is given by the equation:
KP = KC(RT)^(Δn)
Where R is the ideal gas constant, T is the temperature in Kelvin, and Δn is the difference in the number of moles of gaseous products and reactants. This equation shows that KP and KC are related by the value of Δn and the temperature of the reaction.
In conclusion, understanding the different types of equilibrium and the relationship between KP and KC is essential in the study of chemical reactions and their behavior in different conditions.