Equilibrium pressure is the pressure at which a chemical reaction reaches a state of balance, where the rates of the forward and reverse reactions are equal.
Kp, or the equilibrium constant in terms of partial pressures, is a measure of the extent to which a reaction proceeds towards equilibrium at a given pressure. It is directly related to the equilibrium pressure, as Kp increases with increasing equilibrium pressure.
Kp can be calculated using the equilibrium expression, which is the ratio of the partial pressures of the products to the partial pressures of the reactants, each raised to the power of their respective coefficients in the balanced chemical equation.
The value of Kp is temperature-dependent, as it is affected by the enthalpy and entropy changes of the reaction. Generally, Kp increases with increasing temperature for endothermic reactions, and decreases with increasing temperature for exothermic reactions.
If the value of Kp is greater than 1, the reaction favors the formation of products at equilibrium. If the value of Kp is less than 1, the reaction favors the formation of reactants at equilibrium. If the value of Kp is equal to 1, the reaction is at equilibrium.