Search results
The equilibrium constant of a chemical reaction (usually denoted by the symbol K) provides insight into the relationship between the products and reactants when a chemical reaction reaches equilibrium. Learn about Kc and Kp here.
Key points. The equilibrium constant, K p. , describes the ratio of product and reactant concentrations at equilibrium in terms of partial pressures. For a gas-phase reaction, aA ( g) + bB ( g) ⇌ cC ( g) + dD ( g) , the expression for K p. is. K p = ( P C) c ( P D) d ( P A) a ( P B) b.
Aug 14, 2020 · An equilibrium constant calculated from partial pressures ( Kp) is related to K by the ideal gas constant ( R ), the temperature ( T ), and the change in the number of moles of gas during the reaction.
This page explains equilibrium constants expressed in terms of partial pressures of gases, K p. It covers an explanation of the terms mole fraction and partial pressure, and looks at K p for both homogeneous and heterogeneous reactions involving gases.
Nov 14, 2017 · Equilibrium constant Kp is equal to the partial pressure of products divided by partial pressure of reactants and the partial pressure are raised with some power which is equal to the coefficient of the substance in balanced equation.
We can convert between the two types of equilibrium constants using the formula: Kp = Kc (RT)^ (Δn), where R is the gas constant, T is temperature, and Δn is the change in gas molecules per reaction (Δn = moles of gaseous product moles – moles of gaseous reactant moles).
Jan 30, 2023 · This page explains equilibrium constants expressed in terms of partial pressures of gases, Kp. It covers an explanation of the terms mole fraction and partial pressure, and looks at Kp for both …
