# Chemical Equilibria

- Page ID
- 9725

- Balanced Equations and Equilibrium Constants
- In a balanced chemical equation, the total number of atoms of each element present is the same on both sides of the equation. Stoichiometric coefficients are the coefficients required to balance a chemical equation. The coefficients relate to the equilibrium constants because they are used to calculate them.

- Calculating an Equilibrium Concentration
- To calculate an equilibrium concentration from an equilibrium constant, an understanding of the concept of equilibrium and how to write an equilibrium constant is required. Equilibrium is a state of dynamic balance where the ratio of the product and reactant concentrations is constant.

- Calculating An Equilibrium Concentrations
- Balanced Equations And Equilibrium Constants
- Calculating an Equilibrium Constant Using Partial Pressures
- Effect Of Volume Changes On Gas-phase Equilibria
- Writing Equilibrium Constant Expressions Involving Gases
- Gas Equilibrium Constants: Kc And Kp
- The Equilibrium Constant, K
- Writing Equilibrium Constant Expressions Involving Solids and Liquids

- Difference Between K And Q
- Sometimes it is necessary to determine in which direction a reaction will progress based on initial activities or concentrations. In these situations, the relationship between the reaction quotient, Qc , and the equilibrium constant, Kc , is essential in solving for the net change. With this relationship, the direction in which a reaction will shift to achieve chemical equilibrium, whether to the left or the right, can be easily calculated.

- Dissociation Constant
- Page notifications Off Share Table of contents The dissociation constant specifies the tendency of a substance AxBy to reversibly dissociate (separate) in a solution into smaller components A and B.

- Effect of Pressure on Gas-Phase Equilibria
- Le Chatelier's Principle states that a system at equilibrium will adjust to relieve stress when there are changes in the concentration of a reactant or product, the partial pressures of components, the volume of the system, and the temperature of reaction.

- Kc
- This page defines the equilibrium constant and introduces the equilibrium constant expressed in terms of concentrations, Kc. It assumes familiarity with the concept of dynamic equilibrium, as well as the terms "homogeneous" and "heterogeneous" as applied to chemical reactions. The two types of dynamic equilibria (homogeneous and heterogeneous) are discussed separately below, because the equilibrium constants are defined differently.

- Kp
- 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 homogeneous and heterogeneous reactions involving gases. The page assumes that you are already familiar with the concept of an equilibrium constant, and that you know about Kc - an equilibrium constant expressed in terms of concentrations

- The Equilibrium Constant
- Yhe equilibrium constant, K, expresses the relationship between products and reactants of a reaction at equilibrium with respect to a specific unit. There are two different types of equilibrium reactions: (1) heterogeneous and (2) homogeneous. This article illustrates the difference between the two, explains how to write equilibrium constants for both, and introduces the calculations involved with both the concentration and the partial pressure equilibrium constant.