Equilibrium Constant
The equilibrium Constant of any chemical reaction can be described as the ratio of the concentration of the products to the concentration of the reactants. It is denoted by K or KC. It is useful in determining the chemical behavior as well as the direction of the reaction.
Equilibrium Constant Formula
The equilibrium constant of a chemical reaction can be calculated by the concentration of products and reactants.
Suppose the Chemical Reaction is,
aA + bB ⇌ cC + dD
For this, the equilibrium constant can be given by:
KC = ([C]c × [D]d)/ ([A]a × [B]b)
where,
- Kc is Equilibrium Constant
- C ,D is Concentration of Formed Products
- A, B is Concentration of Involved Reactants
- c, d, a, b is Respective Moles of Product and Reactants Involved in Equation
- If Value of Kc is less than 1, it indicates more reactants in the mixture
- If Value of Kc is more than 1, it indicates the formation of products is more
Chemical Equilibrium
Chemical Equilibrium is a condition of a reversible chemical reaction, where the rate of forward and backward reactions are equal. In Chemical equilibrium, the concentrations of the products and reactants remain constant i.e. it does not change with time. This is a state after which there are no observable changes in the properties and the system becomes constant. In this state, the forward reaction proceeds at the same rate as the reverse reaction.
In this article, we will learn more about chemical equilibrium, its types, its examples, and more, so Let’s get started.
Table of Content
- What is Chemical Equilibrium?
- Types of Chemical Equilibrium
- Conditions for Chemical Equilibrium
- Factors Affecting Chemical Equilibrium
- Equilibrium constant
- Importance of Chemical Equilibrium
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