Chemical equilibrium

Chemical equilibrium is a state in a chemical reaction where the concentrations of the reactants and products have no net change over time. This occurs when the forward reaction rate equals the reverse reaction rate, leading to a constant composition of the system.

Overview

Chemical equilibrium is a dynamic state. Although the concentrations of reactants and products remain constant, the reactions continue to occur. This is different from a static equilibrium where no reactions occur. The concept of chemical equilibrium is fundamental in the field of chemistry, particularly in thermodynamics and kinetics.

Equilibrium constant

The equilibrium constant (K) is a measure of the ratio of the concentrations of products to reactants at equilibrium. It is a dimensionless quantity and is temperature dependent. The equilibrium constant provides valuable information about the position of equilibrium and the yield of products.

Le Chatelier's principle

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. This principle is used to predict the effects of changes in pressure, temperature, or concentration on the system at equilibrium.

Applications

Chemical equilibrium concepts are applied in various fields such as chemical engineering, biochemistry, environmental science, and pharmaceuticals. Understanding chemical equilibrium is crucial in these fields to control reactions for desired outcomes.

See also

• Reaction rate
• Reversible reaction
• Thermodynamics
• Kinetics

This article is a stub related to chemistry. You can help WikiMD by expanding it!

• 
  Diagram of chemical equilibrium
• 
  Aluminum hydrolysis process