What is Equilibrium?
In chemistry, equilibrium is the state in which both reactants and products are present at concentrations but have no tendency to change with time. This usually results in with a forward reaction that proceeds at the same time of a reverse reaction. This means that the rate is equal and there is no net changes in the concentrations of either the reactants or products.
Main Points of the Dynamic Equilibrium Theory
- At dynamic equilibrium, reactants are converted to products and products are converted to reactants at an equal and constant rate.
- Another way to explain dynamic equilibrium is that substances move between chemicals at an equal rate, meaning there is no net change.
- Dynamic equilibrium has the ability to be reversible.
- A reversible reaction is a reaction that can proceed in the direction of products to reactants
Why is Dynamic Equilibrium Important?
Dynamic equilibrium is important because it describes the behaviour of chemical reactions over time. Finding the equilibrium constant for a reaction is useful because it allows chemists to understand the reaction. Knowing the equilibrium constant because it allows you to calculate how much product will be formed. Dynamic equilibrium tells you how a particular mixture of chemicals will behave. This is because chemical reactions always occur in the direction that will make the ratio of the products and reactants equal to the equilibrium constant. This is known as Le Chatelier' Principle. (Please go to the Le Chatteliers page to learn more!)
If you would like to find out how dynamic equilibrium is important to biology, click here
If you would like to find out how dynamic equilibrium is important to biology, click here