6 Difference Between Static And Dynamic Equilibrium In Chemistry

SHARE

What Is Static Equilibrium?

Static equilibrium is an equilibrium that occurs when all particles in the reaction are at rest and there is no motion between reactants and products. Static equilibrium occurs when there is no exchange between reactants and products. The process is in static equilibrium if you have a reaction that can occur in only one direction, you can reach equilibrium once you have used up the limiting reagent. In static equilibrium, the rates of the forward and reverse reactions are zero.

An example of static equilibrium is diamond turning into graphite.  Graphite is more stable than diamond but the activation energy is so high that you must heat diamond to about 2000oC before you can see any diamond converting to graphite.

What You Need To Know About Static Equilibrium

  1. Static equilibrium is an equilibrium that occurs when all particles in the reaction are at rest and there is no motion between reactants and products.
  2. In static equilibrium, both the rate of forward and backward reaction is zero.
  3. Static equilibrium can occur in both open and closed systems.
  4. Static equilibrium gives an indication that there is no further chemical reaction in the system.
  5. The nature of this type of equilibrium is that, it is irreversible.
  6. Static equilibriums are more often applied within a mechanical context rather than a chemical context.

What Is Dynamic Equilibrium?

Dynamic equilibrium is an equilibrium that occurs when a particular chemical system can proceed in both the forward and reverse directions at the same time. The overall concentration of the chemicals in this system will remain constant at equilibrium providing the conditions (temperature, pressure, and composition) are not altered. However, this does not mean that the reaction has stopped but continues to form products at exactly the same rate at which the products recombine to form the original chemicals.

What You Need To Know About Dynamic Equilibrium

  1. Dynamic equilibrium is an equilibrium that occurs when the rate of formation of product and the rate of decay of product back to reactant is same.
  2. In dynamic equilibrium, the rates of forward and backward reaction rates are equal.
  3. Dynamic equilibrium can only occur in closed systems.
  4. Dynamic equilibrium gives an indication that products and reactants are still participating in chemical reactions.
  5. The nature of this type of equilibrium is that, it is reversible.
  6. Dynamic equilibriums are more often applied within a chemical context.

Difference Between Static And Dynamic Equilibrium In Chemistry

BASIS OF COMPARISON STATIC EQUILIBRIUM DYNAMIC EQUILIBRIUM
Description Static equilibrium is an equilibrium that occurs when all particles in the reaction are at rest and there is no motion between reactants and products.   Dynamic equilibrium is an equilibrium that occurs when the rate of formation of product and the rate of decay of product back to reactant is same.  
Rate Of Forward And Backward Reaction In static equilibrium, both the rate of forward and backward reaction is zero.   In dynamic equilibrium, the rates of forward and backward reaction rates are equal.  
Occurrence Static equilibrium can occur in both open and closed systems.   Dynamic equilibrium can only occur in closed systems.  
What It Indicates Static equilibrium gives an indication that there is no further chemical reaction in the system.   Dynamic equilibrium gives an indication that products and reactants are still participating in chemical reactions.  
Reversibility The nature of this type of equilibrium is that, it is irreversible.   The nature of this type of equilibrium is that, it is reversible.  
Application Static equilibriums are more often applied within a mechanical context rather than a chemical context.   Dynamic equilibriums are more often applied within a chemical context.  

Comments are closed.