Dynamic equilibrium happens in a reversible reaction when the speed of the forward reaction is the same as the speed of the backward one. This means that both reactions are occurring at the same time, and the amounts of reactants and products remain stable.

According to Le Chatelier's principle, if we change something in the environment, it can move the equilibrium position.

Factors that affect equilibrium:

1. Concentration:

   • If we add more reactants, the equilibrium will move to the right.
   • If we reduce the amount of products, it will move to the left.

2. Temperature:

   • For reactions that release heat (called exothermic reactions), raising the temperature will shift the equilibrium to the left.
   • For reactions that absorb heat (called endothermic reactions), increasing the temperature will shift it to the right.

3. Pressure:

   • If we increase the pressure, the equilibrium will shift toward the side with fewer gas molecules.
   • For example, in the reaction of nitrogen and hydrogen: ( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) )
     • If we increase the pressure here, it will shift to the right because there are 3 gas molecules on the left and only 2 on the right.

Understanding these factors helps us see how changes in conditions can affect reactions!