Catalysts are really important in chemistry. They help speed up reactions but don’t change where the reaction will end up, which is called equilibrium.
Here are some key points about how catalysts work:
Changing Energy Needs: Catalysts create a different path for the reaction that needs less energy. This can lower the energy needed by 20-40%.
Energy Examples: For instance, if a reaction usually needs 100 kJ/mol of energy to get started, a catalyst might reduce that need to somewhere between 60 and 80 kJ/mol.
Equilibrium Constant (K): Catalysts do not change the equilibrium constant, or K. This value only changes with temperature. So, adding a catalyst doesn’t affect K.
Reaction Speeds: Catalysts help speed up both the forward and backward reactions at the same time. This means they help reactions reach equilibrium faster.
Catalysts are really important in chemistry. They help speed up reactions but don’t change where the reaction will end up, which is called equilibrium.
Here are some key points about how catalysts work:
Changing Energy Needs: Catalysts create a different path for the reaction that needs less energy. This can lower the energy needed by 20-40%.
Energy Examples: For instance, if a reaction usually needs 100 kJ/mol of energy to get started, a catalyst might reduce that need to somewhere between 60 and 80 kJ/mol.
Equilibrium Constant (K): Catalysts do not change the equilibrium constant, or K. This value only changes with temperature. So, adding a catalyst doesn’t affect K.
Reaction Speeds: Catalysts help speed up both the forward and backward reactions at the same time. This means they help reactions reach equilibrium faster.