Catalysts

• A catalyst can be used repeatedly to speed up many reactions.
• Catalysts are not consumed during the reaction, so they do not appear on the equation.
• Increasing the temperature increases the kinetic energy of particles, leading to more collisions with enough energy to react.
• An increase in surface area leads to an increase in the number of active sites where the reaction takes place.
• rate of reaction and equilibrium
• If the forward reaction is faster than the reverse reaction, then the overall reaction will proceed from left to right (product formation). If the reverse reaction is faster than the forward reaction, then the overall reaction will proceed from right to left (reactant formation)