Hey can someone check if my understanding of the Collision Theory and how to increase reaction rates is accurate? Please feel free to edit/add/remove anything that is relevant to the VCAA course. Thanks!
Increasing concentration of reactants/ increasing pressure of gaseous reactant molecules:By increasing the concentration of reactants, there is an increase in the number of collisions between reactant molecules. As a result of the increased collision rate, there is an increase in the rate of the overall reaction.
Adding a catalyst:Catalysts lower the minimum quantum of energy required to disrupt bonds within reactant molecules. In the presence of a catalyst, the activation energy is lowered. As a result, a lower amount of energy must be absorbed by the bonds in the reactant molecules in order for the bonds to be broken. Once this has occured, the molecules which have absorbed the quantum of energy needed to activate the reaction collide with one another, increasing the rate at which the reaction occurs as collision rate increases.
Increasing temperature:By increasing temperature, the amount of kinetic energy available also increases. As a result, molecules collide more frequently with one another. As the collision rate increases, the overall rate of the reaction also increases.
Increasing surface area of solids:As surface area increases, the amount of the solid molecules exposed to other molecules' surfaces increases. As a result, there is a greater number of collisions between molecules at their surfaces. The increased collision rate leads to an increase in the overall reaction rate.
Help would be much appreciated. Thank you