kinetics

• particles must collide with sufficient energy and correct orientation in order to react
• most collisions dont result in a reaction
• activation energy is the minimum energy that particles must collide with for a reaction to occur
• increasing temperature increases the rate of reaction because there are more particles with energy higher than the activation energy so there are more successful collisions
• increasing pressure increases the rate of reaction because there are more particles in a given volume so there are more frequent successful collisions
• a catalyst is a substance that increases the rate of reaction but is not used up in the reaction
• catalysts provide an alternative pathway and lower activation energy so more particles have enough energy to successfully collide