Apply collision theory to explain two reasons why increasing the temperature of a reaction by 10 K often doubles the reaction rate?
1 Answer
Increasing temperature increases the rate at which molecules will move past the threshold level, the number of one-to-one collisions and the chance that when they colloid they will be in proper orientation.
Explanation:
The collision theory explains how reactions occur on the atomic level. It basically has 4 parts.
1. One-to-One collisions: Atoms react on a 1-to-1 basis.
2. Atoms must be in proper orientation when they collide or bonds will not be formed
3. Atoms must be moving at or beyond the Threshold Level threshold level has to do with speed. The atoms must be moving at a particular speed in order for the collisions to be effective.
4. Activation Energy is the push/energy needed for the reaction to occur.
By increasing the temperature, the molecules will increase in speed (threshold level), colloid more frequently, and if one collision is ineffective, perhaps the next will find the atoms in proper orientation.
