Collision theory estimates a gas-phase reaction rate by combining encounter frequency with energetic and geometrical requirements for reaction. For distinct hard spheres with contact separation , the collision cross section is , and the mean relative speed is . A reactive barrier and orientation restrictions reduce the fraction of collisions that react.
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Collision theory is a fundamental concept in chemistry that explains how chemical reactions occur. According to this theory, for a reaction to take place, the reactant molecules must collide with each other. However, not all collisions lead to a reaction; specific conditions must be met. Here are the key components of collision theory: 1. **Collision Requirement**: Reactant particles must collide for a chemical reaction to occur. The rate of reaction increases with the frequency of collisions.