collision theory

Question

According to collision theory, the rate of reaction increases with temperature because:

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According to **Collision Theory**, the rate of reaction depends on two factors:
1. **Collision Frequency ($Z$)**: The number of collisions per unit volume per unit time. As temperature increases, molecules move faster, increasing $Z$.
2. **Effective Collisions**: Only some collisions result in a reaction. For success, the colliding molecules must have energy $\ge E_a$.
- According to the Maxwell-Boltzmann distribution, a small increase in temperature substantially increases the **fraction of molecules** that possess enough energy to cross the activation barrier.
- Both factors contribute, but the energy factor is much more significant.

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Collision theory requires effective collisions have: