Which of the following is a postulate of collision theory?

• A. Reactant molecules must collide with sufficient energy to overcome the activation energy barrier.
• B. All collisions between reactant molecules result in the formation of products.
• C. Reaction rate is independent of the frequency of collisions between molecules.
• D. The orientation of molecules during a collision does not affect the reaction outcome.

Answer: (A)

Verified step by step guidance

1. Understand that collision theory explains how chemical reactions occur and why reaction rates differ for different reactions.
2. Recall that one key postulate of collision theory is that reactant molecules must collide to react, but not all collisions lead to a reaction.
3. Recognize that for a collision to be effective, molecules must collide with enough energy to overcome the activation energy barrier, which is the minimum energy required for the reaction to proceed.
4. Note that the orientation of molecules during collision is also important; molecules must be oriented properly for bonds to break and form, affecting the reaction outcome.
5. Conclude that the correct postulate is: Reactant molecules must collide with sufficient energy to overcome the activation energy barrier, while other options either contradict collision theory or are incorrect.