Chemistry · The effect of temperature on the rate of reactions, Arrhenius theory, activation energy and its calculation, collision theory of bi-molecular gaseous reactions (no derivation)
What are effective collisions? This question has multiple correct options
What are effective collisions? This question has multiple correct options
- A. Collisions leading to the transformation of reactants to products
- B. formation of activated complex
- C. collison between two reactant to decrease the activation energy
- D. collison between two reactant to overcome activation energy barrier
Step-by-step solution
An effective collision is defined as a collision between reacting particles that results in the formation of products. It requires sufficient kinetic energy to overcome the activation energy barrier and proper orientation of the colliding molecules. Options B, C, and D are incomplete or incorrect: B describes the activated complex, which is a temporary intermediate but not the defining characteristic; C is wrong because collisions do not decrease activation energy; D describes a necessary condition but not the complete definition of effective collisions, as proper orientation is also required. Therefore, A is the best choice.
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