Examkin

Question

Difficulty: EasyRate of Reaction and Collision Theory

According to the collision theory of chemical reactions, which of the following conditions must be met for a collision between reactant molecules to result in a successful chemical reaction?

  1. The colliding molecules must possess energy equal to or greater than the activation energy and collide with correct orientation.Answer
  2. B
    The colliding molecules must increase the overall equilibrium constant to favor product formation.
  3. C
    The collision must reverse the sign of the overall enthalpy change of the reaction.
  4. D
    Every collision between reactant particles results in product formation regardless of energy.

Answer

The colliding molecules must possess energy equal to or greater than the activation energy and collide with correct orientation.
According to collision theory, a chemical reaction occurs only when colliding particles possess a minimum threshold energy known as the activation energy (EaE_a) and collide with the appropriate spatial orientation to allow new bonds to form.

Step-by-Step Solution

1
Recall the fundamental postulates of collision theory.
Collision theory states that for a reaction to occur, reactant particles must collide with each other.
Physical contact is necessary for bond breaking and bond formation.
2
Identify the two necessary conditions for an effective (successful) collision.
1. Minimum kinetic energy equal to or exceeding the activation energy (EaE_a). 2. Proper relative orientation of colliding species.
Particles with insufficient energy bounce off each other without reacting, and incorrect orientation prevents the proper alignment of reacting bonds.

Key Concept

Collision Theory Criteria for Effective Collisions
Rate this question

Topics

Rate of Reaction and Collision Theory