Question

Which of the following statements is incorrect about the collison theory of chemical reaction?

(i) it considers reacting molecules or atoms to be hard spheres and ignores their structural features.
(ii) number of effective collisions determines the rate of reaction.
(iii) collision of atoms or molecules possessing sufficient threshold energy results into the product formation.
(iv) molecules should collide with sufficient threshold energy and proper orientation for the collision to be effective

Answer 1

The collision theory of chemical reaction states that molecules must collide with sufficient threshold energy and proper orientation for a reaction to occur.

Step-by-step explanation:

The collision theory of chemical reaction states that in order for a reaction to occur, molecules must collide with sufficient threshold energy and proper orientation. This means that the reacting particles can only form products when they collide with enough kinetic energy and in the correct orientation.

One statement that is incorrect about the collision theory is that molecules should collide with sufficient threshold energy and proper orientation for the collision to be effective. In reality, even if molecules collide with enough kinetic energy and the correct orientation, they may still not react due to the presence of other factors such as steric hindrance or unfavorable reactions.

In summary, the collision theory of chemical reaction emphasizes the importance of collision energy and orientation in determining the effectiveness of a reaction, but it is important to note that other factors can also influence the reaction outcome.