Question

Which of the following is not true about collisions that successfully convert reactants to products?

• A. In a reaction mechanism, successful collisions that occur more quickly are less likely to influence the overall rate of the reaction.
• B. These collisions are largely temperature independant if the proper catalyst is used
• C. Successful collisions must have sufficient energy to overcome activation energy barriers
• D. Successful collisions must have orientations that allow the molecules to rearrange in the correct manner.

Answer 1

Answer: (A)

In a reaction mechanism, successful collisions that occur more quickly are less likely to influence the overall rate of the reaction.

For successful conversion of reactants to products, the molecules must collide with proper orientation, the temperature should be high & the molecules should possess energy greater than activation energy.

While the rate of collisions (i.e. fast or slow) does not affect the conversion.

Therefore, option $\left(A\right)$ is the correct answer.