Question

A certain reaction is described as $A+B\to C$.
Just because a molecule of $A$ collides with a molecule of $B$, this does not necessarily result in the formation of a molecule of $C$.
Which of the following choices best describes the factor or factors that help to determine whether or not a molecular collision between $A$ and $B$ will result in the formation of product $C$?

• A. Molecules of $A$ and $B$ must have the proper orientation when they collide with each other.
• B. Molecules of $A$ and $B$ must have enough energy to overcome the activation energy barrier.
• C. Molecules of $A$ and $B$ must have enough energy to overcome the activation energy barrier and they must have the proper spatial orientation.
• D. For there to be a successful collision, molecules of $A$ and $B$ must be in the gas phase when they collide with each other.

Answer 1

The correct option is A Molecules of $A$ and $B$ must have the proper orientation when they collide with each other.

$A+B⟶C$
According to collision theory, for a reactant to from product, the reactants must collide each other with proper orientation.

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