Question

question 9 (1 point)
why does an increase in concentration increase the rate of reaction?
collisions become more effective.
the number of collisions increases.
the activation energy decreases.
the average kinetic energy increases.
when there are more molecules in the container, they all speed up.

Explanation:

According to the collision theory in chemistry, when the concentration of reactants increases, there are more reactant molecules in a given volume. This leads to a higher frequency of collisions between the molecules. A reaction occurs when molecules collide with sufficient energy (activation energy) and proper orientation. An increase in concentration mainly affects the number of collisions (not the effectiveness of collisions, activation energy, average kinetic energy of molecules, or making all molecules speed up). For example, in a reaction \(A + B
ightarrow products\), if we have more \(A\) and \(B\) molecules (higher concentration), there will be more \(A - B\) collisions.

Answer:

The number of collisions increases.