Question

question 10 (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, when the concentration of reactants increases, there are more reactant particles in a given volume. This leads to a higher frequency of collisions between the particles. More collisions mean a greater chance of effective collisions (those with proper orientation and sufficient energy to overcome the activation energy), thus increasing the reaction rate.

• Collisions becoming more effective is related to factors like orientation (not concentration directly).
• Activation energy decrease is usually due to catalysts, not concentration.
• Average kinetic energy increase is related to temperature, not concentration.
• Molecules speeding up is also a temperature - related effect (kinetic - molecular theory, average kinetic energy \(E_{k}=\frac{3}{2}kT\), where \(k\) is Boltzmann's constant and \(T\) is temperature).

Answer:

The number of collisions increases.