In the previous experiment (PART A) you studied the effect of concentration on the rate of reaction. Explain your observations using the collision theory

The collision theory states that for a reaction to occur, it is not enough for reactant particles to collide with each other. They must also have enough energy, known as the activation energy, when they collide to break the existing bonds and form new ones.

In the context of the experiment from Part A, where we studied the effect of concentration on the rate of reaction, the collision theory can explain our observations as follows:

1. Increasing the concentration of the reactants means there are more particles of reactant in the same volume. This increases the likelihood of particles colliding with each other.

2. Because there are more collisions, the chances that these collisions have enough energy to break the existing bonds and form new ones also increase. This means the reaction rate increases.

3. Conversely, if the concentration of the reactants is decreased, there are fewer particles in the same volume, leading to fewer collisions and a slower reaction rate.

So, according to the collision theory, the rate of a reaction is directly proportional to the concentration of the reactants: the higher the concentration, the faster the reaction rate, and vice versa. This is what we observed in our experiment.