Collisions between reacting particles are therefore more likely to occur.
The graph for concentration shows that when the concentrations were relatively
low (10, 15, 20 g/dm3), the increase of rate x1000 was also fairly small
(increasing from 4.47 to 6.71 to 9.47). There was then a gradual increase in
the difference, and between 30 and 35 g/dm3 the rate more than doubled from
17.90 to 37.56s-1. This shows that there are far more collisions at a
concentration of 35 g/dm3 than at 30 g/dm3.
The graph plotting time against the rate of reaction x1000 shows that the
difference of rate between increasing temperatures (excluding the anomaly of
30°C) was pretty much regular, increasing in steps of 6-10 (9.17 to 15.37 to
24.28 to 31.67). However, once again there is a giant gap in the last
temperature increase ? at 60°C the RoR x1000 is 31.67 s-1, and at 70°C it is
57.03 s-1.
For this to fully make sense it is necessary to recap the collision theory
briefly:
For a reaction to occur particles have to collide with each other. Only a small
percent result in a reaction. This is due to the energy barrier to overcome.
Only particles with enough energy to overcome the barrier will react after
colliding. The minimum energy that a particle must have to overcome the barrier
is called the activation energy, or Ea. The size of this activation energy is
different for different reactions. If the frequency of collisions is increased
the rate of reaction will increase. However the percent of successful
collisions remains the same. An increase in the frequency of collisions can be
achieved by increasing the concentration, pressure, or surface area.