Collision theory tells us that molecules need to collide in order for a reaction to take place. All else being equal, anything that increases the frequency of collisions would also increase the rate of reaction. One way to do this is to increase the concentrations of one or more of the reactants. Using a real world example, a busy freeway will experience much more frequent car collisions than a fairly empty neighborhood street. Similarly, forcing more randomly moving molecules into the same amount of space will cause an increased number of collisions over a given length of time, providing the reactants with more opportunities to transform into products.
Jordan and Elizabeth are performing a chemistry experiment for the science fair. Jordan uses a high concentration of the reactants when starting his reactions. Elizabeth uses a low concentration of the reactants when she starts her reactions.
Based on the above, answer the following question:
Who will have reactions with more frequent collisions between the reactant molecules?