April 15, 2013
Lab Experiment 4
Explain how increasing the temperature causes reactions to happen quicker.
A brief comment on the magnitude of the activation energy ( E a ) – needs at
least one properly cited source.
A significant source of error would be the temperature variations during the
course of the chemical reaction between Oxalic Acid and Potassium
Permanganate. The temperature of the solution directly impacts the reaction
rate. This means the time it takes for the reaction to occur could easily vary
from trial to trial, which would make it difficult to obtain an accurate value for
the average time, and thus produce an inaccurate value for ln(k).
Increasing the temperature of the reaction increases the reaction rate due to the
fact that an “activation barrier” must be overcome for the reaction to take
place. By increasing the temperature under which a reaction occurs, you
increase the energy of the particles that are reacting and thus increase the rate
at which they collide with one another. When the particles collide more
frequently, the reaction will occur at a faster rate. By inc