Chemical Kinetics Essay
An iodine clock reaction is a common example of a complex non-linear …show more content…
2013). By increasing the concentration of a chemical (which can be done either by diluting the remaining chemicals in a solution, or by increasing the moles of the specific chemical), the number of total collisions will increase, therefore meaning there is a higher chance of effective collisions occurring. Due to the increased occurrence of collisions, and likewise effective collisions, the rate of such a reaction will increase also. This is proven according to the collision theory, which says reaction rates happen due to frequent collisions. (Kinetics: Factors Affecting Reaction …show more content…
The R^2 value is close to 1, meaning that the data can be modelled by an exponential function.
With respect to the increase in temperature, Le Chatelier’s Principle can explain the increase in the reaction rate. This principle says that as the temperature is increased, the position of the equilibrium is shifted to the right. This is because heat is being absorbed into the solutions. However, when the temperature decreases the equilibrium shift is to the left, as heat is vacuumed out of such reactants. This is why the rate of reaction is able to increase or decrease according to temperature change.
The use of rate laws further proved what was initially hypothesised concerning concentrations. Using the rate law, the rate of the first reaction that was observed in experimentation was determined. This was done because the first reaction is the rate determining reaction. After further calculations it was found that as the concentration of both hydrogen peroxide and potassium iodide increased, so did the rate of reaction. This is seen in the following rate values:
1. Concentration 0.88mol/L →3.265 ×〖10〗^(-5)