9-Hydration Investigation

Aim
The aim of this investigation was to experimentally determine the order and rate law expression of the reaction between sodium iodide and iron (III) nitrate 9-hydrate.

Introduction
The most interesting topic in grade twelve chemistry was the unit on kinetics, therefore after brainstorming a mind map on the stimulus that I chose, I was interested in creating an experiment to determine the order and rate law expression between two reactions myself. The original idea for this project came from a lesson on the order of reactions and rate law expressions. After learning the basics of how to express rates and how to do calculations involving rates in class, I did some extra research to fully understand the topic. In order to create a more complex

This does not occur with every collision, so certain methods are used to increase the probability of a successful collision, and thus increasing the rate of reaction. One of these methods is increasing the concentrations of the reactants. Increased concentrations results in particles colliding more frequently, and more successful collisions will occur. On a graph, there would be a decreasing curve as the concentrations of reactants decreases as the reaction

Controlled Variables
The variables which are controlled are the size of the beaker, the temperature and the volume of the solutions added, such as the distilled water, HCL, sodium iodide solution and the Iron (III) nitrate 9-hydrate solution. The volume must be controlled because each condition consisted of different concentrations of the reactants, the volume would differ in each one. Constant volume was kept to make sure that all conditions had the same number of moles of reactants. Reactions with smaller volumes may have reacted faster than those with larger volumes because successful collisions would occur more frequently. This was controlled by adding a sufficient amount of distilled water to each condition, so the volume stays consistent. The temperature must be controlled because it can affect the rate of reaction, if the temperature increases then the rate of reaction would also increase. To make sure that the temperature is consistent in each condition, this experiment was conducted in one period of time in the same room. Lastly, the size of the beaker needs to be the same because reactions in smaller beakers may occur more quickly than those in bigger beakers because there is more pressure. Therefore, when doing this experiment, the sizes of the beakers were the same. The environment also has to be controlled, the pressure,