Iodine Clock Reaction Essay

1354 Words 5 Pages
Usually, this state results when the forward reaction proceeds at the same rate as the reverse reaction. Chemical reactions vary greatly in the speed at which they occur. Some are essentially instantaneous, while others may take a very long time to reach equilibrium. The reaction is presented by The time in the reaction when the mixture remains colourless is the clock period. This will depend upon the initial concentrations of the sodium bisulphite ions (NaHSO3) and the potassium iodate ions (KIO3). If the concentration is increased

In a recent study developed by L.K.Brice of the Virginia Polytechnic Institute and State University, Blacksburg, Virginia found that there is a limit to the application of this relationship. The ratio of the
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Causing the increase of particles that then have enough kinetic energy to react when they collide.
This Landolt Iodine Clock reaction: Oxidation of Bisulphite by Iodate is to be investigated.

The aim of the experiment will be to discover whether a change in heat and concentration will increase the rate of reaction.

It is hypothesised that when the concentration and temperature increases it will cause the rate of reaction to speed up.

Firstly, The iodine clock reaction is a classic chemical clock demonstration experiment to display chemical kinetics. In the experiment the group varied two conditions being concentration and temperature to order to understand the rate of reaction more clearly. It was hypothesised that when the concentration and temperature increase will cause the rate of reaction to speed up. The data that was collected from the experimental investigation showed that it supported the hypothesis. The results showed the increase in the rate of reaction greatly when the concentration was increase to become more concentrated in moles. Then when the solution was heated and raise in temperature the rate of reaction caused more collisions and therefore the results showed that the speed of reaction was
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From the results it was clear that it supported our hypothesis the when the concentration was increased so was the time of the reaction. When there is a greater number of reactant molecules available to react, there will become a better chance of collision, in this study the more KIO3 that was present per unit volume, there were a better chance of successful collision to happen. An example of this in the test is where the molarity of KIO3 was 0.4M and the molarity of NaHSO3 was 0.1M the average time for the reaction was 0.96 seconds. But when molarity of KIO3 was 0.05M and the molarity of NaHSO3 was 0.1M (which is a weaker concentrations than the first example) the average time was 82.6 seconds which is 86 times slower than the fastest concentration tested. This is because of when you are cramming more particles into a given volume equaling more concentrated solution the reaction will take place over a quicker time. Looking at the effect of when the temperature was increased it decreases the rate of reaction by 7.6 times of what it was at the normal temperature. When the test was tested without the temperature incorporated the results where on average 3.75 seconds with the molarity of KIO3 being 0.25 M and the molarity of NaHSO3 being 0.5 M. Then when heat was added to

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