Iodine clock reactions also known as Landolt Clock Reactions are one of many types of reactions in Chemistry. Clock reactions are an appealing way to show different type of chemicals having a reaction towards each other. This type of chemical reaction shows the demonstration of chemical kinetics. Iodine clock reactions were discovered by Swiss chemist Hans Heinrich Landolt in 1886. The procedure of conducting an iodine clock reaction consist of two colourless chemicals being mixed together. After a short period of time the two colourless chemicals will react with each other causing there to be a colour change in the solution, knows as a clock reaction, considering that over time the chemicals will react. The usual colour of the change that
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Reaction rates show the effect that the different chemicals have on each other whether they are highly reactive together, if so the reaction rate would be higher and faster. On the other hand if the chemical reaction has a slow rate of reaction the chemicals don’t have a very large effect on each other, therefore causing the rate of reaction to be slower. Reaction rate also known as the speed or reaction is defined for a product or reactant of how fast or slow the reaction takes place. For example the rusting of a metal could take years to complete, therefore having a slow rate of reaction. However, the burning of wood is almost instant therefore having a fast rate of reaction.
Concentration plays another part in the reaction in the iodine clock reaction experiments. Concentration is known as the amount of substance per defined space of the chemical. g/cm3 or kg/l The most important concentration to take into consideration when working with an iodine clock reaction is molarity (molar concentration). Molarity is the measure of concentration of a solute in a solution. Solute is a small component of a chemical reaction or any chemical procedure that is used to react with another …show more content…
0.05 M KIO3 & 0.1 Na2S2O5 →exceeded 5 min limit
0.05 M KIO3 & 0.1 Na2S2O5 →exceeded 5 min limit
0.4 M Na2S2O5 and 0.1 M KIO3 →10.7 seconds
0.4 M Na2S2O5 and 0.1 M KIO3 →12.03 seconds
0.4 M Na2S2O5 and 0.1 M KIO3 →12.82 seconds
0.4 M Na2S2O5 and 0.1 M KIO3 →11.31 seconds
0.2 M Na2S2O5 and 0.1 M KIO3 →32.25 seconds
0.2 M Na2S2O5 and 0.1 M KIO3 →29.03 seconds
0.2 M Na2S2O5 and 0.1 M KIO3 →31.35 seconds
0.2 M Na2S2O5 and 0.1 M KIO3 →28.69 seconds
0.1 M Na2S2O5 and 0.1 M KIO3 →1.58.62 mins
0.1 M Na2S2O5 and 0.1 M KIO3 →2.18.12 mins
0.1 M Na2S2O5 and 0.1 M KIO3 →2.16.16 mins
Copper (II)aq
30.97 seconds
30.78 seconds
30.56 seconds
Iron (II)aq
Instantaneous (0.25 seconds)
Instantaneous (0.25 seconds)
Instantaneous (0.16 seconds)
Solid
Reaction rates show the effect that the different chemicals have on each other whether they are highly reactive together, if so the reaction rate would be higher and faster. On the other hand if the chemical reaction has a slow rate of reaction the chemicals don’t have a very large effect on each other, therefore causing the rate of reaction to be slower. Reaction rate also known as the speed or reaction is defined for a product or reactant of how fast or slow the reaction takes place. For example the rusting of a metal could take years to complete, therefore having a slow rate of reaction. However, the burning of wood is almost instant therefore having a fast rate of reaction.
Concentration plays another part in the reaction in the iodine clock reaction experiments. Concentration is known as the amount of substance per defined space of the chemical. g/cm3 or kg/l The most important concentration to take into consideration when working with an iodine clock reaction is molarity (molar concentration). Molarity is the measure of concentration of a solute in a solution. Solute is a small component of a chemical reaction or any chemical procedure that is used to react with another …show more content…
0.05 M KIO3 & 0.1 Na2S2O5 →exceeded 5 min limit
0.05 M KIO3 & 0.1 Na2S2O5 →exceeded 5 min limit
0.4 M Na2S2O5 and 0.1 M KIO3 →10.7 seconds
0.4 M Na2S2O5 and 0.1 M KIO3 →12.03 seconds
0.4 M Na2S2O5 and 0.1 M KIO3 →12.82 seconds
0.4 M Na2S2O5 and 0.1 M KIO3 →11.31 seconds
0.2 M Na2S2O5 and 0.1 M KIO3 →32.25 seconds
0.2 M Na2S2O5 and 0.1 M KIO3 →29.03 seconds
0.2 M Na2S2O5 and 0.1 M KIO3 →31.35 seconds
0.2 M Na2S2O5 and 0.1 M KIO3 →28.69 seconds
0.1 M Na2S2O5 and 0.1 M KIO3 →1.58.62 mins
0.1 M Na2S2O5 and 0.1 M KIO3 →2.18.12 mins
0.1 M Na2S2O5 and 0.1 M KIO3 →2.16.16 mins
Copper (II)aq
30.97 seconds
30.78 seconds
30.56 seconds
Iron (II)aq
Instantaneous (0.25 seconds)
Instantaneous (0.25 seconds)
Instantaneous (0.16 seconds)
Solid