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A student conducting the iodine clock experiment accidentally makes an s2o32- stock solution that is too concentrated. how will this affect the rate measurement? reaction 1: 3i- (aq) + s2o82- (aq) -> i3- (aq) + 2so42- (aq) slow reaction 2: i3- (aq) + 2s2o32- (aq) -> 3i- (aq) + s4o62- (aq) fast reaction 3: i3- (aq) + starch (aq) -> 3i- ---- starch (bluish black) fast

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Erythrosin17
Adding (S2O3)2- would affect the reaction mechanism that involves this ion. From the reaction mechanism given above, the equilibrium of step 2 would be affected. Adding the stock solution of (S2O3)2- would shift the equilibrium to the right thus making more products of the said mechanism. Also, the reaction rate of this step would occur faster than the original rate. This is based on Le Chatelier's Prinicple which states that a corresponding change would happen to the equilibrium of a reaction when pressure, concentration of the substances or temperature is changed. So, that after the addition, a color change would appear immediately because I3- would be removed slowly from solution, and would therefore be able to react with starch. 

A classical reaction that indicates the chemical kinetic of reaction is called iodine clock reaction and was given by Heinrich.

Thiosulfate ion when used in the concentrated form will affect the mechanism of the reaction. From the equations, we can say that step 2 will be affected.

[tex]\rm Step2: I_{3} (aq) + (2S_{2}O_{3})_{2} (aq) \rightarrow 3I (aq) + (S_{4}O_{6})_{2} (aq) \;fast \;reaction[/tex]

  • The addition of concentrated thiosulfate will shift the reaction equilibrium towards the right that will increase the product yield. The rate of reaction will also be affected and it will increase compared to the original pace.

  • When the concentration. pressure and temperature of a reaction are changed then the product formation will be affected due to specific principle.

  • This addition of thiosulfate will result in instant colour change as [tex]\rm I_{3}[/tex] will be removed and the reaction will occur at a fast pace.

To learn more about the iodine clock experiment follow the link:

https://brainly.com/question/16944311

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