Astudent 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

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. 

Sorry i don’t know answer to this