Final answer:
Increasing the concentration of S2O2−3 stock solution in the iodine clock experiment will increase the rate measurement. This is due to the principle behind the collision theory, indicating an increase in successful collisions thus hastening the reaction. This results in faster, potentially inaccurate rate measurements.
Step-by-step explanation:
If a student conducting the iodine clock experiment makes an S2O2−3 stock solution that is too concentrated, it will significantly affect the rate measurement in the experiment. Specifically, it will increase the rate measurement. This is because in chemical reactions, the concentration of the reactants directly influences the rate of reaction. A higher concentration of reactants means more molecules or ions are available to collide and form new products, thus increasing the frequency of successful collisions - this is the principle behind the collision theory, and it dictates that the rate of reaction will increase as the concentration of reactants increases. So if a more concentrated solution of S2O2−3 is used in the iodine clock experiment, the reaction will happen faster, thus increasing the rate measurement. This might result in time measurements that are shorter than they should be, making it difficult to plot accurate rate measurements.
Learn more about Chemical Reaction Rate