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Only two of these reactant concentration have a direct influence on the reaction rate Which two are they? In this experiment, you will determine the rate of an iodine clock reaction. The completion of this particular reaction is signalled by the sudden appearance of the dark-blue colour that is characteristic of the interaction of molecular iodine (I2) with starch. When the reaction is performed correctly, the blue colour appears so suddenly that it can be as startling as the sudden sound of an alarm clock, hence the title of the experiment. The rate of an iodine clock reaction depends on the concentrations of the reactants, as you would expect. Therefore, the time required for the appearance of the dark colour can be adjusted by adjusting the concentrations of the reactants (so one can set the “colour alarm” of a clock reaction just as you can set the sound alarm on a clock).You will study the rate of reduction of potassium persulfide (K2S2O8) by sodium iodide (NaI). The net ionic equation for this reaction is the following:S2O82– + 2 I - → 2 SO42– + I2 (1)The rate law for this reaction isRate = k [S2O82–]q [I -]
