Final answer:
Without the specific concentration data of iodine (I2), we cannot calculate the exact rate of the reaction from the time it took for the color to disappear. The average rate of a reaction is typically calculated with the formula ∆[I2]/∆t, but here we lack the concentration change ∆[I2], making the computation impossible from the provided information.
Step-by-step explanation:
To calculate the rate of the reaction where I2 color disappears in 1450 seconds, you would typically use the concentration change of I2 over that time period. The reaction rate is given by the change in concentration divided by the change in time. However, without the concentrations data, we cannot provide an exact rate. If the reaction follows a simple rate law, such as rate = k[I2], and we assume a pseudo-first-order reaction due to excess of other reactants, an approximation might be possible.
In general, to find the average rate you would take the initial and final concentrations of I2 (let's say [I2]initial and [I2]final) and use the formula: Average rate = ∆[I2]/∆t, where ∆[I2] is the change in concentration over the time interval ∆t. Since ∆[I2] is not provided in the question, this calculation cannot be completed.
To assess the rate at which the reaction has slowed down over time, one might compare it to earlier rates in the reaction, as indicated by provided tables or datasets. For example, using data like an initial rate of 2.0 × 105 M/h helps to contextualize whether the rate has decreased significantly over subsequent hours.