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The initial rate of the reaction is given as \( 79 \, \text{mM/s} \) in the table under the "Observations" section. Therefore, the initial rate for this trial is **79 mM/s**.

Would you like a further breakdown of the calculations involved in finding the initial rate? Or do you have any other questions?

Here are some follow-up questions related to the experiment:
1. How is the initial rate calculated in chemical kinetics?
2. Why is the reaction time important when determining the initial rate?
3. How does the concentration of each reactant influence the reaction rate?
4. What role does the temperature play in this experiment?
5. What causes the color change observed in the reaction?

**Tip:** The initial rate of a reaction can often be determined by measuring the concentration of reactants/products at very early time points when the reaction has just started.

Explore how to calculate the initial reaction rate from kinetics data, such as reactant concentrations and reaction time. This example involves iodine, hydrogen peroxide, and thiosulfate solutions, yielding an initial rate of 79 mM/s.

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