How do I find the rate law? I did a iodine clock lab but i am having trouble finding the rate law equation as well as the slow and fast reactions. I used these materials:

Solution 1
o 1.0 grams Starch
o 10.0 mL of Acetic Acid
o 4.1 grams of Sodium Acetate
o Sodium Iodide 1, 2, 3
o 1.57 grams of Sodium Thiosulfate
Solution 2
500 mL of 3% Hydrogen Peroxide
500 mL of distilled water
500 mL beaker
I mixed the two solutions together and in the course of three trials I increased the sodium iodide concentration while other substances remained constant. Please help.

At the moment I am unable to post a link but if you will go to Google and type in rate law for i2 clock reaction, you should be able to go from there.

To find the rate law equation for a reaction, such as the iodine clock reaction you performed, you need to analyze the effect of changing the concentration of reactants on the reaction rate.

Here is a step-by-step guide to finding the rate law equation:

1. Determine the overall balanced equation for the reaction using the given materials and observations from your lab. It seems you mixed Solution 1 and Solution 2, but without more specific information, we cannot provide the balanced equation for your specific reaction.

2. Choose one reactant, let's say reactant A, and vary its concentration while keeping all other reactant concentrations constant. Perform multiple trials and measure the reaction rate for each trial.

3. Compare the reaction rates obtained from the trials and determine the effect of changing the concentration of reactant A. If the reaction rate doubles when the concentration of A doubles, the reaction is first-order with respect to A. If the reaction rate quadruples when the concentration of A doubles, the reaction is second-order with respect to A. And so on.

4. Repeat step 3 for each reactant to determine the order of the reaction with respect to each reactant.

5. Once you have determined the order of the reaction for each reactant, you can write the rate law equation. For example, if Reactant A is first-order and Reactant B is second-order, the rate law equation could be: Rate = k[A][B]², where k is the rate constant.

6. To find the overall order of the reaction, add up the individual orders obtained in step 5. For example, if the order of A is 1 and the order of B is 2, the overall order of the reaction would be 1 + 2 = 3.

7. Lastly, determine the slow and fast reactions. The slow step is the step that determines the overall rate of the reaction and is usually the step with the highest activation energy. The fast reactions occur in earlier steps and may be reversible or have lower activation energies.

Note: Without specific data from your lab, it is difficult to provide a more detailed explanation for your specific case. Make sure to record accurate measurements, perform multiple trials, and vary reactant concentrations systematically to obtain reliable rate data.