Reposting since it wasn't clear in the previous post

S2O82-(aq) + 2I-(aq) ----------> 2SO42-(aq) + I2(aq) (I)

Rate = k [S2O82-]x [I-]y

Rate1 = k [S2O82-]x [I-]y

Experiment data
Experiment: 0.20M NaI,0.20M NaCl, 0.010M Na2S2O3,2% Starch,0.20M K2SO4, 0.20 M K2S2O8
Used 2ml = 20 drops of each solution for the experiment 1.
Time for Exp 2 and 3 are 101 sec and 96 seconds
Experiment2 20 drops 20 drops 20 drops 20 drops 0 drops 40 drops

Experiment3 40 drops 0 drops 20 drops 20 drops 20 drops 20 drops

Need help calculating these:

Calculated concentration of S2O82ƒ{ _______________ mol/L

Calculated concentration of Iƒ{ _______________ mol/L

Total elapsed time (ƒ´t) _______153sec

Rate of reaction _______________ M/sec
(from mathematical rate expression)

Rate constant, k _______________ sec-1

Calculated reaction orders (show work in lab report): x: _____ y: _____

Complete rate law (with orders): ______________________________

ignore f's in the question

To calculate the requested values, we will use the given experimental data and the mathematical rate expression:

Rate = k [S2O82-]^x [I-]^y

1. Calculating the concentration of S2O82-:
In Experiment 1, we used 0.010M Na2S2O3, which means the initial concentration of S2O82- is 0.010M.

2. Calculating the concentration of I-:
Since NaI and NaCl are both 0.20M in all experiments, the initial concentration of I- is also 0.20M.

3. Calculating the total elapsed time (Δt):
The total elapsed time is the sum of the individual experiment times, which is 101 seconds (Experiment 2) + 96 seconds (Experiment 3) = 197 seconds.

4. Calculating the rate of reaction:
The rate of reaction can be determined by dividing the change in concentration by the total elapsed time. However, we need additional information regarding the concentration changes or any observed changes in the amount of reactants or products.

5. Calculating the rate constant, k:
To calculate the rate constant, we need to use the rate expression and substitute the values from any of the given experiments, along with the corresponding rate of reaction. Without this information, we cannot calculate the rate constant.

6. Calculating the reaction orders:
The reaction orders, x and y, can be determined by comparing the rates of reaction at different concentrations of reactants. Unfortunately, the given experimental data does not provide different concentrations to determine the reaction orders.

7. Complete rate law (with orders):
Without the calculated reaction orders (x and y) and the rate constant (k), we cannot fully determine the complete rate law.

To accurately calculate the requested values, we need additional information regarding the concentration changes or any observed changes in the amount of reactants or products, as well as the rate of reactions at different concentrations.