[skylit]

I have this table of data I collected from an experiment, as follows:

Run 1---
Run 2:
[H2O2]AM,. MOL/L: 0.220 M
[I-]AM, MOL/L: 0.0417 M
ln[H2O2]AM: -1.51
ln[I-]AM: -3.18
RATE, kPa/s: 0.10405
ln(Rate): -2.2629

We were supposed to measure the rate of reaction using the initial rate method.
It asks me to SHOW how I calculated [H2O2]AM (After mixture), Mol/L for Run 2. My lab partner said the answer should be 0.220 M, as listed above. But I don't know how to get there. I know you have to use Rate=k[H2O2]p[I-]q, but I don't know what values to use. I think p and q are both equal to one, and so that is first order. But that's the extent of my knowledge. Help?

EDIT:
There's a lot of additional information for this lab, I'm not sure if I provided enough information to answer that I've asked. If I didn't please let me know.

[rabolisk]

I'm a little confused on exactly what you did for the experiment. Did you mix a solution of peroxide of known concentration and a solution of iodide of known concentration?

[skylit]

I'm a little confused on exactly what you did for the experiment. Did you mix a solution of peroxide of known concentration and a solution of iodide of known concentration?

"In this experiment, we will use potassium iodide, KI, to catalyze the decomposition, where the iodide ion, I^-(aq), acts as the catalyst."
We dispensed required amounts of H2O2 and KI solutions into a flask with DI water and collected pressure data using a computer interface.

Sorry if this is not sufficient..

[rabolisk]

Was the concentration of the solutions given? If so, then you are given the volume of solutions used, so you can calculate the initial concentration of each reagent after mixing.