[sanfonts]

Hello! I think you might be familiar with the Briggs-Rauscher reaction, where you mix 3 solutions and then they do oscillate between colorless-yellow-dark blue for a couple of minutes.

I thought this kind of reaction would be quite useful for measuring the effects of temperature over the duration of the oscillations.

Right after you mix the solutions, they turn into a yellow color, then blue, clear, yellow, blue...

So I decided to measure the time it takes for the solution to undergo the cycle blue-clear-yellow, and I restarted the chronometer the moment the solution turned into blue again.

So, let's say that for 20°C, I got the next data for the duration of one cycle: 13.09, 12.68, 12.15, 11.77, 11.5 and so on, averaging 12.24 seconds.  

My teacher said it was ok to calculate the rate of reaction only with the "general" reaction that acounts for one oscillation, that is to be said:

IO3- + 2 H2O2 + CH2(CO2H)2 + H+ --> ICH(CO2H)2 + 2 O2 + 3 H2O

If I know that the nominal concentrations of the reactants were:

0.050M for CH2(CO2H)2
0.067M IO3-
0.038M H2SO4
1.3M H2O2
0.0067M MN2+

Can I just assume that the overall rate of reaction was 1/(12.24) = 0.08170?

I wasn't told until a few days ago we were supposed to calculate rates of reaction (I thought comparing just the seconds would be more than enough), and I truly don't know how to calculate them. Could you please help me?

Thank you in advance,