Yes, several times.
It says "For each experiment, determine the initial rate of reaction. That is convert the volume, or mass, or increase in pressure of O2 within the time interval to get an initial rate of mol O2/(L*S). Using the stoichiometry of the reaction, convert this initial rate to a rate of decomposition of H202 in mol/(L*S)".
There are 2 questions here. Find the intial rate for O2, then using this rate, stoichiometrically determine the rate of decomposition of H202 which would be double.
I'll try and explain the lab. All trial are independant from each other. That is, they are different concentrations they are left to react for the same time. But it is not one experiment recording at different times, it is 7 different experiments with different concentrations and each 10 seconds. What the lab wants me to do is figure the initial rate for each experiment using the data of volume recorded, with units mol/(L*S). Then I graph the initial rates where H202 is constant and determine what order the reaction is regarding NaI, and vice versa. I can do ALL of this else except I don't know how I am supposed to find the initial rates with the volume of O2 into mol/(L*S). I can get ml/S or mol/S but not mol/(L*S).
Maybe my first attempt was correct when I changed to moles, then to concentration, and divided by time?
The data I have is the volume and concentration of H202 and NaI, and the volume of O2 recorded.
Thanks
to clarify, the concentration was changed manually, as an independant variable to see what affect it would have on the amount of oxygen produced (dependant variable).
