[sci0x]

Quick Question:

The formula for rate = k (reactant)^a [reactant]^b [reactant]^c

Now i do three experiments with

Experiment 1:
0.8mL Water,
0.8mL 2-butanol, 2M
0.8mL Sulfuric Acid, 1M
0.8mL Potassium Permanganate, 0.2M

Experiment 2:
All the same only I have 0.4mL Potassium Permanganate

Experiment 3:
All the same only I use 0.2mL Potassium Permanganate

Now I have to calculate the rate for each experiment:

So for experiment 1 is the rate:
k (reactant)^a [reactant]^b [reactant]^c

(0.8ml KMnO4)[2M 2-butanol][1M Sulfuric Acid]
= 1.6

But what values do I use for k and the exponents a, b and c?

[plu]

You can only find the rate of the reaction through experiment.  (i.e. indicators and a stopwatch)

[sci0x]

What about using time vs absorbance. I have graphs made out for each of these experiments.

[plu]

Great!  Now, you can make a rate vs. concentration graph (rate = change in concentration/time).  From that, you can deduce the initial rate of the three experimental reactions and thus the order of the reaction in respects to the three reagents.

[Donaldson Tan]

Quick Question:
The formula for rate = k (reactant)^a [reactant]^b [reactant]^c

what are the 3 reactants in the  rate equation?

I am not sure if you have sufficient data. there are 4 unknowns (a,b,c,k) and therefore you need 4 sets of experimental data to solve for each unknown.