Help with reaction orders and rates please!

From: Istari (newt_jedi_at_yahoo.com)
Date: 11/27/04 

Date: 27 Nov 2004 13:54:30 -0800

Hey,

I'm in first year college and I'm having some trouble with my
chemistry lab. I reacted varying amounts of HCL, acetone and iodine
with water in 4 different systems (20 ml of one, 10 ml of all the
others) and recorded the reaction times. I then calculated the
reaction rates of all four systems (negative change in [I2]/time), and
also the initial concentrations of the HCl, acetone and iodine. Now I
must find the reaction orders of each of the above by using the
equation:

rate 2/rate 1 = k[acetone]2^m[I2]2^n[H+]2^p/k[acetone]1^m[I2]1^n[H+]1^p

In [acetone]2^m, for example, the 2 just symbolizes that it is system
2 (I think). This equation then burns down to:

rate 2/rate 1 = (2[x]1)^m/[x]1^m = 2^m

For example, if I wanted the order of reaction for acetone, rate 2
would be the system where acetone was 20 ml, and rate 1 would be the
system where they were all 10 ml, except for water (20 ml). 'X', of
course, would be the initial concentration of acetone in each system.
I should basically get values close to integers like 1, 2, 3, and I
get almost exactly 1 for my acetone. My problem is, the values for the
orders of iodine and HCL are 0.4 and 1.2 respectively. I don't even
know if 0 is possible as a reaction order! Hopefully I'm doing
something stupid, yet simple to fix. Help would be very appreciated.

Thanks

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