[slu1986]

The following set of data was obtained by the method of initial rates for the reaction:

     2HgCl2 + C2O4^2- ---> 2Cl- + 2CO2 + Hg2Cl2

 What is the rate law for the reaction?

  [HgCl2] (M)   [C2O4^2-] (M)       Rate (M/s)

   0.10                 0.10                1.3 * 10^-7
   0.10                 0.20                5.2 * 10^-7 
   0.20                 0.20                1.0 * 10^-6

A) Rate = k[HgCl2]^2 [C2O4^2-]^2
B) Rate = k[HgCl2][C2O4^2-]
C) Rate = k[HgCl2]^2[C2O4^2-]
D) Rate = k[HgCl2][C2O4^2-]^2


I am having some trouble understanding how to work this problem...Could someone please explain to me how to solve for the answer.  I know that you have to solve for m and then solve for n, but I don't quite understand the concept...So if someone could help me, I would appreciate it! Thanks

[Astrokel]

hey,

check this out: http://www.chemicalforums.com/index.php?topic=25958.msg98386#msg98386 (oberservation method)

alternatively,

r = k[HgCl₂]^m [C₂O₄^2-]ⁿ

you can set up two equations by subsitutes the values in the data provided into the general rate law above, solve for m and n. You have to eliminate one variable first, in order to do so, logically, you would consider data 1&2 or 2&3 values into the rate law.

hope it helps