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