Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: slu1986 on September 25, 2008, 01:13:00 PM
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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
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hey,
check this out: http://www.chemicalforums.com/index.php?topic=25958.msg98386#msg98386 (oberservation method)
alternatively,
r = k[HgCl2]m [C2O42-]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