IF anyone can help me with this involved question it would be greatly appreaciat
ID: 810297 • Letter: I
Question
IF anyone can help me with this involved question it would be greatly appreaciated.
the following data were collected from two separate experiments for the following reaction in aqueous, by measuring the number of moles of Hg2Cl2 that precipated per liter per minute
2HgCl2(aq) + C2O4^2-(aq) ---> 2Cl-(aq) + 2CO2(g) Hg2Cl2 (s)
Experiment 1 Experiment 2
time HgCl2 mol/L excess C2O4^2- C2O4^2- mol/L excess HgCl2
0 0.150 0.300
3.33 0.0843 0.283
5.00 0.0755 0.275
6.67 0.0676 0.268
8.33 0.0606 0.261
10.00 0.0543 0.254
16.67 0.0340 0.229
23.33 ? ?
d.) In a separate experiment when HgCl2 = 0.105 M and C2O4^2- = 0.300 M the initial rate was 7.1 * 10^-5 mol L^-1min-1. Determine the overall rate law constant (K). What would be the initial rate of the reaction if HgCl2 = 0.02 M and C2O4^2- = 0.22 M under this condition?
Explanation / Answer
Assuming the order of reaction with respect to HgCl2 is 2 and that with respect to oxalate is 1,
the rate = K[HgCl2]^2[oxalate]
K = 7.1x10^-5/(0.105)^2(0.3) = 0.0215
initial rate = 0.0215*(0.02)^2*(0.22) = 1.889x10^-6 M/min