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 ? ?

a.) Determine the order of the reaction with respect to HgCl2, with respect to C2O4^2- and the overall rate. Write the rate law.

b.) Write the integrated rate law and the rate constant (K') with respect to HgCl2 and the integrated rate law and rate constant (K'') with respect to C2O4^2-

c.) What would be the concentration of both HgCl2 and C2O4^2- ion at 23.33 minutes

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?

e.) Compare the values of K', K'', and K

f.) What is the first half life of both HgCl2 and C2O4^2- from the concentration at t=0 minutes?

Thanks, I know this is a long question.