Consider the following reaction between mercury(II) chloride and oxalate ion.

2 HgCl₂(aq) + C₂O₄^2-(aq) 2 Cl ^-(aq) + 2 CO₂(g) + Hg₂Cl₂(s)

The initial rate of this reaction was determined for several concentrations of HgCl₂ and C₂O₄^2-, and the following rate data were obtained for the rate of disappearance of C₂O₄^2-.

Experiment	[HgCl2] (M)	[C2O42-] (M)	Rate (M/s)
1	0.164	0.15	3.2 10-5
2	0.164	0.45	2.9 10-4
3	0.082	0.45	1.4 10-4
4	0.246	0.15	4.8 10-5

(a) What is the rate law for this reaction?

k[HgCl₂]²[C₂O₄^-2]k[HgCl₂][C₂O₄^-2]² k[HgCl₂]²[C₂O₄^-2]^1/2

(b) What is the value of the rate constant? M^-2s^-1 (c) What is the reaction rate when the concentration of HgCl₂ is 0.16 M and that of C₂O₄^2- is 0.12 M if the temperature is the same as that used to obtain the data shown above? M/s