Consider the following reaction between mercury (II) chloride and oxalate ion:
2 HgCI2(aq) + C2O42- (aq) †’
2 CIˉ (aq) + 2 CO2(g) + Hg2CI2(s)
The initial rate of this reaction was determined for several concentration of HgCI2 and C2O42-, and the following rate data were obtained for the rate of disappearance of C2O42-:

(a) What is the rate law for this reaction?
(b) What is the value of the rate constant with proper units?
(c) What is the reaction rate when the initial concentration of HgCl2 is 0.100 M and that of (C2O42-) is 0.25 M if the temperature is the same as that used to obtain the data shown?

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Experiment [HgCl2l (M) C2041 (M) Rate (M/s) 3.2 X 10-5 2.9 × 10-4 1.4 × 10-4 4.8 × 10-5 0.164 0.164 0.082 0.246 0.15 0.45 0.45 0.15 4