Consider the following reaction:

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

(a) The rate law for this reaction is first order in HgCl₂(aq) and second order in C₂O₄^2-(aq). What is the rate law for this reaction?

Rate = k [HgCl₂(aq)] [C₂O₄^2-(aq)]

Rate = k [HgCl₂(aq)]² [C₂O₄^2-(aq)]

Rate = k [HgCl₂(aq)] [C₂O₄^2-(aq)]²

Rate = k [HgCl₂(aq)]² [C₂O₄^2-(aq)]²

Rate = k [HgCl₂(aq)] [C₂O₄^2-(aq)]³

Rate = k [HgCl₂(aq)]⁴ [C₂O₄^2-(aq)]

(b) If the rate constant for this reaction at a certain temperature is 0.0133, what is the reaction rate when [HgCl₂(aq)] = 0.157 M and [C₂O₄^2-(aq)] = 0.238 M? Rate = ____ M/s. (c) What is the reaction rate when the concentration of HgCl₂(aq) is doubled, to 0.314 M while the concentration of C₂O₄^2-(aq) is 0.238 M? Rate = ____ M/s