Solved: Consider the following reaction between
Chapter 6, Problem 100AE(choose chapter or problem)
Consider the following reaction between mercury(II) chloride and oxalate ion:
\(2 \mathrm{HgCl}_2(a q)+\mathrm{C}_2 \mathrm{O}_4{ }^{2-}(a q) \longrightarrow\) \(2 \mathrm{Cl}^{-}(a q)+2 \mathrm{CO}_2(g)+\mathrm{Hg}_2 \mathrm{Cl}_2(s)\)
The initial rate of this reaction was determined for several concentrations of \(\mathrm{HgCl}_2\) and \(\mathrm{C}_2 \mathrm{O}_4{ }^{2-}\), and the following rate data were obtained for the rate of disappearance of \(\mathrm{C}_2 \mathrm{O}_4{ }^{2-}\):
(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 \(\mathrm{Hg}_2 \mathrm{Cl}_2\) is 0.100 M and that of \((\mathrm{C}_2 \mathrm{O}_4{ }^{2-})\) is 0.25 M. if the temperature is the same as that used to obtain the data shown?
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