# Problem: What is the rate law for the overall reaction 2HgCl2 + C2O42- =&gt; 2Cl-- + 2CO2 + Hg2Cl2 given the following mechanism?1. HgCl2 + C2O42- &lt;=&gt; HgCl2C2O42- (fast, equilibrium)2. HgCl2C2O42- + C2O42- =&gt; Hg + 2Cl-- + CO2 + C2O4CO22- (slow)3. Hg + HgCl2 =&gt; Hg2Cl2 (fast)4. C2O4CO22- =&gt; C2O42- + CO2 (fast)a.rate = k [C2O4CO22-]b. rate = k [HgCl2][C2O42- ]c. rate = k [HgCl2][Hg]d. rate = k [HgCl2][C2O42- ]e. rate = k [HgCl2C2O42-][C2O42-]

###### FREE Expert Solution

Determine the overall order of the reaction by analyzing the provided elementary reactions:

1. HgCl2 + C2O42-  HgCl2C2O42- (fast, equilibrium)

2. HgCl2C2O42- + C2O42- Hg + 2Cl-- + CO2 + C2O4CO22- (slow)

3. Hg + HgCl2 Hg2Cl2 (fast)

4. C2O4CO22- → C2O42- + CO2 (fast)

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###### Problem Details

What is the rate law for the overall reaction 2HgCl2 + C2O42- => 2Cl-- + 2CO2 + Hg2Cl2 given the following mechanism?

1. HgCl2 + C2O42- <=> HgCl2C2O42- (fast, equilibrium)

2. HgCl2C2O42- + C2O42- => Hg + 2Cl-- + CO2 + C2O4CO22- (slow)

3. Hg + HgCl2 => Hg2Cl2 (fast)

4. C2O4CO22- => C2O42- + CO2 (fast)

a.rate = k [C2O4CO22-]

b. rate = k [HgCl2][C2O42- ]

c. rate = k [HgCl2][Hg]

d. rate = k [HgCl2][C2O42- ]

e. rate = k [HgCl2C2O42-][C2O42-]