Question
Phosgene (Cl2CO), a poison gas used in World War I, is formedby the reaction of Cl2 and CO. The proposed mechanism for thereaction is:What rate law is consistent with this mechanism?
Step 1
We can do this by cancelling out the species that appear on both the reactant and product sides of the reaction. The overall reaction is given by: \[2Cl_2 + CO \rightarrow 2Cl_2CO\] Show more…
Show all steps
Your feedback will help us improve your experience
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Recommended Videos
Phosgene $\left(\mathrm{Cl}_{2} \mathrm{CO}\right),$ a poison gas used in World War I, is formed by the reaction of $\mathrm{Cl}_{2}$ and CO. The proposed mechanism for the reaction is: $$\begin{array}{l}{\mathrm{Cl}_{2} \rightleftharpoons 2 \mathrm{Cl}} &{\text { (fast, equilibrium) }} \\ {\mathrm{Cl}+\mathrm{CO} \rightleftharpoons \mathrm{ClCO}} &{\text { (fast, equilibrium) }}\\ {\mathrm{ClCO}+\mathrm{Cl}_{2} \longrightarrow \mathrm{Cl}_{2} \mathrm{CO}+\mathrm{Cl}} &{\text { (slow) }}\end{array}$$ What rate law is consistent with this mechanism?
The formation of phosgene by the reaction $$\mathrm{CO}+\mathrm{Cl}_{2}=\mathrm{COCl}_{2}$$ appears to follow the mechanism $$\begin{array}{c}\mathrm{Cl}_{2} \frac{k_{1}}{\overline{k_{-1}}} 2 \mathrm{Cl} \\ \mathrm{Cl}+\mathrm{CO} \frac{k_{2}}{\overline{k_{-2}}} \mathrm{COCl} \\\mathrm{COCl}+\mathrm{Cl}_{2} \stackrel{k_{3}}{\longrightarrow} \mathrm{COCl}_{2}+\mathrm{Cl}\end{array}$$ Assuming that the intermediates $\mathrm{Cl}$ and $\mathrm{COCl}$ are in a steady state, what is the rate law for this reaction?
The formation of phosgene by the reaction CO + Cl2 = COCl2 appears to follow the mechanism Cl2 ⇌ 2Cl (k1, k-1) Cl + CO ⇌ COCl (k2, k-2) COCl + Cl2 → COCl2 + Cl (k3) Assuming that the intermediates Cl and COCl are in a steady state, what is the rate law for this reaction?
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD