Consider the mechanism below. Identify the intermediate(s). Cl2 <--> 2 Cl Fast Cl + CHCl3 --> HCl + CCl3 Slow Cl + CCl3 --> CCl4 Fast
Added by Jordan L.
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The mechanism consists of three steps: 1. \( \text{Cl}_2 \rightleftharpoons 2 \text{Cl} \) (Fast equilibrium) 2. \( \text{Cl} + \text{CHCl}_3 \rightarrow \text{HCl} + \text{CCl}_3 \) (Slow) 3. \( \text{Cl} + \text{CCl}_3 \rightarrow \text{CCl}_4 \) (Fast) Show more…
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1. Cl2 (g) ⟶ 2 Cl (g) Fast 2. Cl (g) + CHCl3 (g) ⟶ HCl (g) + CCl3 (g) Slow 3. Cl (g) + CCl3 (g) ⟶ CCl4 (g) Fast Based on the reaction mechanism above, determine the overall reaction. a. Cl2 + 2 Cl + CHCl3 + CCl3 ⟶ 2 Cl + HCl + CCl3 + CCl4 b. CHCl3 + CCl3 ⟶ HCl + CCl4 c. Cl2 + CHCl3 ⟶ HCl + CCl4 d. 2 CHCl3 ⟶ 2 HCl + CCl4
Pahal S.
Consider this three-step mechanism for a reaction: $\mathrm{Cl}_{2}(g) \underset{k_{2}}{\stackrel{k_{1}}{\rightleftharpoons}} 2 \mathrm{Cl}(g)$ Fast $\mathrm{Cl}(g)+\mathrm{CHCl}_{3}(g) \underset{k_{3}}{\longrightarrow} \mathrm{HCl}(g)+\mathrm{CCl}_{3}(g)$ Slo $\mathrm{Cl}(g)+\mathrm{CCl}_{3}(g) \underset{k_{4}}{\longrightarrow} \mathrm{CCl}_{4}(g)$ Fast a. What is the overall reaction? b. Identify the intermediates in the mechanism. c. What is the predicted rate law?
Consider this three-step mechanism for a reaction: $\mathrm{Cl}_{2}(g) \underset{k_{2}}{\stackrel{k_{1}}{\rightleftarrows}} 2 \mathrm{Cl}(g)$ Fast $\mathrm{Cl}(g)+\mathrm{CHCl}_{3}(g) \longrightarrow \mathrm{HCl}(g)+\mathrm{CCl}_{3}(g) \quad$ Slow $\mathrm{Cl}(g)+\mathrm{CCl}_{3}(g) \longrightarrow \mathrm{CCl}_{4}(g)$ Fast a. What is the overall reaction? b. Identify the intermediates in the mechanism. c. What is the predicted rate law?
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