1. What is the overall reaction? (b) What are the
Chapter , Problem 110AE(choose chapter or problem)
The following mechanism has been proposed for the gas-phase reaction of chloroform \(\left(\mathrm{CHCl}_{3}\right)\) and chlorine:
\(step 1: \quad C l_{2}(g) \underset{k-1}{\stackrel{k}{\rightleftarrows}} 2 C l(g) (fast)\)
\(step 2: \quad \mathrm{Cl}(g)+\mathrm{CHCl}_{3}(g)_{\rightarrow}^{k_{2}} \mathrm{HCl}(g)+\mathrm{CCl}_{3}(g)( slow )\)
\(step 3: $\quad \mathrm{Cl}(\mathrm{g})+\mathrm{CCl}_{3}(\mathrm{~g}) \stackrel{k_{3}}{\rightarrow} \mathrm{CCl}_{4} \quad (fast)\)
(a) What is the overall reaction?
(b) What are the intermediates in the mechanism?
(c) What is the molecularity of each of the elementary reactions?
(d) What is the rate-determining step?
(e) What is the rate law predicted by this mechanism? (Hint: The overall reaction order is not an integer.)
Equation Transcription:
Text Transcription:
(CHCl3)
step 1: \quad C l_2(g) \underset k-1\stackrelk \rightleftarrows 2 C l(g) (fast)
step 2: \quad Cl(g)+CHCl_3(g)_\rightarrow^k_2 HCl(g)+CCl_3(g)( slow )
step 3: \quad Cl(g)+CCl_3(g) \stackrel{k_3 \rightarrow CCl_4 \quad (fast)
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