The reaction of chloroform and chlorine forms carbon...

The reaction of chloroform and chlorine forms carbon tetrachloride and hydrogen chloride in the following proposed mechanism: $\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{Cl}(g)$ $\mathrm{Cl}(g)+\mathrm{CHCl}_{3}(g) \longrightarrow \mathrm{HCl}(g)+\mathrm{CCl}_{3}(g) \quad$ (slow) $\mathrm{CCl}_{3}(g)+\mathrm{Cl}(g) \longrightarrow \mathrm{CCl}_{4}(g)$ (fast) What are the intermediates in the proposed mechanism? What is the balanced equation for the overall reaction? What is the rate law for the reaction?

The reaction of chloroform and chlorine forms carbon tetrachloride and hydrogen chloride in the following proposed mechanism:
$\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{Cl}(g)$
$\mathrm{Cl}(g)+\mathrm{CHCl}_{3}(g) \longrightarrow \mathrm{HCl}(g)+\mathrm{CCl}_{3}(g) \quad$ (slow)
$\mathrm{CCl}_{3}(g)+\mathrm{Cl}(g) \longrightarrow \mathrm{CCl}_{4}(g)$
(fast)
What are the intermediates in the proposed mechanism? What is the balanced equation for the overall reaction? What is the rate law for the reaction?

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Key Concepts

Rate Law Derivation

The rate law expresses how the reaction rate depends on the concentrations of reactants. It is typically determined by the slow, or rate-determining, step. When a fast pre-equilibrium precedes this step, concentrations of reactive intermediates are expressed in terms of the reactants, leading to a rate law that may involve a fractional order with respect to some reactants.

Overall Reaction Equation

The overall reaction is obtained by summing the elementary steps of the mechanism and canceling out intermediates. The resulting balanced equation shows only the initial reactants and the final products, reflecting the net change in the reaction.

Reaction Intermediates

In a reaction mechanism, intermediates are species that are produced in one step and consumed in a later step, so they do not appear in the overall balanced equation. They are transient and often highly reactive. In a free-radical mechanism, such as this one, intermediates include radicals that propagate the reaction chain but vanish when the overall reaction is summed.

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