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: $\begin{array}{rlr}\mathrm{Cl}_{2}(g) & \rightleftharpoons 2 \mathrm{Cl}(g) & & \text { (fast) } \\ \mathrm{Cl}(g)+\mathrm{CHCl}_{3}(g) & \longrightarrow \mathrm{HCl}(g)+\mathrm{CCl}_{3}(g) & & \text { (slow) } \\ \mathrm{CCl}_{3}(g)+\mathrm{Cl}(g) & \longrightarrow \mathrm{CCl}_{4}(g) & & \text { (fast) }\end{array}$ 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? Make a graph of concentration versus time for the formation of $\mathrm{C}_{2} \mathrm{H}_{4}$ and the decomposition of $\mathrm{C}_{4} \mathrm{H}_{8}$ on the same graph. What are the rates of formation of $\mathrm{C}_{2} \mathrm{H}_{4}$ at $t=1.00 \times 10^{3} \mathrm{~s}$ and $t=9.00 \times 10^{3} \mathrm{~s},$ and the rates of decomposition of $\mathrm{C}_{4} \mathrm{H}_{8}$ at $t=1.00 \times 10^{3} \mathrm{~s}$ and $t=9.00$ $\times 10^{3} \mathrm{~s}$ ? What can be said about the relationship between the values of the rates of formation and decomposition?

The reaction of chloroform and chlorine forms carbon tetrachloride and hydrogen chloride in the following proposed mechanism: $\begin{array}{rlr}\mathrm{Cl}_{2}(g) & \rightleftharpoons 2 \mathrm{Cl}(g) & & \text { (fast) } \\ \mathrm{Cl}(g)+\mathrm{CHCl}_{3}(g) & \longrightarrow \mathrm{HCl}(g)+\mathrm{CCl}_{3}(g) & & \text { (slow) } \\ \mathrm{CCl}_{3}(g)+\mathrm{Cl}(g) & \longrightarrow \mathrm{CCl}_{4}(g) & & \text { (fast) }\end{array}$ 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? Make a graph of concentration versus time for the formation of $\mathrm{C}_{2} \mathrm{H}_{4}$ and the decomposition of $\mathrm{C}_{4} \mathrm{H}_{8}$ on the same graph. What are the rates of formation of $\mathrm{C}_{2} \mathrm{H}_{4}$ at $t=1.00 \times 10^{3} \mathrm{~s}$ and $t=9.00 \times 10^{3} \mathrm{~s},$ and the rates of decomposition of $\mathrm{C}_{4} \mathrm{H}_{8}$ at $t=1.00 \times 10^{3} \mathrm{~s}$ and $t=9.00$
$\times 10^{3} \mathrm{~s}$ ? What can be said about the relationship between the values of the rates of formation and decomposition?

Key Concepts

Reaction Mechanism

A reaction mechanism describes the step?by?step process by which reactants convert into products. It includes a sequence of elementary reactions that can be fast or slow, with at least one step typically being rate-determining. The mechanism provides insight into the roles of individual species and the order in which bonds are broken and formed.

Reaction Intermediate

An intermediate is a chemical species that is formed in one step of a reaction mechanism and consumed in a subsequent step. Intermediates do not appear in the overall balanced reaction because they are produced and used up during the reaction process. Their identification is crucial for understanding the pathway and kinetics of the reaction.

Overall Reaction

The overall reaction is obtained by combining all the elementary steps of the mechanism and canceling out any common species, particularly intermediates. This aggregation results in a balanced equation that represents the net change from reactants to products, accounting for stoichiometry.

Rate Law Derivation

The rate law expresses the reaction rate in terms of the concentrations of reactants, often based on the slow (rate-determining) step of the mechanism. Using concepts such as the steady-state or pre-equilibrium approximations, the derivation of the rate law links the molecular steps of the mechanism to the observed kinetics of the overall reaction.

Graphical Analysis in Kinetics

Graphical analysis involves plotting concentration versus time to visualize the progression of a reaction. These plots allow for the determination of reaction rates by examining the slopes at given time points, and they are especially useful for comparing the formation and consumption rates of different species within a reaction.

Reaction Rates Comparison

Comparing the rates of formation for products and the rates of decomposition for reactants typically involves analyzing the slopes of their concentration versus time graphs at specific time points. This comparison can reveal relationships such as simultaneous or complementary changes during the course of a reaction, often providing evidence for the validity of the proposed mechanism and indicating steady-state behavior.

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