For the reaction A+2 B ⟶C+D, the rate law is rate of reaction =k[A][B] (a) Show that the followi

step 1 This question is in regards to two possible mechanisms for the reaction of A plus 2B goes to C p

For the reaction A+2 B ⟶C+D, the rate law is rate of...

For the reaction $\mathrm{A}+2 \mathrm{B} \longrightarrow \mathrm{C}+\mathrm{D},$ the rate law is rate of reaction $=k[\mathrm{A}][\mathrm{B}]$ (a) Show that the following mechanism is consistent with the stoichiometry of the overall reaction and with the rate law. $$\begin{array}{l} \mathrm{A}+\mathrm{B} \longrightarrow \mathrm{I} \quad(\text { slow }) \\ \mathrm{I}+\mathrm{B} \longrightarrow \mathrm{C}+\mathrm{D} \quad(\text { fast }) \end{array}$$ (b) Show that the following mechanism is consistent with the stoichiometry of the overall reaction, but not with the rate law. $$\begin{array}{c} 2 \mathrm{B} \stackrel{k_{1}}{\mathrm{k}_{1}} \mathrm{B}_{2} \text { (fast) } \\ \mathrm{A}+\mathrm{B}_{2} \stackrel{k_{2}}{\longrightarrow} \mathrm{C}+\mathrm{D} \text { (slow) } \end{array}$$

For the reaction $\mathrm{A}+2 \mathrm{B} \longrightarrow \mathrm{C}+\mathrm{D},$ the rate law is rate of reaction $=k[\mathrm{A}][\mathrm{B}]$
(a) Show that the following mechanism is consistent with the stoichiometry of the overall reaction and with the rate law.
$$\begin{array}{l}
\mathrm{A}+\mathrm{B} \longrightarrow \mathrm{I} \quad(\text { slow }) \\
\mathrm{I}+\mathrm{B} \longrightarrow \mathrm{C}+\mathrm{D} \quad(\text { fast })
\end{array}$$
(b) Show that the following mechanism is consistent with the stoichiometry of the overall reaction, but not with the rate law.
$$\begin{array}{c}
2 \mathrm{B} \stackrel{k_{1}}{\mathrm{k}_{1}} \mathrm{B}_{2} \text { (fast) } \\
\mathrm{A}+\mathrm{B}_{2} \stackrel{k_{2}}{\longrightarrow} \mathrm{C}+\mathrm{D} \text { (slow) }
\end{array}$$

Key Concepts

Reaction Mechanism

A reaction mechanism describes the step-by-step sequence of elementary reactions by which an overall chemical change occurs. It provides details on the order in which bonds are broken and formed, as well as the intermediates involved, helping to understand how the reaction progresses from reactants to products.

Rate Law

The rate law is an equation that links the reaction rate to the concentrations of the reactants, usually with experimentally determined orders. It is crucial in determining how changes in concentration affect the speed of the reaction and in identifying the rate-determining step within the mechanism.

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. It ensures the conservation of atoms and mass in the overall reaction, defining the proportions in which chemicals react and products form.

Rate-Determining Step

The rate-determining step is the slowest step in a reaction mechanism that essentially controls the overall reaction rate. This step's kinetics typically determine the form of the observed rate law and is critical when using mechanisms to explain experimentally observed rate laws.

Reaction Intermediates

Reaction intermediates are species that are formed in one step of the mechanism and consumed in subsequent steps. Their concentrations are typically low and not present in the overall balanced equation, but they play a key role in the detailed step-by-step pathway of the reaction.

Transcript

Please give Ace some feedback