3) Given the following proposed mechanism, predict the rate law for the overall reaction. A2 + 2 B ? 2 AB (overall reaction) Mechanism A2 ? 2 A fast A + B ? AB slow A) Rate = k[A2][B] B) Rate = k[A]2[B]2 C) Rate = k[A2]1/2[B]1/2 D) Rate = k[A2]1/2[B] E) Rate = k[A2]2
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The rate law for this step is Rate = k[A][B]. However, A is not a reactant in the overall reaction. It is an intermediate, produced in the fast step and consumed in the slow step. We can express the concentration of A in terms of the reactants in the overall Show more…
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A possible mechanism for the reaction 2A + B → C + D is: step 1: A + A ⇌ A2 (fast) step 2: A2 + A → A3 (slow) step 3: A3 + B → A + C + D (fast) According to this mechanism, the rate law will be: rate = k[A]^2[B] rate = k[A]^2 rate = k[A][B] rate = k[A3][B] rate = k[A] rate = k[A]^3
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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. $$ \begin{array}{c} 2 \mathrm{B} \frac{k_{1}}{k_{-1}} \mathrm{B}_{2} \text { (fast) } \\ \mathrm{A}+\mathrm{B}_{2} \stackrel{k_{2}}{\longrightarrow} \mathrm{C}+\mathrm{D} \text { (slow) } \end{array} $$
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. $$\begin{array}{c} 2 \mathrm{B} \stackrel{k_{1}}{\mathrm{k}_{1}} \mathrm{B}_{2} \text { (fast) } \\ \mathrm{A}+\mathrm{B}_{2} \stackrel{k_{2}}{\longrightarrow} \mathrm{C}+\mathrm{D} \text { (slow) } \end{array}$$
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