ABC26PH0676 · Chemical Kinetics

Subject: Physical Chemistry · Chapter: Chemical Kinetics · Topic: Steady State Approximation · Exam: JAM 2001-2022 · Marks: 2 · Difficulty: Hard

For the reaction, $\mathrm{H_2(g) + Br_2(g) \longrightarrow 2HBr(g)}$ the following mechanism has been proposed.
\[ \begin{array}{l} \text{Initiation: } \mathrm{Br_2 + M \xrightarrow{k_i} Br^{\bullet} + Br^{\bullet} + M} \\ \text{Propagation: } \mathrm{Br^{\bullet} + H_2 \xrightarrow{k_p} HBr + H^{\bullet}}\text{;}\;\; \mathrm{H^{\bullet} + Br_2 \xrightarrow{k_{p'}} HBr + Br^{\bullet}} \\ \text{Retardation: } \mathrm{H^{\bullet} + HBr \xrightarrow{k_r} H_2 + Br^{\bullet}} \\ \text{Termination: } \mathrm{Br^{\bullet} + Br^{\bullet} + M \xrightarrow{k_t} Br_2 + M + energy} \end{array} \]
where M is the initiator/terminator.
(a)Write the differential rate equations for the formation of the two intermediates $\mathrm{H}^{\bullet}$ and $\mathrm{Br}^{\bullet}$.
(b)Using the steady-state approximate calculate the concentration of the intermediate $\mathrm{H}^{\bullet}$ and $\mathrm{Br}^{\bullet}$ and obtain the rate law for the formation of HBr.
Answer
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Explanation
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