ABC26PH0679 · Chemical Kinetics

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

The following initial rate data were obtained for the reaction
\[ 2\mathrm{NO(g)} + \mathrm{O_2(g)} \rightarrow 2\mathrm{NO_2(g)} \]
Partial pressure of NOPartial pressure of O$_2$Initial rate
Run 1$p_{\mathrm{NO}}$$p_{\mathrm{O_2}}$v
Run 2$2p_{\mathrm{NO}}$$p_{\mathrm{O_2}}$4v
Run 3$p_{\mathrm{NO}}$$2p_{\mathrm{O_2}}$2v
(i) What is the rate law for this reaction? (ii) One of the mechanism proposed for this reaction is
\[ \begin{array}{l} \mathrm{NO(g) + O_2(g)} \underset{\mathrm{k_{-1}}}{\overset{\mathrm{k_1}}{\rightleftharpoons}} \mathrm{NO_3(g)} \\ \mathrm{NO_3(g) + NO(g) \xrightarrow{k_2} 2NO_2(g)} \end{array} \]
Obtain the rate law predicted for this mechanism, assuming a steady state concentration of $\mathrm{NO_3}$. (iii) Predict the rate law for this mechanism, if the first equilibrium step is established quickly and the second step is slow.
Answer
SELF-PRACTICE — the source book printed no answer.

Nothing is invented here, so this question has no answer on record.

Explanation
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