The hypothetical reaction, A 2 + B 2 → 2 A B follows the following mechanism: A₂ ⇌ A + A (fast) A + B₂ → AB + B (slow) A + B → AB (fast) The order of the overall reaction is:

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The hypothetical reaction, $A_{2} + B_{2} \to 2 A B$ follows the following mechanism:

A₂ $⇌$ A + A (fast)

A + B₂ $\to$ AB + B (slow)

A + B $\to$ AB (fast)

The order of the overall reaction is:

Answer:

Solution:

The rate-determining step is A + B₂ $\to$ AB + B (slow).

From the fast equilibrium, $[A] = k_{e q} [A_{2}]^{1/2}$ .

Rate = $k [A] [B_{2}] = k k_{e q} [A_{2}]^{1/2} [B_{2}]$ .

Overall order = $1/2 + 1 = 3/2$ .

Stream:JEESubject:ChemistryTopic:Chemical KineticsSubtopic:Rate of Reactions/Rate Law

⏱ 2mℹ️ Source: QB

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