A chemical reaction occurs in two steps :(i) NO2Cl(g) —(slow)→ NO2(g) + Cl(g)(ii) NO2Cl(g) + Cl(g) —(fast)→ NO2(g) + Cl2(g)(a) Write down the rate law.(b) Identify the reaction intermediate.

Question

Q.13 A chemical reaction occurs in two steps : (i) NO₂Cl_((g)) —(slow)→ NO_(2(g)) + Cl_((g)) (ii) NO₂Cl_((g)) + Cl_((g)) —(fast)→ NO_(2(g)) + Cl_(2(g)) (a) Write down the rate law. (b) Identify the reaction intermediate.

Doubtly AI · Accepted Answer

Answer: (a) Rate = k[NO₂Cl] (b) Cl (atomic chlorine) Overall reaction (adding the steps): 2NO₂Cl_((g)) → 2NO_(2(g)) + Cl_(2(g)). (a) The rate of the overall reaction is decided by the slowest (rate-determining) step, step (i), which is unimolecular in NO₂Cl. Hence rate = k[NO₂Cl]; the reaction is first order. (b) Cl is formed in step (i) and consumed in step (ii); it does not appear in the overall equation, so Cl is the reaction intermediate.

A chemical reaction occurs in two steps :(i) NO2Cl(g) —(slow)→ NO2(g) + Cl(g)(ii) NO2Cl(g) + Cl(g) —(fast)→ NO2(g) + Cl2(g)(a) Write down the rate law.(b) Identify the reaction intermediate.

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