1.

What is the rate law for the reaction, NO_(2(g)) + CO_((g)) to NO_((g)) + CO_(2(g)) The reaction occurs in the following steps :(i) NO_(2) + NO_(2) to NO_(3) + NO (Slow) (ii) NO_(3) + CO to NO_(2) + O_(2) (fast) What is the role of NO_(3) ?

Answer»

Solution : Overall reaction: `NO_(2(G)) +CO_(2(g)) to NO_((g)) + CO_(2(g))`
Step - I : `NO_(2) +NO_(2) to NO_(3) + NO` (slow)
Step -II : `NO_(3) + CO to NO_(2) +CO_(2)` (FAST)
(A) From first rate determining slow step, rate law is, Rate `= K [NO_(2)]^(2)`
(B)Role of `NO_(3)` : In the reaction, `NO_(3)`is the reaction INTERMEDIATE which is formed in first step and removed in the second step.


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