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The possible mechanism for the reaction 2NO(g)+O_(2)(g) to 2NO_(2)(g) is (i) NO+O_(2) overset(k)to NO_(3) (fast) (ii) NO_(3)+NO overset(k_(2))to NO_(2)+NO_(2)(g) (slow) Write the rate law and order for the reaction. |
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Answer» SOLUTION :RATE LAW is derived from slow step `(DX)/(dt) =k_(2)[NO_(3)][NO]` From (i) `k=([NO_(3)])/([NO][O_(2)]) or [NO_(3)]=k[NO][O_(2)]` Substituting value of `[NO_(3)]` in the above rate law, we get `(dx)/(dt)= k_(2) xx k[NO]^(2)[O_(2)]^(1)` It is rate law. The order of reaction is `2+1=3`. |
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