the reaction 2NO + Br2 -> 2NOBr obeys the following mechanism
No + Br -> NOBr 2 (fast)
NOBr2 + NO -> 2NOBr
suggest the rate expression
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Rate law is determined by the slowest step in the reaction mechanism. Here, the slowest step is the 2nd step. For a slowest step, the rate law is :
rate = k [NOBr2] [NO] (i)
The concentration of NOBr2 is an intermediate , it should not appear in the rate law equation:
From step 1
Keq =[NOBr2][NO][Br2][NOBr2]= Keq[NO][Br2]Substituting in (i)Rate =k.Keq[NO][Br2][NO]Rate =k.Keq[NO]2[Br2]Rate =k[NO]2[Br2]
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rate = k [NOBr2] [NO] (i)
The concentration of NOBr2 is an intermediate , it should not appear in the rate law equation:
From step 1
Keq =[NOBr2][NO][Br2][NOBr2]= Keq[NO][Br2]Substituting in (i)Rate =k.Keq[NO][Br2][NO]Rate =k.Keq[NO]2[Br2]Rate =k[NO]2[Br2]
Hope this information will clear your doubts regarding the topic. If you have any other doubts please ask here on the forum and our experts will try to solve them as soon as possible.
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