A reaction `ArarrB` , involes following mechanism :
Step1 : `Aoverset(k_(1))rarrB" "("fast")`
Step2 : `Boverset(k_(2))rarrC " "("slow")`
Step3: `Coverset(k_(3))rarrD " "("fast")`
The rate law of the reaction may be given as :

For hypothetical reaction ArarrB takes placed according to Aoverset(k_(1))hArrC("fast"),A+Coverset(k_(2))rarrD("slow") Rate law will be :

Mechanism of the reaction is: A overset(k_(1))rarrB, 2Aoverset(k_(2))rarr C + D What is (-d[A])/(dt) ?

Mechanism of the reaction is: A overset(k_(1))rarrB, 2Aoverset(k_(2))rarr C + D What is (-d[A])/(dt) ?

A reaction A_(2)+B rarr products, involves the following mechanism : A_(2) hArr 2A ("Fast")" " ( A being the intermediate ) A+B underset(k_(2))rarr products (slow). The rate law consistant to this mechanism is :

For the reaction 2H_(2) + 2NO rarr N_(2) + 2H_(2)O , the following mechanism has been suggested : 2NO ? N_(2)O_(2) equilibrium constant K_(1) (fast) N_(2)O_(2) +H_(2) overset(k_(2)) rarr N_(2)O +H_(2)O (slow) N_(2) O +H_(2) overset(k_(3)) rarr N_(2)+H_(2)O (fast) Establish the rate law for given reaction.

The mechanism of the reaction 2NO + O_(2) rarr 2NO_(2) is NO + NO underset(k_(-1))overset(k_(1))hArr N_(2)O_(2) ("fast") N_(2)O_(2) + O_(2) overset(k_(2))rarr 2NO_(2) (slow) The rate constant of the reaction is

The mechanism of the reaction 2NO + O_(2) rarr 2NO_(2) is NO + NO underset(k_(-1))overset(k_(1))hArr N_(2)O_(2) ("fast") N_(2)O_(2) + O_(2) overset(k_(2))rarr 2NO_(2) (slow) The rate constant of the reaction is