Rate law for ozone layer depletion is,
`(d[O_(3)])/(dt)=(K[O_(3)]^(2))/([O_(2)])`
Give the proboble mechanism of reaction ?

Ozone (O_(3)) depletion is due to

The gaseous decomposition of ozome 2O_(3)rarr3O_(2) obeys the rate law r=-(d[O_(3)])/(dt)=(k[O_(3)]^(2))/([O_(2)]) Show that the following mechanims is consistent with the above rate law : O_(3)overset(K_(eq))hArrO_(2)+O" " ("fast") O+O_(3)overset(k_(1))rarr2O_(2)" " ("slow")

For the reaction 2O_(3)(g)rarr3O_(2)(g) , the experimentally obtained rate equation , rate =k=([O_(3)]^(2))/([O_(2)]) . What is the overall order of this reaction? What is the order of the reaction with respect to O_(3) and O_(2) ?

In the decompoistion of N_(2)O_(5)(g) , 2N_(2)O_(5)(g)overset(k_(obs))rarr4NO_(2)(g) + O_(2)(g) , the observed rate law is given by (d[O_(2)])/(dt) = k_(obs)[N_(2)O_(5)] . Which of the following proposed mechanics is conisstent with the rate law? a. N_(2)O_(5)(g)overset(k)rarrN_(2)O_(3)(g) + O_(2)(g) b. N_(2)(g) + NO_(3)(g)overset(k_(1))rarrNO(g) + NO_(2)(g)+O_(2)(g)

In the decompoistion of N_(2)O_(5)(g) , 2N_(2)O_(5)(g)overset(k_(obs))rarr4NO_(2)(g) + O_(2)(g) , the observed rate law is given by (d[O_(2)])/(dt) = k_(obs)[N_(2)O_(5)] . Which of the following proposed mechanics is conisstent with the rate law?

Nitric oxide, NO, reacts with oxygen to produce nitrogen dioxide : 2NO(g)+O_(2)(g)to2NO_(2)(g) The rate law for this reaction is : Rate =k[NO]^(2)[O_(2)]. Propose a mechanism for the above reaction.

The rate law expression for the reaction, 2NO+O_(2) rarr 2NO_(2) is: rate =K[NO][O_(2)] Suggest the possible mechanism.

Nitric oxide (NO) reacts with oxygen to produce nitrogen dioxide (NO_(2)) : 2NO(g) + O_(2) to 2NO_(2) (g) The rate law for the reaction is: rate = k[NO]^2[O_(2)] Propose a mechanism for the above reaction.

The rate law for the reaction O_(3) + O rarr 2O_(2) is rate = k[O_(3)][NO] . Then which is/are correct? (more than one correct)