Home
Class 12
CHEMISTRY
Rate law for ozone layer depletion is, ...

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

Text Solution

Verified by Experts

`O_(3)hArrO_(2)+O` (fast reaction)
`" " ` (equilibirum constant `K_(c))`
`O_(3)+Orarr2O_(2)` (slow reaction, rate constan k)
Rate `=k[O_(3)][O]" " ....(i)`
`K_(c)([O_(3)][O])/([O_(3)])or[O]=k_(c)([O_(3)])/([O_(2)])`
`" "` putting the value in eq. (i)
From eq. (i).
Rate `=k*[O_(3)]*K_(c)([O_(3)])/([O_(2)])=k*K_(c)([O_(3)]^(2))/([O_(2)])=k*([O_(3)]^(2))/([O_(2)])`
Here, `K=kxxK_(c)`
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL KINETICS

    OP TANDON|Exercise ILLUSTRATIONS|34 Videos

  • CHEMICAL KINETICS

    OP TANDON|Exercise PRACTICE PROBLEMS|70 Videos

  • CARBOXYLIC ACIDS AND THEIR DERIVATIVES

    OP TANDON|Exercise Integer|4 Videos

  • Chemical Thermodynamics and Thermochemistry

    OP TANDON|Exercise Self Assessment (Integer type).|3 Videos

Similar Questions

Explore conceptually related problems

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")

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.

For the reaction KO_(2)+H_(2)O+CO_(2)rarrKHCO_(3)+O_(2) , the mechanism of reaction suggest.

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)

Determining the rate law from a mechanism with an initial slow step: Ozone reacts with nitrogen dioxide to produce oxygen and dinitrogen pentoxide O_(3)(g)+2NO_(2)(g)rarrO_(2)(g)+N_(2)O_(5)(g) The proposed mechanism is O_(3)(g)+NO_(2)(g)overset(slow)rarr NO_(3)(g)+O_(2)(g) NO_(3)(g)+NO_(2)(g)overset("fast")rarrN_(2)O_(5)(g) What is the rate law predicted by this mechanism ? Strategy : The designations "slow" and "fast" indicate the relative rates of the steps. The rate is determined completely by the slow step, or rate-determining sterp.