अभिक्रिया दो पदों में होती है(i) NO_(2)Cl_((g))overset(K_(q))rarr NO_(2(g))+Cl_((g)) (ii) NO_(2)...

The reaction takes place in two steps as (i) NO_(2) Cl _((g)) overset(K_(1)) to NO_(2(g)) +Cl_((g)) (ii ) NO_(2) Cl_((g)) +Cl_((g)) overset(K_(2)) to NO_(2(g)) +Cl_(2(g)) Identify the reaction intermediate .

The rate law for the decompoistion of gaseous N_(2)O_(5) , N_(2)O_(5)(g) rarr 2NO_(2)(g) + (1)/(2)O_(2)(g) is observed to be: r = (-d[N_(2)O_(5)])/(dt) = k[N_(2)O_(5)] A reaction machanism which has been suggested to be conisstent with this rate law is N_(2)O_(5)(g) overset(k_(eq))hArr NO_(2)(g)+NO_(3)(g) ("fast equilibrium") NO_(2) (g) + NO_(3)(g) overset(k_(1))rarr NO_(2)(g) + NO(g) + O_(2)(g) (slow) NO(g) + NO_(3)(g) overset(k_(2))rarr 2NO_(2)(g) (fast)

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.

Equilibrium constants K_(1) and K_(2) for the following equilibria NO(g) +1//2O_(2)(g) overset(K_(1))(hArr) NO_(2)(g) and 2NO_(2)(g) overset(K_(2))(hArr)2NO(g)+O_(2)(g) are related as

In the following reaction: 2NO(g)+O_(2)(g) overset(k')rarr2NO_(2)(g) What is the predicted rate law, if the mechanism is NO+O_(2)(g) overset(k_(eq))hArr NO_(3) ("fast") (fast) NO_(3) + NO overset(k_(1))rarr NO_(2) + NO_(2) (slow)