Nitric oxide reacts with oxygen to produce nitrogen dioxide.
` 2NO (g) +O_(2) (g) to 2NO_(2) (g)`
What is the predicted rate law and order if the mechanism is:
`(i) NO +O_(2) overset(K) hArr NO_(3) ` ( fast)
` (ii ) NO_(3) +NO overset(K_1) hArr NO_(2) +NO_2` ( slow)

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)

Nitric oxide NO reacts with oxygen to produce nitrogen dioxide: 2NO(g) +O_2 (g) to 2NO _2(g) The rate law for this reaction is rate =k [NO]^2 [O_2] Propose a mechanism for the above reaction.

Nitric oxide (NO) reacts with oxygen to produce nitrogen dioxide 2NO_((g))+O_2(g)rarr2N_(2(g)) If the mechanism of reaction is NO+O_2overset(K)hArrNO_3 (fast) NO_3+NOoverset(K_1)rarrNO_2+NO_2 (slow) then rate law is

N_(2)O_(3) overset(R.T.) to NO+NO_(2)

N_(2)O_(3) overset(R.T.) to NO+NO_(2)

NO+NO_(2) overset(-11^(@)C) to N_(2)O_(3)

NO+NO_(2) overset(-11^(@)C) to N_(2)O_(3)

The forward reaction rate for the nitric oxide-oxygen reaction 2NO+O_(2) rarr 2NO_(2) has the rate law as: Rate = k[NO]^(2)[O_(2)] . If the mechanism is assumed to be: 2NO+O overset(k_(eq))hArr , (rapid equilibration) N_(2)O_(2) + O_(2) overset(k_(2))rarr 2NO_(2) (slow step), then which of the following is (are) correct? (I) Rate constant = k_(eq)k_(2) , (II) [N_(2)O_(2)] = k_(eq)[NO]^(2) (III) [N_(2)O_(2)] = k_(eq)[NO] , (IV) Rate constant = k_(2) The correct option is

Pb(NO_(3))_(2) overset(Delta)to PbO+NO_(2)+O_(2)

Pb(NO_(3))_(2) overset(Delta)to PbO+NO_(2)+O_(2)