For the reaction, 2 NO + Cl 2 longrightarrow 2 NOCl The following mechanism has been proposed NO +leftharpoons NOCl 2 text (fast) NOCl 2+ NO longrightarrow 2 NOCl text (slow)

Question

For the reaction, 2 NO + Cl 2 longrightarrow 2 NOCl The following mechanism has been proposed NO +leftharpoons NOCl 2 text (fast) NOCl 2+ NO longrightarrow 2 NOCl text (slow)  (A) Rate = k [ NO ][ Cl 2]2 (B) Rate = k [ NO ]2[ Cl 2] (C) Rate = k [ NOCl ]2 (D) Rate = k [ NOCl 2][ NO ]

Tardigrade Admin · Accepted Answer

From slow step, Rate = k [ NOCl 2][ NO ] (i) From fast step Equation constant K =([ NOCl 2]/[ NO ][ CL 2]) Putting the value of [ NOCl 2] in (i) Rate = Kk'[ NO ]2[ Cl 2] Rate = k [ NO ]2[ Cl ]

Q. For the reaction, $2 NO + C l_{2} ⟶ 2 NOCl$ The following mechanism has been proposed
$NO + ⇌ NOC l_{2} (fast)$
$NOC l_{2} + NO ⟶ 2 NOCl (slow)$

Rate $= k [NO] [C l_{2}]^{2}$

Rate $= k [NO]^{2} [C l_{2}]$

Rate $= k [NOCl]^{2}$

Rate $= k [NOC l_{2}] [NO]$

From slow step,
Rate $= k [NOC l_{2}] [NO]$
From fast step
Equation constant $K = \frac{[ NOC l _{2} ]}{[ NO ] [ C L _{2} ]}$
Putting the value of $[NOC l_{2}]$ in (i)
Rate $= K k^{'} [NO]^{2} [C l_{2}]$
Rate $= k [NO]^{2} [Cl]$

Q. For the reaction, 2NO+Cl2​⟶2NOCl The following mechanism has been proposed NO+⇌NOCl2​ (fast) NOCl2​+NO⟶2NOCl (slow)

Rate =k[NO][Cl2​]2

Rate =k[NO]2[Cl2​]

Rate =k[NOCl]2

Rate =k[NOCl2​][NO]