The reaction 2 NO+Br2 arrow 2NOBr, obeys the following mechanism: NO+Br2 [Fast] NOBr2 ;+NO -[Slow] 2NOBr The rate expression of the above reaction can be written as

Question

The reaction 2 NO+Br2 arrow 2NOBr, obeys the following mechanism: NO+Br2 <=>[Fast] NOBr2 ;+NO ->[Slow] 2NOBr The rate expression of the above reaction can be written as (A) r=k[NO]2 [Br2] (B) r=k[NO] [Br2] (C) r=k NO2Br2 (D) r=k[NOBr2]

Tardigrade Admin · Accepted Answer

For slowest step: rate =k[NOBr2][NO] ldots(i) For equilibrium also Kc=([NOBr2]/[NO][Br2]) ldots(ii) By eqs. (i) and (ii), r=k⋅ kc[NO]2[Br2] Rate=k[NO]2 [Br2]

Q. The reaction $2 NO + B r_{2}$ $\to$ $2 NOB r$ , obeys the following mechanism :
$NO + B r_{2}$ $Fast$ $NOB r_{2}; + NO$ $Slow$ $2 NOB r$ The rate expression of the above reaction can be written as

$r = k [NO]^{2}$ $[B r_{2}]$

$r = k [NO]$ $[B r_{2}]$

$r = k N O^{2} B r_{2}$

$r = k [NOB r_{2}]$

For slowest step : rate $= k [NOB r_{2}] [NO]$ $\dots (i)$
For equilibrium also $K_{c} = \frac{[ NOB r _{2} ]}{[ NO ] [ B r _{2} ]}$ $\dots (ii)$
By eqs. $(i) an d (ii)$ , $r = k \cdot$ $k_{c} [NO]^{2} [B r_{2}]$
Rate $= k [NO]^{2}$ $[B r_{2}]$

Q. The reaction 2NO+Br2​ → 2NOBr, obeys the following mechanism : NO+Br2​ Fast​ NOBr2​;+NO Slow​ 2NOBr The rate expression of the above reaction can be written as

r=k[NO]2 [Br2​]

r=k[NO] [Br2​]

r=kNO2Br2​

r=k[NOBr2​]