For the reaction; 2 NO + Br 2 leftharpoons 2 NOBr the mechanism is given in two steps a: NO + Br 2 stackrel text Fast leftharpoons NOBr 2 b. NOBr 2+ NO stackrel text Slow longrightarrow 2 NOBr The rate expression for the reaction is

Question

For the reaction; 2 NO + Br 2 leftharpoons 2 NOBr the mechanism is given in two steps a: NO + Br 2 stackrel text Fast leftharpoons NOBr 2 b. NOBr 2+ NO stackrel text Slow longrightarrow 2 NOBr The rate expression for the reaction is (A) r=K[N O]2[B r2] (B) r=K[ NO ][ Br 2] (C) r=K[NO ][B r2]2 (D) r=K[N O B r2]

Tardigrade Admin · Accepted Answer

rate = k [ NOBr 2][ NO ] Also kc=([N O B r2]/[N O][B r2]) [ NOBr 2]= k c[ NO ][ Br 2] =k' kc[N O][B r2][N O] = k [ NO ]2[ Br 2]

Q. For the reaction; $2 NO + B r_{2} ⇌ 2 NOB r$
the mechanism is given in two steps
a: $NO + B r_{2} ⇌ Fast NOB r_{2}$
b. $NOB r_{2} + NO ⟶ Slow 2 NOB r$
The rate expression for the reaction is

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

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

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

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

rate $= k [NOB r_{2}] [NO]$

Also $k_{c} = \frac{[ NOB r _{2} ]}{[ NO ] [ B r _{2} ]}$

$[NOB r_{2}] = k_{c} [NO] [B r_{2}]$

$= k^{'} k_{c} [NO] [B r_{2}] [NO]$

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

Q. For the reaction; 2NO+Br2​⇌2NOBr the mechanism is given in two steps a: NO+Br2​⇌ Fast​NOBr2​ b. NOBr2​+NO⟶ Slow ​2NOBr The rate expression for the reaction is

r=K[NO]2[Br2​]

r=K[NO][Br2​]

r=K[NO][Br2​]2

r=K[NOBr2​]