In the reversible reaction, 2 NO 2 undersetk2 stackrelk1leftharpoons N 2 O 4 the rate of disappearance of NO 2 is equal to

Question

In the reversible reaction, 2 NO 2 undersetk2 stackrelk1leftharpoons N 2 O 4 the rate of disappearance of NO 2 is equal to (A) (2 k1/k2)[ NO 2]2 (B) 2 k1[ NO 2]2-2 k2[ N 2 O 4] (C) 2 k1[ NO 2]2-k2[ N 2 O 4] (D) (2 k1-k2)[ NO 2]

Tardigrade Admin · Accepted Answer

2 NO 2 underset k 2 stackrelk1leftharpoons N 2 O 4 Rate =-(1/2) (d[ NO 2]/dt)=k1[ NO 2]2-k2[ N 2 O 4] ∴ Rate of disappearance of NO 2 i.e., -(d[ NO 2]/d t)=2 k1[ NO 2]2-2 k2[ N 2 O 4]

Q. In the reversible reaction,
$2 N O_{2} k_{2} ⇌ k_{1} N_{2} O_{4}$
the rate of disappearance of $N O_{2}$ is equal to

$\frac{2 k _{1}}{k _{2}} [N O_{2}]^{2}$

$2 k_{1} [N O_{2}]^{2} - 2 k_{2} [N_{2} O_{4}]$

$2 k_{1} [N O_{2}]^{2} - k_{2} [N_{2} O_{4}]$

$(2 k_{1} - k_{2}) [N O_{2}]$

$2 N O_{2} k_{2} ⇌ k_{1} N_{2} O_{4}$

Rate $= - \frac{1}{2} \frac{d [ N O _{2} ]}{d t} = k_{1} [N O_{2}]^{2} - k_{2} [N_{2} O_{4}]$

$∴$ Rate of disappearance of $N O_{2}$

i.e., $- \frac{d [ N O _{2} ]}{d t} = 2 k_{1} [N O_{2}]^{2} - 2 k_{2} [N_{2} O_{4}]$

Q. In the reversible reaction, 2NO2​k2​⇌k1​​​N2​O4​ the rate of disappearance of NO2​ is equal to

k2​2k1​​[NO2​]2

2k1​[NO2​]2−2k2​[N2​O4​]

2k1​[NO2​]2−k2​[N2​O4​]

(2k1​−k2​)[NO2​]