For the reaction, N2O5 arrow 2NO2 + (1/2) O2 (-d[N2O5]/dt) = k1[N2O5] (d[NO2]/dt) = k2[N2O5] (d[O2]/dt) = k3 [N2O5] The relation in between k1 , k2 and k3 is

Question

For the reaction, N2O5 arrow 2NO2 + (1/2) O2 (-d[N2O5]/dt) = k1[N2O5] (d[NO2]/dt) = k2[N2O5] (d[O2]/dt) = k3 [N2O5] The relation in between k1 , k2 and k3 is (A)  2k1 = k2 = 4k3  (B)  k1 = k2 = k3  (C)  2k1 = 4k2 = k3  (D) None of these

Tardigrade Admin · Accepted Answer

The rate of reaction is given by (-d[N2O5]/dt) = + (1/2) (d[NO2]/dt) = +(2d[O2]/dt) Substituting the given values, we get k1[N2O5] = (1/2)k2[N2O5] = 2k3 [N2O5] or k1 = (k2/2) = 2 k3 or 2k1 = k2 = 4k3

Q. For the reaction,
$N_{2} O_{5} \to 2 N O_{2} + \frac{1}{2} O_{2}$
$\frac{- d [ N _{2} O _{5} ]}{d t} = k_{1} [N_{2} O_{5}]$
$\frac{d [ N O _{2} ]}{d t} = k_{2} [N_{2} O_{5}]$
$\frac{d [ O _{2} ]}{d t} = k_{3} [N_{2} O_{5}]$
The relation in between $k_{1}$ , $k_{2}$ and $k_{3}$ is

$2 k_{1} = k_{2} = 4 k_{3}$

$k_{1} = k_{2} = k_{3}$

$2 k_{1} = 4 k_{2} = k_{3}$

None of these

Q. For the reaction, N2​O5​→2NO2​+21​O2​ dt−d[N2​O5​]​=k1​[N2​O5​] dtd[NO2​]​=k2​[N2​O5​] dtd[O2​]​=k3​[N2​O5​] The relation in between k1​ , k2​ and k3​ is

2k1​=k2​=4k3​

k1​=k2​=k3​

2k1​=4k2​=k3​

None of these

The rate of reaction is given by dt−d[N2​O5​]​=+21​dtd[NO2​]​=+dt2d[O2​]​ Substituting the given values, we get k1​[N2​O5​]=21​k2​[N2​O5​]=2k3​[N2​O5​] or k1​=2k2​​=2k3​ or 2k1​=k2​=4k3​

Q. For the reaction,
$N_{2} O_{5} \to 2 N O_{2} + \frac{1}{2} O_{2}$
$\frac{- d [ N _{2} O _{5} ]}{d t} = k_{1} [N_{2} O_{5}]$
$\frac{d [ N O _{2} ]}{d t} = k_{2} [N_{2} O_{5}]$
$\frac{d [ O _{2} ]}{d t} = k_{3} [N_{2} O_{5}]$
The relation in between $k_{1}$ , $k_{2}$ and $k_{3}$ is

$2 k_{1} = k_{2} = 4 k_{3}$

$k_{1} = k_{2} = k_{3}$

$2 k_{1} = 4 k_{2} = k_{3}$