The decomposition of Nitrogen pentoxide is given as 2N2O5→4NO2+O2. The rates of reaction are d[N2O5]dt=K1[N2O5], d[NO2]dt=K2[N2O5] and d[O2]dt=K3[N2O5]. Then the relation between K1,K2 & K3 is:

2N2O5→4NO2+O2r=−12d[N2O5]dt=+14d[NO2]dt=+d[O2]dt.⇒12K1[N2O5]=14K2[N2O5]=K3[N2O5]⇒K12=K24=K3⇒2K1=K2=4K3

The decomposition of Nitrogen pentoxide is given as 2N2O5→4NO2+O2. The rates of reaction are d[N2O5]dt=K1[N2O5], d[NO2]dt=K2[N2O5] and d[O2]dt=K3[N2O5]. Then the relation between K1,K2 & K3 is:

2N2O5→4NO2+O2r=−12d[N2O5]dt=+14d[NO2]dt=+d[O2]dt.⇒12K1[N2O5]=14K2[N2O5]=K3[N2O5]⇒K12=K24=K3⇒2K1=K2=4K3

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The decomposition of Nitrogen pentoxide is given as $2 N_{2} O_{5} \to 4 N O_{2} + O_{2} .$ The rates of reaction are $\frac{d [N_{2} O_{5}]}{d t} = K_{1} [N_{2} O_{5}]$ , $\frac{d [N O_{2}]}{d t} = K_{2} [N_{2} O_{5}]$ and $\frac{d [O_{2}]}{d t} = K_{3} [N_{2} O_{5}] .$ Then the relation between $K_{1}, K_{2} & K_{3}$ is:

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$K_{1} = K_{2} = K_{3}$

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

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

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

answer is B.

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Detailed Solution

$2 N_{2} O_{5} \to 4 N O_{2} + O_{2}$

$r = \frac{- 1}{2} \frac{d [N_{2} O_{5}]}{d t} = + \frac{1}{4} \frac{d [N O_{2}]}{d t} = + \frac{d [O_{2}]}{d t}$ .

$\Rightarrow \frac{1}{2} K_{1} [N_{2} O_{5}] = \frac{1}{4} K_{2} [N_{2} O_{5}] = K_{3} [N_{2} O_{5}]$

$\Rightarrow \frac{K_{1}}{2} = \frac{K_{2}}{4} = K_{3}$

$\Rightarrow 2 K_{1} = K_{2} = 4 K_{3}$

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The decomposition of Nitrogen pentoxide is given as 2N2O5→4NO2+O2. The rates of reaction are d[N2O5]dt=K1[N2O5], d[NO2]dt=K2[N2O5] and d[O2]dt=K3[N2O5]. Then the relation between K1,K2 & K3 is:

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