$\pi_{2 p_{x}}^{2}=\pi_{2 p_{y}}^{2}, \pi_{2 p_{x}}^{*_{1}}=\pi_{2 p_{y}}^{*_{1}}, \sigma_{2 p_{2}}^{*}$
Bond order of $\mathrm{O}_{2} \Rightarrow 2$
Bond order of $\mathrm{O}_{2}^{-} \Rightarrow 1.5$
Bond order of $\mathrm{O}_{2}^{2-} \Rightarrow 1$
Bond order of $\mathrm{O}_{2}^{+} \Rightarrow 2.5$
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In the above first order reaction the initial concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ is $2.40 \times 10^{-2}\, \mathrm{~mol} \,\mathrm{~L}^{-1}$ at $318 \,K.$ The concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ after $1\, hour$ was $1.60 \times 10^{-2}\, \mathrm{~mol} \,\mathrm{~L}^{-1}$, The rate constant of the reaction at $318\, \mathrm{~K}$ is $.....\,\times 10^{-3} \mathrm{~min}^{-1}$. (Nearest integer)
[Given: $\log 3=0.477, \log 5=0.699$ ]
|
List $-I$ (Element) |
List $-II$ (Electronic Configuration) | ||
| $A.$ | $N$ | $I.$ | $[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^2 4 \mathrm{p}^5$ |
| $B.$ | $S$ | $II.$ | $[\mathrm{Ne}] 3 \mathrm{~s}^2 3 \mathrm{p}^4$ |
| $C.$ | $Br$ | $III.$ | $[\mathrm{He}] 2 \mathrm{~s}^2 2 \mathrm{p}^3$ |
| $D.$ | $Kr$ | $IV.$ | $[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^2 4 \mathrm{p}^6$ |
Choose the correct answer from the options given below:
$A+B\xrightarrow{K}C$
Rate Order