MCQ
The oxide without nitrogen-nitrogen bond is :
- A$\mathrm{N}_{2} \mathrm{O}$
- B$\mathrm{N}_{2} \mathrm{O}_{4}$
- C$\mathrm{N}_{2} \mathrm{O}_{3}$
- ✓$\mathrm{N}_{2} \mathrm{O}_{5}$

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The rate constants of the above reaction at $200 \,K$ and $300 \,K$ are $0.03 \,min ^{-1}$ and $0.05 \,min ^{-1}$ respectively. The activation energy for the reaction is $....J$ (Nearest integer)
(Given : In $10=2.3$
$R =8.3\,J\,K ^{-1}\, mol ^{-1}$
$\log 5=0.70$
$\log 3=0.48$
$\log 2=0.30$
