MCQ
Nitrogen forms how many oxides
- A$3$
- B$4$
- ✓$5$
- D$6$
$(i)$ $\underset{\begin{smallmatrix}
\text{Nitric oxide } \\
\text{Colourless gas}
\end{smallmatrix}}{\mathop{NO\,\,\,\,}}\,$
$(ii)$ $\underset{\begin{smallmatrix}
\text{Nitrous oxide} \\
\text{Colourless gas}
\end{smallmatrix}}{\mathop{{{N}_{2}}O\,\,\,}}\,$
$(iii)$ $\underset{\begin{smallmatrix}
\text{Dinitrogen } \\
\text{trioxide Blue}
\\
\text{liquid}
\end{smallmatrix}}{\mathop{{{N}_{2}}{{O}_{3}}}}\,$
$(iv)$ $\underset{\begin{smallmatrix}
\text{Dinitrogen} \\
\text{tetraoxide }
\\
\text{colourless liquid }
\end{smallmatrix}}{\mathop{{{N}_{2}}{{O}_{4}}\,\,\,\,\,\,\,}}\,$
$(v)$ $\underset{\begin{smallmatrix}
\text{Dinitrogen} \\
\text{pentaoxide}
\\
\text{colourless gas}
\end{smallmatrix}}{\mathop{{{N}_{2}}{{O}_{5}}\,\,\,\,\,}}\,$
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$2 C _{( s )}+ O _{2( g )} \rightarrow 2 CO ( g )$
When $12\,g$ carbon is burnt in $48\,g$ of oxygen, the volume of carbon monoxide produced is $......\times 10^{-1}\,L$ at STP [nearest integer]
[Given : Assume $CO$ as ideal gas, Mass of $C$ is $12\,g\,mol ^{-1}$, Mass of $O$ is $16\,g\,mol ^{-1}$ and molar volume of an ideal gas at STP is $22.7\,L\, mol ^{-1}$ ]
(Henry's law constant for $\mathrm{CO}_{2}$ at $298\, \mathrm{~K}$ is $1.67 \times 10^{3}$ $bar$)