MCQ
When $Pb{O_2}$ reacts with conc. $HN{O_3}$ the gas evolved is
- A$N{O_2}$
- ✓${O_2}$
- C${N_2}$
- D${N_2}O$
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$(I)$ $\begin{array}{*{20}{c}}
{{{(C{H_3})}_3}Si - NB{H_2}} \\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,|} \\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,Si{{(C{H_3})}_3}}
\end{array}$ $(II)$ $\begin{array}{*{20}{c}}
{{{(C{H_3})}_3}C - NB{H_2}} \\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,|} \\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,C{{(C{H_3})}_3}}
\end{array}$
| List$-I$ Reaction | List$-II$ Type of redox reaction | ||
| $(A)$ | $N _{2(g)}+ O _{2(g)} \rightarrow 2 NO _{( g )}$ | $(I)$ | Decomposition |
| $(B)$ | $2 Pb\left( NO _3\right)_{2(s)} \rightarrow 2 PbO _{( s )}+4 NO _{2(g)}+ O _{2(g)}$ | $(II)$ | Displacement |
| $(C)$ | $2 Na _{( s )}+2 H _2 O _{( l )} \rightarrow 2 NaOH _{( aq .)}+ H _{2(g)}$ | $(III)$ | Disproportionation |
| $(D)$ | $2 NO_{2(g)}+2 OH_{(aq)}^{-} \rightarrow NO_{2(qq)}^{-}+NO_{3(aq)}^{-}+H_2 O_{(l)}$ | $(IV)$ | Combination |