MCQ
The oxidation state of $Mn$ in ${K_2}Mn{O_4}$
- A$+2$
- B$+7$
- C$-2$
- ✓$+6$
$2 + x - 2 \times 4 = 0$
$x = 8 - 2 = + 6$.
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|
List-$I$ Reaction |
List-$II$ Type of redox reaction |
| $(A)$ $\mathrm{N}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{NO}_{(\mathrm{g})}$ | $(I)$ Decomposition |
| $(B)$ $\begin{aligned} & 2 \mathrm{~Pb}\left(\mathrm{NO}_3\right)_{2(\mathrm{~s})} \rightarrow 2 \mathrm{PbO}_{(\mathrm{s})}+4 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}\end{aligned}$ | $(II)$ Displacement |
| $(C)$ $\begin{aligned} 2 \mathrm{Na}_{(\mathrm{s})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})} \rightarrow 2 \mathrm{NaOH}_{(\mathrm{aq} .)}+\mathrm{H}_{2(\mathrm{~g})}\end{aligned}$ | $(III)$ Disproportionation |
| $(D)$ $\begin{aligned} 2 \mathrm{NO}_{2(\mathrm{~g})}+2-\mathrm{OH}_{(\mathrm{aq})} \rightarrow \mathrm{NO}_{2(\mathrm{aq} .)}^{-}+\mathrm{NO}_{3(\mathrm{qq} .)}^{-}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}\end{aligned}$ | $(IV)$ Combination |
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