MCQ
The compound that cannot be formed by xenon is
- A$XeO_3$
- B$XeF_4$
- ✓$XeCl_4$
- D$XeO_2F_2$
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$\begin{array}{*{20}{c}}
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,C{H_2}OC{H_3}} \\
| \\
{\mathop {C{H_3}CHBr}\limits_{(R)} }
\end{array}$ $\xrightarrow[{acetone}]{{NaCN}}$ $\begin{array}{*{20}{c}}
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,C{H_2}OC{H_3}} \\
| \\
{\mathop {C{H_3}CHCN}\limits }
\end{array}$
If $\mathop H\limits^ \oplus $ ion concentration is doubled, electrode potential of the half cell will
$3Br_2 + 6CO_3^{2-} + 3H_2O \longrightarrow 5Br^-+ BrO_3^-+ 6HCO_3^-$
Which of the following statements is true regarding this reaction
[Atomic Number: $\mathrm{Fe}=26, \mathrm{Mn}=25, \mathrm{Co}=27$ ]
| List-$I$ | List-$II$ |
| ($P$) $ t_{2 g}^6 e_g^0$ | ($1$)$\left[\mathrm{Fe}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+}$ |
| ($Q$) $t_{2 g}^3 e_g^2$ | ($2$) $\left[\mathrm{Mn}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+}$ |
| ($R$) $e^2 t_2^3$ | ($3$)$\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right]^{3+}$ |
| ($S$) $t_{2 g}^{+} e_g^2$ | ($4$)$\left[\mathrm{FeCl}_4\right]^{-}$ |
| $\left[\mathrm{CoCl}_4\right]^{2-}$ |