MCQ
Heating an aqueous solution of aluminium chloride to dryness will give:
- A$AlCl_3$
- B$Al_2Cl_6$
- ✓$Al_2O_3$
- D$Al(OH)Cl_2$
$\mathrm{AlCl}_{3}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{Al}(\mathrm{OH})_{3}+\mathrm{HCl}$
On strongly heating $\mathrm{Al}(\mathrm{OH})_{3}$ is converted into $\mathrm{Al}_{2} \mathrm{O}_{3}$
$\mathrm{Al}(\mathrm{OH})_{3} \rightarrow \mathrm{Al}_{2} \mathrm{O}_{3}+3 \mathrm{H}_{2} \mathrm{O}$
$\mathrm{AlCl}_{3}$ on heating gives $\mathrm{Al}_{2} \mathrm{O}_{3}$
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The equilibrium constant of the reaction $2N{H_3} + \frac{5}{2}{O_2} \rightleftharpoons 2NO + 3{H_2}O$ in terms of $K_1, K_2$ and $K_3$ is
$(i)\,\begin{array}{*{20}{c}}
{C{H_3} - \mathop C\limits^ \oplus - C{H_3}} \\
| \\
{\,\,\,\,\,\,OC{H_3}}
\end{array}$
$(ii)\,\begin{array}{*{20}{c}}
{C{H_3} - \mathop C\limits^ \oplus - C{H_3}} \\
| \\
{\,\,\,\,\,\,C{H_3}}
\end{array}$
$(iii)\begin{array}{*{20}{c}}
{C{H_3} - \mathop C\limits^ \oplus {H_2} - NH} \\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,|} \\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,C{H_3}}
\end{array}$
$(iv)\,C{H_3} - \mathop C\limits^ \oplus {H_2}$