- A${E_n} = - \frac{{131.38}}{{{n^2}}}\,kJ\,mo{l^{ - 1}}$
- B${E_n} = - \frac{{131.33}}{n}\,kJ\,mo{l^{ - 1}}$
- ✓${E_n} = - \frac{{1313.3}}{{{n^2}}}\,kJ\,mo{l^{ - 1}}$
- D${E_n} = - \frac{{313.13}}{{{n^2}}}\,kJ\,mo{l^{ - 1}}$
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From above data what is the molecular mass of $CH_4$ containing all isotopes of carbon but hydrogen on ${}_1^1 H$ ................ $\mathrm{u}$ (Given that atomic mass of hydrogen $= 1.008$)
$\mathrm{Cd}_{(s)}+\mathrm{Hg}_{2} \mathrm{SO}_{4(s)}+\frac{9}{5} \mathrm{H}_{2} \mathrm{O}_{(l)} \rightleftharpoons \mathrm{CdSO}_{4} \cdot \frac{9}{5} \mathrm{H}_{2} \mathrm{O}_{(s)}+2 \mathrm{Hg}_{(l)}$
The value of $\mathrm{E}_{\text {cell }}^{0}$ is $4.315\, \mathrm{~V}$ at $25^{\circ} \mathrm{C}$. If $\Delta \mathrm{H}^{\circ}=-825.2\, \mathrm{~kJ} \,\mathrm{~mol}^{-1}$, the standard entropy change $\Delta \mathrm{S}^{\circ}$ in $\mathrm{J} \,\mathrm{K}^{-1}$ is ........ . (Nearest integer) [Given : Faraday constant $=96487\, \mathrm{C}\, \mathrm{mol}^{-1}$ ]
$[A]$ $\mathrm{A} 1\left(\mathrm{CH}_3\right)_3$ has the three-centre two-electron bonds in its dimeric structure
$[B]$ $\mathrm{BH}_3$ has the three-centre two-electron bonds in its dimeric structure
$[\mathrm{C}] \mathrm{AlCl}_3$ has the three-centre two-electron bonds in its dimeric structure
$[D]$ The Lewis acidity of $\mathrm{BCl}_5$ is greater than that of $\mathrm{AlCl}_5$