$(A)$ $\Delta G$ is positive $(B)$ $\Delta S _{\text {system }}$ is positive
$(C)$ $\Delta S _{\text {surroundings }}=0$ $(D)$ $\Delta H =0$
$\Delta S_{\text {surr }}=0 \quad \text { No heat exchange between solution and surrounding. } $
$\Delta H =0 \quad \text { For ideal solution. } $
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(Given : Molar Mass $\mathrm{Na}: 23$ and $\mathrm{Cl}: 35.5 \mathrm{gmol}^{-1}$ )
$ \mathrm{N}_2=3.0 \times 10^{-3} \mathrm{M}, \mathrm{O}_2=4.2 \times 10^{-3} \mathrm{M} \text { and } \mathrm{NO}=2.8 \times 10^{-3} \mathrm{M} . $
$ 2 \mathrm{NO}_{(\mathrm{g})} \rightleftharpoons \mathrm{N}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}$
If $0.1 \mathrm{~mol} \mathrm{~L} \mathrm{~L}^{-1}$ of $\mathrm{NO}_{(\mathrm{g})}$ is taken in a closed vessel, what will be degree of dissociation ( $\alpha$ ) of $\mathrm{NO}_{(\mathrm{g})}$ at equilibrium?