Which of the following order is incorrect ?

$\begin{array}{*{20}{c}}
{C{H_3}\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,C{H_3}\,\,\,\,\,\,\,\,\,\,}\\
{|\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,|\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,}\\
{C{H_3} - C{H_2} - C = C - CH - C - C{H_2} - C{H_2} - C{H_3}}\\
{|\,\,\,\,\,\,\,\,\,}\\
{{C_2}{H_5}}
\end{array}$

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The osmotic pressure of equimolar solutions of $BaCl_2, NaCl$ and glucose at same temperature follow the order

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$2.5 \mathrm{~g}$ of a non-volatile, non-electrolyte is dissolved in $100 \mathrm{~g}$ of water at $25^{\circ} \mathrm{C}$. The solution showed a boiling point elevation by $2^{\circ} \mathrm{C}$. Assuming the solute concentration in negligible with respect to the solvent concentration, the vapour pressure of the resulting aqueous solution is . . . . . . $\mathrm{mm}$ of $\mathrm{Hg}$ (nearest integer)

[Given : Molal boiling point elevation constant of water $\left(\mathrm{K}_{\mathrm{b}}\right)=0.52 \mathrm{K.} \mathrm{kg} \mathrm{mol}^{-1}$,

$1 \mathrm{~atm}$ pressure $=760 \mathrm{~mm}$ of $\mathrm{Hg}$, molar mass of water $\left.=18 \mathrm{~g} \mathrm{~mol}^{-1}\right\rfloor$

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Consider the following statements

$I.$ In gaseous phase, the vapour pressure of $CH_3COOH$ is less than expected.

$II.$ In benzene, acetic acid dimerises.

$III.\, CH_3OH$ is more viscous than $H_2O.$

$IV.\, CH_3OCH_3$ is non-polar but soluble in water.