Calculate the enthalpy for the following reaction using the given bond energies (kJ/ mol)

$\left(\begin{array}{cc}\mathrm{C}-\mathrm{H}=414;& \mathrm{H}-\mathrm{O}=463;\\ \mathrm{H}-\mathrm{C}\mathrm{l}=431,& \mathrm{C}-\mathrm{C}\mathrm{l}=326;\\ \mathrm{C}-\mathrm{O}=335& \end{array}\right)$

$\mathrm{C}{\mathrm{H}}_3-\mathrm{O}\mathrm{H}\left(\mathrm{g}\right)+\mathrm{H}\mathrm{C}\mathrm{l}\left(\mathrm{g}\right)\to \mathrm{C}{\mathrm{H}}_3-\mathrm{C}\mathrm{l}\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

For which of the following systems, the difference between $\mathrm{\Delta H}$ and $\mathrm{\Delta U}$ is not significant?

(i) Solids

(ii) Gases

(iii) Mixture of gases and liquids

(iv) Liquids

$\mathrm{A}$ fish swimming in water body when taken out from the water body is covered with a film of water of weight $36 \mathrm{g}$. When it is subjected to cooking at $100 °\mathrm{C}$, then the internal energy for vaporization in ${\mathrm{kJmol}}^{-1}$ is integer]

[Assume steam to be an ideal gas. Given ${\mathrm{\Delta }}_{\mathrm{vap}}{\mathrm{H}}^{\ominus }$ for water at $373 \mathrm{K}$ and $1$ bar is $41.1 \mathrm{kJ}{ \mathrm{mol}}^{-1}:\mathrm{R}=8.31 \mathrm{J}{ \mathrm{K}}^{-1}{ \mathrm{mol}}^{-1}$]

The quantity of heat (in $J$) required to raise the temperature of $1.0\mathit{ }kg$ of ethanol from $293.45 K$ to the boiling point and then change the liquid to vapor at that temperature is closest to [Given, boiling point of ethanol $351.45 K$. Specific heat capacity of liquid ethanol $2.44\mathit{ }J\mathit{ }{g}^{-1} K^{-1}$. Latent heat of vaporisation of ethanol $855 J{g}^{-1}$ ]

The internal energy change (in $\mathrm{J}$) when $90 \mathrm{g}$ of water undergoes complete evaporation at $100°\mathrm{C}$ is ..............

(Given : ${\mathrm{\Delta H}}_{\mathrm{vap}}$ for water at $373 \mathrm{K}=41 \mathrm{kJ}/\mathrm{mol}$, $\mathrm{R}=8.314 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}$)