The number of endothermic process/es from the following is:
$A. I_{2(g)} \rightarrow 2I_{(g)}$
$B. HCl_{(g)} \rightarrow H_{(g)} + Cl_{(g)}$
$C. H_2O_{(l)} \rightarrow H_2O_{(g)}$
$D. C_{(s)} + O_{2(g)} \rightarrow CO_{2(g)}$
$E. \text{Dissolution of ammonium chloride in water}$

One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of $27\,^oC$. If the work done during the process is $3\,kJ$,the final temperature will be equal to $(C_v = 20\,J\,K^{-1} \, mol^{-1})$

$\Delta H^o_f$ of water is $-285.5 \, kJ \, mol^{-1}$. If enthalpy of neutralisation of monoacidic strong base is $-57.3 \, kJ \, mol^{-1}$,$\Delta H^o_f$ of $OH^{-}$ ion will be.....$kJ \, mol^{-1}$

For a spontaneous process, the correct statement$(s)$ is (are):

$A$ fish swimming in a water body,when taken out,is covered with a film of water of weight $36 \ g$. When it is subjected to cooking at $100^{\circ} C$,the internal energy change for vaporization in $kJ \ mol^{-1}$ is $......$ [nearest integer].
[Assume steam to be an ideal gas. Given $\Delta_{vap} H^{\ominus}$ for water at $373 \ K$ and $1 \ bar$ is $41.1 \ kJ \ mol^{-1}$; $R = 8.31 \ J \ K^{-1} \ mol^{-1}$]

Consider the reversible processes for $1.0 \ mol$ of an ideal gas. $w_1, w_2, w_3$ and $w_4$ represent work done (in calories) in the processes $1, 2, 3$ and $4$, respectively; $\Delta U_2$ and $\Delta U_4$ are changes in the internal energy for the processes $2$ and $4$, respectively. (use $R = 2 \ cal \ K^{-1} \ mol^{-1}$). The correct option is: