For a certain thermochemical reaction $M \rightarrow N$ at $T = 400 \ K$,$\Delta H^{\ominus} = 77.2 \ kJ \ mol^{-1}$ and $\Delta S = 122 \ J \ K^{-1} \ mol^{-1}$,the value of $\log K$ is $ . . . . . . \times 10^{-1}$.

For the reaction $Br_{2(l)} + Cl_{2(g)} \rightarrow 2BrCl_{(g)}$,the enthalpy change is $\Delta H = 30 \ kJ/mol$ and the entropy change is $\Delta S = 105 \ J/mol \cdot K$. The temperature at equilibrium is $...... \ K$.

At $25^{\circ} C$ and $1 \, atm$ pressure,the enthalpy of combustion of benzene$_{(l)}$ and acetylene$_{(g)}$ are $-3268 \, kJ \, mol^{-1}$ and $-1300 \, kJ \, mol^{-1}$,respectively. The change in enthalpy for the reaction $3 C_2H_{2(g)} \rightarrow C_6H_{6(l)}$ is $..... \, kJ \, mol^{-1}$.

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

Match the following terms in Column-$I$ with their corresponding descriptions in Column-$II$:

Column-$I$	Column-$II$
$(a)$ Adiabatic process	$(1)$ Heat
$(b)$ Isolated system	$(2)$ At constant volume
$(c)$ Isothermal change	$(3)$ First law of thermodynamics
$(d)$ Path function	$(4)$ No exchange of matter and energy
$(e)$ State function	$(5)$ No heat exchange
$(f)$ $\Delta U = q$	$(6)$ Constant temperature
$(g)$ Law of conservation of energy	$(7)$ Internal energy
$(h)$ Reversible process	$(8)$ $p_{ext} = 0$
$(i)$ Free expansion	$(9)$ At constant pressure
$(j)$ $\Delta H = q$	$(10)$ Infinitely slow process involving multiple equilibrium states
$(k)$ Intensive property	$(11)$ Entropy
$(l)$ Extensive property	$(12)$ Pressure,$(13)$ Specific heat

Chloroform has $\Delta H_{vaporization} = 29.2 \ kJ/mol$ and boils at $61.2 \ ^oC$. What is the value of $\Delta S_{vaporization}$ for chloroform? $...... \ J/mol \ K$