During which of the following processes, does entropy decrease ?

(A) Freezing of water to ice at $0°\mathrm{C}$
(B) Freezing of water to ice at $-10°\mathrm{C}$
(C) ${\mathrm{N}}_2( \mathrm{g})+3{\mathrm{H}}_2( \mathrm{g})\to 2{\mathrm{NH}}_3( \mathrm{g})$
(D) Adsorption of $\mathrm{CO}\left(\mathrm{g}\right)$ and lead surface
(E) Dissolution of $\mathrm{NaCl}$ in water

The point of intersection and sudden increase in the slope, in the diagram given below, respectively, indicates:

The standard enthalpies of formation of ${\mathrm{Al}}_2{\mathrm{O}}_3$ and $\mathrm{CaO}$ are $-1675 \mathrm{kJ}{ \mathrm{mol}}^{-1}$ and $-635 \mathrm{kJ}{ \mathrm{mol}}^{-1}$ respectively.

For the reaction

$3\mathrm{CaO}+2\mathrm{Al}\to 3\mathrm{Ca}+{\mathrm{Al}}_2{\mathrm{O}}_3$ the standard reaction enthalpy ${\mathrm{\Delta }}_{\mathrm{r}}{\mathrm{H}}^0=$ ________ $\mathrm{kJ}.$

(Round off to the Nearest Integer).

At $25°\mathrm{C},50 \mathrm{g}$ of iron reacts with $\mathrm{HCl}$ to form ${\mathrm{FeCl}}_2$. The evolved hydrogen gas expands against a constant pressure of $1 \mathrm{bar}$. The work done by the gas during this expansion is -_______ $\mathrm{J}$.

(Round off to the Nearest Integer)

[Given : $\mathrm{R}=8.314 \mathrm{J}{ \mathrm{mol}}^{-1}{ \mathrm{K}}^{-1}$. Assume, hydrogen is an ideal gas]

[Atomic mass off Fe is $55.85 \mathrm{u}$]

For the reaction $\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{B}\left(\mathrm{g}\right)$ at $495 \mathrm{K}$, ${\mathrm{\Delta }}_{\mathrm{r}}{\mathrm{G}}^{°}=-9.478 \mathrm{kJ} {\mathrm{mol}}^{-1}$

If we start the reaction in a closed container at $495 \mathrm{K}$ with $22$ millimoles of $\mathrm{A}$, the amount of $\mathrm{B}$ is the equilibrium mixture is ________ millimoles. (Round off to the Nearest Integer).

$\left[\mathrm{R}=8.314 \mathrm{J} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1};\ell \mathrm{n}10=2.303\right]$