The value of $\Delta S$ for freezing of $10 \ g$ of $H_2O_{(l)}$ (enthalpy of fusion is $80 \ cal/g$) at $0 \ ^\circ C$ and $1 \ atm$ pressure is.......$J/K$

$A$ container is divided into two compartments by a removable partition as shown below:
In the first compartment,$n_{1}$ moles of ideal gas $He$ is present in a volume $V_{1}$. In the second compartment,$n_{2}$ moles of ideal gas $Ne$ is present in a volume $V_{2}$. The temperature and pressure in both the compartments are $T$ and $p$,respectively. Assuming $R$ is the gas constant,the total change in entropy upon removing the partition when the gases mix irreversibly is:

Statement-$1$: For a process at equilibrium,the total entropy is maximum and the change in total entropy is zero.
Statement-$2$: For a reversible process,if the same amount of heat is supplied to a system at two different temperatures,then the entropy change is less at a lower temperature.

For which one of the following reactions, the entropy change is positive?

The enthalpy change for the transition of liquid water to steam at $373 \, K$ is $40.8 \, kJ \, mol^{-1}$. What is the $\Delta S$ for the process in $J \, K^{-1} \, mol^{-1}$?

For the reaction $NH_4Cl_{(s)} \rightarrow NH_{3(g)} + HCl_{(g)}$,the entropy change is ...... .