Which of the following statements is incorrect when a system consisting of an ideal gas undergoes a change of state?

Assertion : Water in liquid state is more stable than ice at room temperature.
Reason : Water in liquid form has higher entropy than ice.

Will ice at $273 \ K$ placed in a surrounding at $298 \ K$ melt to form water at $273 \ K$? Prove this statement. The molar enthalpy of fusion of ice is $6.025 \ kJ \ mol^{-1}$.

$A$ 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:

When two gases are mixed,the entropy $......$

Calculate the entropy change for the melting of $1 \, kg$ of ice at $0 \, ^\circ C$ in $SI$ units. (Latent heat of fusion of ice = $80 \, cal \, g^{-1}$) (in $.67$)