Calculate the sign of $\Delta S$ for the melting of ice at $275 \ K$.

When $2 \ mol$ of an ideal gas $\left( C_{p,m} = \frac{5}{2} R \right)$ is heated from $300 \ K$ to $600 \ K$ at constant pressure,the change in entropy of the gas $\left( \Delta S \right)$ is:

In which of the following reactions is $\Delta S$ maximum?

The enthalpy change for the conversion of water into vapor at $27^\circ C$ is $30 \ kJ/mol$. The entropy change for this process in $J/mol \ K$ is:

What is the entropy of vaporisation of water at $100\,^{\circ}C$,if the molar heat of vaporisation is $9710\,cal/mol$?

Which of the following statements is correct?