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:

The entropy change involved in the isothermal reversible expansion of $2 \, \text{mole}$ of an ideal gas from a volume of $10 \, dm^3$ to a volume of $100 \, dm^3$ at $27 \, ^oC$ is : .............. $J \, K^{-1}$

Which of the following equations indicates an increase in entropy?

Which of the following statements is correct?

$30.4 \, kJ$ of heat is required to melt one mole of sodium chloride and the entropy change at the melting point is $28.4 \, J \, K^{-1} \, mol^{-1}$ at $1 \, atm$. The melting point of sodium chloride is $........... \, K$ (Nearest Integer).

Find the change in entropy for the fusion of $1 \, mol$ of ice in $J \, K^{-1} \, mol^{-1}$. The melting point of water is $273 \, K$ and the molar enthalpy of fusion for water is $6.0 \, kJ \, mol^{-1}$.