At $373 \, K$,steam and water are in equilibrium and $\Delta H = 39.2 \, kJ \, mol^{-1}$. What will be $\Delta S$ for the conversion of $1 \, mole$ of water into steam?
$H_2O_{(l)} \to H_2O_{(g)}$ ... $J \, K^{-1} \, mol^{-1}$

For an isolated system,$\Delta U = 0,$ what will be $\Delta S?$

The entropy change in the isothermal reversible expansion of $2 \, \text{moles}$ of an ideal gas from $10 \, L$ to $100 \, L$ at $300 \, K$ is $..... \, J \, K^{-1}$.

In which of the following processes does entropy increase?
$A$. $A$ liquid evaporates to vapour.
$B$. Temperature of a crystalline solid is lowered from $130 \ K$ to $0 \ K$.
$C$. $2 NaHCO_{3(s)} \rightarrow Na_2CO_{3(s)} + CO_{2(g)} + H_2O_{(g)}$
$D$. $Cl_{2(g)} \rightarrow 2 Cl_{(g)}$
Choose the correct answer from the options given below:

What is the unit of entropy?

In which state does matter have the highest entropy?