In a reversible expansion,one mole of gas is expanded isothermally at $200 \ K$ till its volume increases $10$ times. Calculate $\Delta S_{total}$ at equilibrium (in $J \ K^{-1}$)?

The positive value of $\Delta S$ indicates that

$\Delta S_{surr}$ for an exothermic reaction is

$A$ heat engine is operating between $500 \ K$ and $400 \ K$. If the engine absorbs $100 \ J$ of heat,which of the following is an impossible amount of heat rejected by the engine (in $J$)?

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?
$H_2O_{(l)} \to H_2O_{(g)}$ ... $J \, K^{-1} \, mol^{-1}$

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: