In an isolated system,find the condition for a spontaneous reaction.

The enthalpy change for the transition of liquid water to steam,$\Delta H_{vap} = 37.3 \ kJ \ mol^{-1}$ at $373 \ K$. The entropy change for the process is......$J \ mol^{-1} K^{-1}$.

At $298 \, K$ and $1 \, atm$ pressure,the entropies of $H_2(g)$,$Cl_2(g)$,and $HCl(g)$ are $130.6$,$223$,and $186.7 \, J \, K^{-1} \, mol^{-1}$ respectively. What is the entropy change for the reaction $H_2(g) + Cl_2(g) \rightarrow 2HCl(g)$ in $J \, K^{-1} \, mol^{-1}$?

Which of the following has the highest entropy?

Melting point of a solid is $x \ K$ and its latent heat of fusion is $600 \ cal \ mol^{-1}$. The entropy change for fusion of $1 \ mol$ solid is $2 \ cal \ mol^{-1} \ K^{-1}$. The value of $x$ will be......$K$

What is the entropy change in $J K^{-1}$ during the melting of $27.3 \ g$ of ice at $0^{\circ} C$? (Latent heat of fusion of ice $= 330 \ J g^{-1}$)