The enthalpy change for the transition of liquid water to steam at $373 \, K$ is $40.8 \, kJ \, mol^{-1}$. What is the $\Delta S$ for the process in $J \, K^{-1} \, mol^{-1}$?

Heat has a randomizing influence on a system,and temperature is the measure of the average chaotic motion of particles in the system. Write the mathematical relation that relates these three parameters.

For which of the following processes,$\Delta S$ is negative?

Calculate the entropy change for melting $1 \ g$ of ice at $0^{\circ} C$ in $J \ g^{-1} K^{-1}$,if the heat of fusion of ice at $0^{\circ} C$ is $80 \ J \ g^{-1}$.

The entropy values (in $J K^{-1} mol^{-1}$) of $H_{2(g)} = 130.6$,$Cl_{2(g)} = 223.0$ and $HCl_{(g)} = 186.7$ at $298 \ K$ and $1 \ atm$ pressure. Then entropy change for the reaction $H_{2(g)} + Cl_{2(g)} \to 2HCl_{(g)}$ is :-

If the standard molar entropies $(S^o)$ for $H_2$,$Cl_2$,and $HCl$ are $0.13$,$0.22$,and $0.19 \, kJ \, K^{-1} \, mol^{-1}$ respectively,what is the total change in standard entropy $(\Delta S^o)$ for the reaction $H_2 + Cl_2 \rightarrow 2HCl$ in $J \, K^{-1} \, mol^{-1}$?