Calculate the sign of $\Delta S$ for the melting of ice at $275 \ K$.

Explain entropy and spontaneity of reactions.

What is the change in entropy in $J \ K^{-1} \ mol^{-1}$ for the conversion of $1 \ mol$ of ice to water at $0 \, ^\circ C$? For the process $H_2O_{(s)} \rightarrow H_2O_{(l)}$ at $0 \, ^\circ C$,$\Delta H_{fus} = 6 \, kJ \ mol^{-1}$.

In which of the following reactions is $\Delta S$ positive?

What is the unit of $\Delta S_m^\circ$?

For which one of the following reactions is the entropy change positive?