The change of entropy $(dS)$ is defined as

In a reversible adiabatic process $\Delta S$ is :-

At $300 \ K$,for the reaction $A \rightarrow P$,the $\Delta S_{sys}$ is $5 \ J \ K^{-1} \ mol^{-1}$. What is the heat absorbed (in $kJ \ mol^{-1}$) by the system?

The latent heat of melting of ice at $0^{\circ} C$ is $6 \, kJ \, mol^{-1}$. The entropy change during the melting in $J \, K^{-1} \, mol^{-1}$ is closest to

Given $\Delta S_{Total} = -40 \ kJ/mol \cdot K$,$\Delta H_{System} = 2000 \ kJ/mol$,and $T = 400 \ K$. Find the value of $\Delta S_{System}$ in $kJ/mol \cdot K$.

The increase in entropy in $J K^{-1}$ of a substance when it absorbs $1 \ kJ$ of heat energy at $3 \ K$ is