QuestionFor each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy $S$ of the system, decrease $S$, or leave $S$ unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column.
Note for advanced students: you may assume ideal gas and ideal solution behaviour. \begin{tabular}{|c|c|c|} \hline System & Change & $\Delta S$ \\ \hline A solution made of potassium chloride $(\mathrm{KCl})$ in water, at $80^{\circ} \mathrm{C}$. & 50. mL of pure water is added to the solution. & $\Delta S<0$ $\Delta S=0$ $\Delta S>0$ not enough information \\ \hline A mixture of krypton $(\mathrm{Kr})$ gas and xenon ( Xe ) gas at 2 atm and $47^{\circ} \mathrm{C}$. & An additional 2.0 L of pure Xe gas is added to the mixture, with the pressure kept constant at 2 atm . & $\Delta S<0$ $\Delta S=0$ $\Delta S>0$ not enough information \\ \hline 1.0 g of potassium chloride $(\mathrm{KCl})$ and 2.0 L of pure water at $80^{\circ} \mathrm{C}$, & The potassium chloride is dissolved in the water. & $\Delta S<0$ $\Delta S=0$ $\triangle S>0$ not enough information \\ \hline \end{tabular}