Import Question JSON

\textbf{Hint:} \text{An isolated system, exchange of heat and matter does not take place between system and surrounding.} \text{Since the system is isolated, no heat can escape it (the process is thus adiabatic), so when this flow of energy disperses inside the system, the entropy of the system increases, i.e. } \Delta S_{\text{sys}} > 0\text{. Hence, the entropy of the system must increase for a spontaneous process in this isolated system.} \text{So, } \Delta S \text{ will be positive and the reaction will be spontaneous.} \text{For an isolated system:} \bullet \text{ No exchange of heat or matter with surroundings} \bullet \text{ The process is adiabatic } (q = 0) \bullet \text{ Given that } \Delta U = 0 \text{ (no change in internal energy)} \text{According to the Second Law of Thermodynamics, for any spontaneous process in an isolated system, the total entropy must increase. This is because:} \bullet \text{ Energy tends to disperse and spread out within the system} \bullet \text{ Even with no net change in internal energy } (\Delta U = 0)\text{, energy redistribution occurs} \bullet \text{ This redistribution leads to increased disorder and higher entropy} \text{The entropy change for the universe in an isolated system is:} \Delta S_{\text{universe}} = \Delta S_{\text{system}} + \Delta S_{\text{surroundings}} = \Delta S_{\text{system}} + 0 = \Delta S_{\text{system}} \text{For a spontaneous process: } \Delta S_{\text{universe}} > 0 \text{Therefore: } \Delta S_{\text{system}} > 0 \text{Therefore, option (1) is correct.}