Import Question JSON

$\text{Hint:}$ $\Delta\text{S value is negative if}$ $\Delta\text{n}_g$ $\text{value is negative.}$ $\text{To determine the correct thermodynamic parameters for the reaction 2Cl(g)}$ $\rightarrow$ $\text{Cl}_2\text{(g), we need to analyze both the enthalpy and entropy changes:}$ $\text{Step 1: Analyze the entropy change (}\Delta_r\text{S)}$ $\text{For the given reaction:}$ $\text{2Cl(g)}$ $\rightarrow$ $\text{Cl}_2\text{(g)}$ $\text{The change in the number of gas molecules (}\Delta\text{n}_g\text{) is:}$ $\Delta\text{n}_g = \text{number of gaseous molecules in products - number of gaseous molecules in reactants}$ $\Delta\text{n}_g = 1 - 2 = -1$ $\text{Since}$ $\Delta\text{n}_g$ $\text{is negative, the entropy change (}\Delta_r\text{S) will also be negative.}$ $\text{This makes sense physically because:}$ $\text{- Two separate chlorine atoms have more disorder/randomness than one chlorine molecule}$ $\text{- The reaction decreases the total number of particles in the system}$ $\text{- Fewer particles generally means less disorder and lower entropy}$ $\text{Step 2: Analyze the enthalpy change (}\Delta_r\text{H)}$ $\text{This reaction represents the formation of a chlorine-chlorine bond:}$ $\text{Cl + Cl}$ $\rightarrow$ $\text{Cl}_2$ $\text{Bond formation is always an exothermic process, releasing energy. Therefore:}$ $\Delta_r\text{H} < 0$ $\text{This makes sense because:}$ $\text{- A more stable bond is being formed}$ $\text{- Energy is released when the bond forms}$ $\text{- The chlorine molecule has lower energy than the separate atoms}$ $\text{Combining our findings:}$ $\Delta_r\text{H} < 0 \text{ (negative enthalpy change - exothermic)}$ $\Delta_r\text{S} < 0 \text{ (negative entropy change - decrease in disorder)}$ $\text{Therefore, option 3 is the correct answer:}$ $\Delta_r\text{H} < 0 \text{ and } \Delta_r \text{S} < 0$