Dry ice (solid carbon dioxide, CO2\text{CO}_2CO2) undergoes sublimation at room temperature and pressure to form carbon dioxide gas. Which option correctly describes the enthalpy change (ΔH\Delta HΔH), the primary forces overcome, and the change in molecular arrangement during this change of state?
Enthalpy change: Endothermic (ΔH>0\Delta H > 0ΔH>0); Forces overcome: Weak intermolecular (London dispersion) forces; Arrangement change: From a highly ordered molecular lattice to a highly disordered, widely spaced distribution
Enthalpy change: Exothermic (ΔH<0\Delta H < 0ΔH<0); Forces overcome: Weak intermolecular (London dispersion) forces; Arrangement change: From a closely-packed random arrangement to a regular crystalline lattice
Enthalpy change: Endothermic (ΔH>0\Delta H > 0ΔH>0); Forces overcome: Strong covalent C=O\text{C}=\text{O}C=O double bonds; Arrangement change: From a highly ordered molecular lattice to a highly disordered, widely spaced distribution
Enthalpy change: Exothermic (ΔH<0\Delta H < 0ΔH<0); Forces overcome: Strong covalent C=O\text{C}=\text{O}C=O double bonds; Arrangement change: From a regular crystalline lattice to a closely-packed random arrangement
