Consider the reaction:
\[ \text{C (graphite)} + 2\text{Cl}_2 \text{(g)} \rightarrow \text{CCl}_4 \text{(l)} \]
\[ \Delta^\circ = -139 \text{ kJ/mol} \]

Calculate the quantities for \(\Delta S_{\text{sys}}\), \(\Delta S_{\text{surr}}\), \(\Delta S_{\text{univ}}\).

a) \(\Delta S_{\text{sys}} = -139 \text{ J/K}\), \(\Delta S_{\text{surr}} = 139 \text{ J/K}\), \(\Delta S_{\text{univ}} = 0 \text{ J/K}\)

b) \(\Delta S_{\text{sys}} = 0 \text{ J/K}\), \(\Delta S_{\text{surr}} = 139 \text{ J/K}\), \(\Delta S_{\text{univ}} = 139 \text{ J/K}\)

c) \(\Delta S_{\text{sys}} = 139 \text{ J/K}\), \(\Delta S_{\text{surr}} = -139 \text{ J/K}\), \(\Delta S_{\text{univ}} = 0 \text{ J/K}\)

d) \(\Delta S_{\text{sys}} = 139 \text{ J/K}\), \(\Delta S_{\text{surr}} = 0 \text{ J/K}\), \(\Delta S_{\text{univ}} = 139 \text{ J/K}\)

Without additional data such as standard entropy values for reactants and products, we cannot calculate the precise entropy changes (ΔSsys, ΔSsurr, ΔSuniv) for the provided chemical reaction.

Explanation:

The question pertains to the calculation of entropy changes in a chemical reaction, specifically the formation of carbon tetrachloride from graphite and chlorine gas. The given reaction is C (graphite) + 2Cl2 (g) → CCl4 (l) with an enthalpy change (ΔH°) of -139 kJ/mol. While the student provided potential answers for changes in system entropy (ΔSsys), surrounding entropy (ΔSsurr), and universal entropy (ΔSuniv), we cannot definitively ascertain these values without additional data such as entropy values of reaction species or further context on reaction conditions. Therefore, without the necessary standard entropy data (ΔS°) for reactants and products, we cannot calculate the precise entropy changes. The Gibbs free energy change (ΔG°) can be related to both the enthalpy (ΔH°) and entropy (ΔS°) changes at a constant temperature using the equation ΔG° = ΔH° - TΔS°, but data are incomplete to solve for ΔS° in this scenario.