Carbon disulfide, $$\(\mathrm{CS}_{2}\)$$, is flammable and reacts readily with oxygen, as shown in reaction 1. $$\[ \text { reaction } 1 \quad \mathrm{CS}_{2}(\mathrm{~g})+3 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g})+2 \mathrm{SO}_{2}(\mathrm{~g}) \]$$ Table 3.1 shows the standard enthalpy of formation, $$\(\Delta H_{\mathrm{f}}^{\ominus}\)$$, and the standard entropy, $$\(S^{\ominus}\)$$, for some substances. Calculate the standard Gibbs free energy change, $$\(\Delta G^{\ominus}\)$$, in $$\(\mathrm{kJ} \mathrm{mol}^{-1}\)$$, for reaction 1 at $$\(25^{\circ} \mathrm{C}\)$$. $$\[ \Delta G^{\ominus}=\ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots \mathrm{kJ} \mathrm{mol}^{-1}\]$$

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