Determine the limiting reactant. \( \mathrm{CS}_{2}(\mathrm{~g})+3 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g})+2 \mathrm{SO}_{2}(\mathrm{~g}) \) Express your answer as a chemical formula. \( \square \) A chemical reaction does not occur for this question.

We begin with the balanced chemical equation \[ \mathrm{CS}_2 + 3\,\mathrm{O}_2 \rightarrow \mathrm{CO}_2 + 2\,\mathrm{SO}_2. \] To determine the limiting reactant, we need to know the amount (in moles or mass) of each reactant present. In general, if we denote the number of moles of \(\mathrm{CS}_2\) as \(n_{\mathrm{CS}_2}\) and of \(\mathrm{O}_2\) as \(n_{\mathrm{O}_2}\), we compare the mole ratio required by the balanced equation to the mole ratio available. The reaction requires 3 moles of \(\mathrm{O}_2\) for every 1 mole of \(\mathrm{CS}_2\). Thus, one approach is to compute \[ \text{Required moles of } \mathrm{O}_2 = 3 \, n_{\mathrm{CS}_2}. \] Then, if - \(n_{\mathrm{O}_2} < 3\,n_{\mathrm{CS}_2}\), \(\mathrm{O}_2\) is the limiting reactant. - \(n_{\mathrm{O}_2} > 3\,n_{\mathrm{CS}_2}\), \(\mathrm{CS}_2\) is the limiting reactant. - \(n_{\mathrm{O}_2} = 3\,n_{\mathrm{CS}_2}\), the reactants are exactly enough to react completely. Because no numerical amounts are provided, there is no basis for choosing one reactant over the other. Without an initial quantity (mass, volume, or moles) for either reactant, it is impossible to determine which one is limiting. Therefore, since no quantities are provided, we cannot determine a unique limiting reactant. \[ \boxed{\text{Insufficient data}} \]