What is the theoretical yield of \( \mathrm{Cl}_{2} \) ? theoretical yield:

To calculate the theoretical yield of \( \mathrm{Cl}_{2} \) (chlorine gas), we need to know the balanced chemical equation for the reaction that produces \( \mathrm{Cl}_{2} \) and the amounts of reactants used. For example, if we consider the reaction of hydrochloric acid (\( \mathrm{HCl} \)) with manganese dioxide (\( \mathrm{MnO}_2 \)) to produce chlorine gas, the balanced equation is: \[ 4 \, \mathrm{HCl} + \mathrm{MnO}_2 \rightarrow \mathrm{Cl}_2 + \mathrm{MnCl}_2 + 2 \, \mathrm{H}_2\mathrm{O} \] From this equation, we can see that 4 moles of \( \mathrm{HCl} \) produce 1 mole of \( \mathrm{Cl}_2 \). To calculate the theoretical yield, follow these steps: 1. **Determine the moles of the limiting reactant**: Identify which reactant will produce the least amount of \( \mathrm{Cl}_2 \) based on the stoichiometry of the reaction. 2. **Use stoichiometry to find moles of \( \mathrm{Cl}_2 \)**: Use the mole ratio from the balanced equation to convert moles of the limiting reactant to moles of \( \mathrm{Cl}_2 \). 3. **Convert moles of \( \mathrm{Cl}_2 \) to grams (if needed)**: Use the molar mass of \( \mathrm{Cl}_2 \) (approximately 70.90 g/mol) to convert moles to grams. If you provide the specific amounts of reactants used in your reaction, I can help you calculate the theoretical yield of \( \mathrm{Cl}_2 \).