How many grams of Cl are in a \( 38.0-\mathrm{g} \) sample of the chlorofluorocarbon \( \mathrm{CF}_{2} \mathrm{Cl}_{2} \) ? Express your answers in grams of chlorine to three significant figures. \( \square \sqrt[\square]{\square} \mathrm{A} \phi \) ?

To find the amount of chlorine (Cl) in a \( 38.0 \, \text{g} \) sample of the chlorofluorocarbon \( \text{CF}_2\text{Cl}_2 \), we first need to determine the molar mass of \( \text{CF}_2\text{Cl}_2 \). 1. **Calculate the molar mass of \( \text{CF}_2\text{Cl}_2 \)**: - Carbon (C): \( 1 \times 12.01 \, \text{g/mol} = 12.01 \, \text{g/mol} \) - Fluorine (F): \( 2 \times 19.00 \, \text{g/mol} = 38.00 \, \text{g/mol} \) - Chlorine (Cl): \( 2 \times 35.45 \, \text{g/mol} = 70.90 \, \text{g/mol} \) Now, add these together: \[ \text{Molar mass of } \text{CF}_2\text{Cl}_2 = 12.01 + 38.00 + 70.90 = 120.91 \, \text{g/mol} \] 2. **Determine the mass fraction of chlorine in \( \text{CF}_2\text{Cl}_2 \)**: - Total mass of chlorine in one mole of \( \text{CF}_2\text{Cl}_2 \) is \( 70.90 \, \text{g} \). - The mass fraction of chlorine is: \[ \text{Mass fraction of Cl} = \frac{70.90 \, \text{g}}{120.91 \, \text{g}} \approx 0.585 \] 3. **Calculate the mass of chlorine in the \( 38.0 \, \text{g} \) sample**: \[ \text{Mass of Cl} = 38.0 \, \text{g} \times 0.585 \approx 22.23 \, \text{g} \] 4. **Express the answer in three significant figures**: \[ \text{Mass of Cl} \approx 22.2 \, \text{g} \] Thus, the mass of chlorine in a \( 38.0 \, \text{g} \) sample of \( \text{CF}_2\text{Cl}_2 \) is \( \boxed{22.2} \, \text{g} \).