If the original sample of Zn had a mass of 1.4 g , what mass of \( \mathrm{ZnCl}_{2} \) can be produced in the reaction?

To determine the mass of \( \mathrm{ZnCl}_{2} \) that can be produced from a given mass of zinc (Zn), we first need to know the balanced chemical equation for the reaction between zinc and chlorine gas (Cl\(_2\)) to form zinc chloride (ZnCl\(_2\)): \[ \mathrm{Zn} + \mathrm{Cl}_2 \rightarrow \mathrm{ZnCl}_2 \] From the balanced equation, we can see that 1 mole of zinc reacts with 1 mole of chlorine gas to produce 1 mole of zinc chloride. Next, we need to calculate the number of moles of zinc in the original sample: 1. **Calculate the molar mass of Zn:** - The molar mass of Zn is approximately 65.38 g/mol. 2. **Calculate the number of moles of Zn:** \[ \text{moles of Zn} = \frac{\text{mass of Zn}}{\text{molar mass of Zn}} = \frac{1.4 \, \text{g}}{65.38 \, \text{g/mol}} \approx 0.0214 \, \text{mol} \] 3. **Using the stoichiometry of the reaction:** - From the balanced equation, 1 mole of Zn produces 1 mole of ZnCl\(_2\). Therefore, the moles of ZnCl\(_2\) produced will also be 0.0214 mol. 4. **Calculate the mass of ZnCl\(_2\):** - First, we need the molar mass of ZnCl\(_2\): - Molar mass of Zn = 65.38 g/mol - Molar mass of Cl = 35.45 g/mol - Molar mass of ZnCl\(_2\) = 65.38 g/mol + 2 × 35.45 g/mol = 65.38 g/mol + 70.90 g/mol = 136.28 g/mol 5. **Now calculate the mass of ZnCl\(_2\):** \[ \text{mass of ZnCl}_2 = \text{moles of ZnCl}_2 \times \text{molar mass of ZnCl}_2 = 0.0214 \, \text{mol} \times 136.28 \, \text{g/mol} \approx 2.91 \, \text{g} \] Therefore, the mass of \( \mathrm{ZnCl}_{2} \) that can be produced from 1.4 g of Zn is approximately **2.91 g**.