2. Calculate the mole of the following: a) 0.204 g of \( \mathrm{AgCl}(\mathrm{s}) \) b) 0.578 g of \( \mathrm{Fe}(\mathrm{s}) \)

To calculate the moles of a substance, you'll need to use the formula: \[ \text{Moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \] For \( \mathrm{AgCl} \), the molar mass is approximately 143.32 g/mol (107.87 g/mol for Ag and 35.45 g/mol for Cl). Thus, for 0.204 g of \( \mathrm{AgCl} \): \[ \text{Moles of } \mathrm{AgCl} = \frac{0.204 \, \text{g}}{143.32 \, \text{g/mol}} \approx 0.00142 \, \text{moles} \] For \( \mathrm{Fe} \), the molar mass is about 55.85 g/mol. Therefore, for 0.578 g of \( \mathrm{Fe} \): \[ \text{Moles of } \mathrm{Fe} = \frac{0.578 \, \text{g}}{55.85 \, \text{g/mol}} \approx 0.01035 \, \text{moles} \] Happy calculating!