How many mg of iron ( \( \mathrm{MM}=55.845 \mathrm{~g} / \mathrm{mol}) \) are in 15.00 mL of a solution that contains \( 2.130 \mathrm{mg} \mathrm{Fe} / \) liter? Report your answer to the correct number of significant figures-in standord notation (Le.- not scientific notation). Omit the units.

To find the amount of iron in 15.00 mL of a solution that contains 2.130 mg of Fe per liter, we can use the following steps: 1. **Convert the volume from mL to L**: \[ 15.00 \, \text{mL} = 0.01500 \, \text{L} \] 2. **Calculate the amount of iron in 0.01500 L**: \[ \text{Amount of Fe} = \text{Concentration} \times \text{Volume} = 2.130 \, \text{mg/L} \times 0.01500 \, \text{L} \] 3. **Perform the multiplication**: \[ \text{Amount of Fe} = 2.130 \times 0.01500 = 0.03195 \, \text{mg} \] 4. **Report the answer with the correct number of significant figures**: The concentration (2.130 mg/L) has four significant figures, and the volume (0.01500 L) has four significant figures as well. Therefore, the final answer should also be reported with four significant figures. Thus, the amount of iron in 15.00 mL of the solution is: \[ \boxed{0.03195} \]