How many particles are in 3.0 miles of aluminum?

To determine the number of particles (in this context, assuming atoms) in 3.0 miles of aluminum, you'd need additional information such as the dimensions of the aluminum, especially since aluminum doesn’t necessarily come in linear "miles". However, if we're considering a wire or some continuous piece of aluminum that extends for 3.0 miles, we can perform a calculation. We would do this by finding the volume of the aluminum, then using the density of aluminum to find the mass, and finally using Avogadro's number and the molar mass of aluminum to find the number of atoms.

The steps would be as follows: 1. Determine the volume of the aluminum in cubic centimeters (assuming you have the cross-sectional area). 2. Calculate the mass using the density of aluminum (assuming standard aluminum density of 2.70 g/cm³). 3. Use the molar mass of aluminum (approximately 26.98 g/mol) to find the number of moles. 4. Multiply the number of moles by Avogadro's number (6.022 x 10^23 atoms/mol) to find the number of aluminum atoms.

Since crucial information is missing (specifically the cross-sectional area or volume of the aluminum), I am unable to provide the exact number of particles without making a number of assumptions.