Final answer:
The mass of the aluminum foil with the given dimensions and density is 0.1376 grams, which corresponds to 0.00510 moles of aluminum when divided by the molar mass of aluminum. The available answer choices do not include this value, indicating a potential error.
Step-by-step explanation:
To determine how many moles of aluminum were used, we must first calculate the mass of the aluminum foil. Given the dimensions (1.00 cm square and 0.510 mm thick) and the density of aluminum (2.699 g/cm3), the volume of the foil can be calculated as the product of the area and the thickness. The mass is then the product of the volume and the density.
The calculation steps are as follows:
- Convert thickness from mm to cm: 0.510 mm = 0.0510 cm.
- Calculate volume: 1.00 cm * 1.00 cm * 0.0510 cm = 0.0510 cm3.
- Calculate mass: 0.0510 cm3 * 2.699 g/cm3 = 0.1376 g.
- Convert mass to moles using the molar mass of aluminum (approximately 26.98 g/mol): 0.1376 g / 26.98 g/mol = 0.00510 moles.
Considering the provided options for the mass of aluminum foil, none of them matches the calculated mass (0.1376 g), and it seems there might be a typographical error in the options. However, option (b) 0.0510 g is close to the volume in cm3, which may indicate a mix-up in the choices given.