Final answer:
The mass of 4.60 x 10^21 particles of aluminum is approximately 0.206 g, calculated using Avogadro's number and the molar mass of aluminum.
Step-by-step explanation:
To determine the mass of 4.60 x 10^21 particles of aluminum (Al), we first need to understand the concept of molar mass and Avogadro's number.
The molar mass of aluminum is 26.98 g/mol, and Avogadro's number is approximately 6.022 x 10^23, which is the number of atoms or molecules in one mole of a substance.
The calculation involves using the ratio of particles to moles and then moles to grams. Here is the process:
Next, convert moles of Al to grams using the molar mass of Al: (7.64 x 10^-3 mol Al) x (26.98 g/mol Al) = 0.206 g Al.
The calculated value makes sense and is expressed to four significant figures: the mass of 4.60 x 10^21 particles of aluminum is approximately 0.206 g.