What is the average mass of a single aluminum atom in grams?
How do I solve this? I got 4.482 x 10^23. I divided 26.986/6.02x10^23
To find the average mass of a single aluminum atom, you need to use the molar mass concept.
1. First, you'll need to find the molar mass of aluminum (Al). The atomic mass of aluminum is 26.986 grams per mole (g/mol). This value represents the average mass of one mole of aluminum atoms.
2. Next, you need to convert this molar mass to grams per atom. Since there are Avogadro's number (6.02 x 10^23) atoms in one mole of any substance, you divide the molar mass by Avogadro's number to find the mass of one atom.
Let's calculate it step by step:
Molar mass of aluminum (Al) = 26.986 g/mol
Average mass of one aluminum atom = Molar mass of aluminum / Avogadro's number
= 26.986 g/mol / (6.02 x 10^23)
Calculating the division, we get:
Average mass of one aluminum atom ≈ 4.482 x 10^-23 grams
So, your calculation is correct. The average mass of a single aluminum atom is approximately 4.482 x 10^-23 grams.
Your method is OK but your math is lousy.
Should that be 4.48E-23.