How many grams do 6.2×1024 atoms of argon
weigh?
Answer in units of g.
How many mols Ar do you have? Since 1 mole contains 6.02E23 atoms, then 6.2E24 atoms of Ar will be
6.2E24/6.02E23 = # moles of Ar atoms.
Then since 1 mol Ar weighs 39.9 g, the your # mols will weigh what?
To find the weight of 6.2×10^24 atoms of argon, we need to use the atomic mass of argon and convert it to grams.
The atomic mass of argon (Ar) is approximately 39.95 g/mol.
Now, we will use the Avogadro's number (6.022 × 10^23 atoms/mol) to convert the given number of atoms to moles.
Number of moles = (6.2×10^24 atoms) / (6.022 × 10^23 atoms/mol)
≈ 10.28 moles
Finally, we can multiply the number of moles by the atomic mass of argon to find the weight.
Weight of argon = (10.28 mol) * (39.95 g/mol)
≈ 410.82 g
Therefore, 6.2×10^24 atoms of argon weigh approximately 410.82 grams (g).
To calculate the weight of atoms in grams, you need to use the concept of molar mass. Molar mass is the mass of one mole of a substance (atoms or molecules) and is expressed in grams per mole (g/mol).
To find the molar mass of argon (Ar), you can use the periodic table. The atomic mass of argon is approximately 39.95 g/mol.
Now, you have the number of atoms of argon, which is 6.2×10^24 atoms. To find the weight in grams, you need to multiply the number of atoms by the molar mass.
Weight in grams = Number of atoms × Molar mass
Weight in grams = 6.2×10^24 atoms × 39.95 g/mol
Calculating the above expression, we get:
Weight in grams ≈ 2.475 × 10^26 g
Therefore, 6.2×10^24 atoms of argon weigh approximately 2.475 × 10^26 grams.