Question

How many grams of aluminum are equivalent to 1.20 X 10^24 atoms?

a.) 0.0739 g
b.) 2.68 X 10^46 g
c.) 13.5g
d.) 53.8g

Answer 1

To find out how many grams of aluminum are equivalent to 1.20 x 10^24 atoms, one must calculate the number of moles using Avogadro's number and then multiply by the molar mass of aluminum, resulting in 53.8 grams. So the correct option is d.

Step-by-step explanation:

To determine the mass of aluminum that is equivalent to 1.20 x 1024 atoms, we need to use Avogadro's number and the molar mass of aluminum. Avogadro's number tells us how many atoms are in one mole, which is approximately 6.022 x 1023 atoms. The molar mass of aluminum is 26.98 grams per mole. Therefore, to calculate the mass of 1.20 x 1024 aluminum atoms, we perform the following calculation:

1. Divide the number of atoms by Avogadro's number to find the number of moles of aluminum: 1.20 x 1024 atoms / 6.022 x 1023 atoms/mol.
2. Multiply the number of moles of aluminum by the molar mass of aluminum to find the mass in grams: Moles of Al x 26.98 g/mol.

Performing this calculation gives us:

1.20 x 1024 atoms / 6.022 x 1023 atoms/mol ≈ 1.99 moles of Al

1.99 moles of Al x 26.98 g/mol = 53.7 grams of Al

Therefore, the answer is 53.8 grams of aluminum, which corresponds to option (d).

Answer 2

Answer: 35.9 g

Step-by-step explanation:

What would be the mass of 1.20 x 1024 molecules of water? Where —number of the moles, —Avogadro number, 6.02 * 1023 mol-1, —molar mass of water, 18 g/mol. = 1.2 ∗ 1024 6.02 ∗ 1023 ∗ 18 = 35.9