Question

Calculate the mass in gram of 2.01×10^10 atoms of Mg

Answer 1

The mass of 2.01×10^10 atoms of Mg is 8.12×10^-13 grams.

Step-by-step explanation:

To calculate the mass of 2.01×10^10 atoms of Mg, we need to convert the number of atoms to moles using Avogadro's number, and then convert moles to grams using the molar mass of Mg. Avogadro's number, 6.022×10^23, is the number of atoms in one mole of a substance. The molar mass of Mg is 24.31 g/mol.

First, we convert the number of atoms to moles:

2.01×10^10 atoms ÷ 6.022×10^23 atoms/mol = 3.34×10^-14 mol

Next, we convert moles to grams:

3.34×10^-14 mol × 24.31 g/mol = 8.12×10^-13 g

Therefore, the mass of 2.01×10^10 atoms of Mg is 8.12×10^-13 grams.

Answer 2

First we need to convert the given atoms of Mg to units of moles. To do this, we divide the given with the Avogadros number.

Moles of Mg = number of atoms / Avogadro’s number

Moles of Mg = 2.01 x 10^10 atoms / (6.022 x 10^23 atoms / mol)

Moles of Mg = 3.33776 x 10^-14 mol Mg

Then we convert moles to mass by multiplying with the Molar mass. Molar mass of Mg = 24.305 g / mol

Mass of Mg = Moles of Mg * Molar mass of Mg

Mass of Mg = 3.33776 x 10^-14 mol * 24.305 g / mol

Mass of Mg = 8.11 x 10^-13 g