# How would you find the mass in grams of the following

4.01*10^23 atoms Ca, 40.08 g/mol

## To find the mass in grams of 4.01 * 10^23 atoms of Ca, you need to use the molar mass of Ca and Avogadro's number.

Step 1: Find the molar mass of Ca (calcium)

The molar mass of Ca is given as 40.08 g/mol.

Step 2: Convert the number of atoms to moles

To convert from atoms to moles, divide the number of atoms by Avogadro's number (6.022 * 10^23 mol^-1):

Number of moles = (4.01 * 10^23 atoms) / (6.022 * 10^23 atoms/mol)

≈ 0.666 mol (approximately)

Step 3: Calculate the mass in grams

To calculate the mass in grams, multiply the number of moles by the molar mass:

Mass = (0.666 mol) * (40.08 g/mol)

≈ 26.72 g (approximately)

Therefore, the mass in grams of 4.01 * 10^23 atoms of Ca is approximately 26.72 g.

## To find the mass in grams of a given number of atoms, you can use the concept of molar mass. Molar mass is the mass of one mole of a substance, which is expressed in grams.

First, you need to determine the molar mass of calcium (Ca), which is given as 40.08 g/mol. This value represents the mass of one mole of calcium atoms.

Next, convert the given number of atoms (4.01 x 10^23) to moles. Since there are Avogadro's number of particles (atoms, molecules, etc.) in one mole, you can divide the number of atoms by Avogadro's number (6.022 x 10^23).

(4.01 x 10^23 atoms Ca) / (6.022 x 10^23 atoms/mol) = 0.666 mol Ca

Now that you have the number of moles of calcium, you can calculate the mass in grams by multiplying the number of moles by the molar mass of calcium.

0.666 mol Ca x 40.08 g/mol = 26.7 g

Therefore, the mass in grams of 4.01 x 10^23 atoms of calcium is approximately 26.7 grams.