a pure sample of silver has 2.79 X10^23 atoms of silver. What mass of silver is present in this sample

Answer 1

Here we are using the concept that 1 mole of any substance = 6.022 x10²³ particles (Avogadro #). Remember this statement can be applied to atoms, molecules, ions if needed.

Since here we are talking about silver atoms,

1 mole of Ag = 107.9 g of silver =6.022 x10²³ silver atoms^.

2.79 x10²³ Ag atoms (107.9 g Ag/6.022 x10²³) = 50.0 g

Hope this helps!

Answer 2

To calculate the mass of silver present in the given sample, we need to use Avogadro's number and the molar mass of silver.

Avogadro's number (NA) is approximately 6.022 × 10^23, which represents the number of atoms or molecules in one mole of a substance.

The molar mass of silver (Ag) is 107.87 g/mol.

First, let's determine the number of moles of silver in the sample by dividing the given number of atoms by Avogadro's number:

Number of moles of silver = (2.79 × 10^23 atoms) / (6.022 × 10^23 atoms/mol)

Number of moles of silver ≈ 0.463 moles

Next, we can calculate the mass of silver by multiplying the number of moles by the molar mass:

Mass of silver = (0.463 moles) × (107.87 g/mol)

Mass of silver ≈ 49.96 grams

Therefore, the mass of silver present in the given sample is approximately 49.96 grams.