Question

The molar mass of sulfur S is 32.06 g/mol

Calculate the mass in grams of a sample of S containing 2.01x10^24 atoms
Help Please<3

Answer 1

To calculate the mass of sulfur with 2.01x10^24 atoms, convert the number of atoms to moles using Avogadro's number and then multiply the moles by the molar mass of sulfur. The result is approximately 107.00 grams.

Step-by-step explanation:

The mass in grams of a sample of sulfur (S) containing 2.01x1024 atoms can be calculated using Avogadro's number and the molar mass of sulfur.

First, we need to find out how many moles of sulfur atoms are there in 2.01x1024 atoms. Avogadro's number (6.022x1023 atoms/mol) tells us how many atoms are in one mole of any substance.

To find the number of moles, we divide the number of sulfur atoms by Avogadro's number:

Number of moles = 2.01x1024 atoms / 6.022x1023 atoms/mol

This gives us approximately 3.34 moles of sulfur.

To convert moles to grams, we multiply by the molar mass of sulfur:

Mass in grams = 3.34 moles * 32.06 g/mol

This results in approximately 107.00 grams of sulfur.

Answer 2

Answer: 107.01 g

Step-by-step explanation:

Since we are starting from the number of atoms of Sulfur, we need to know two sets of formulas:

• mass = moles × molar mass
• moles = atoms ÷ Avogadro's Number

⇒ mass = (atoms ÷ Avogadro's Number) × molar mass

mass = [(2.01 × 10²⁴ atoms) ÷ (6.022 × 10²³ atoms/mole)] × (32.06 g/mol)

= 107.01 g

the mass of a sample of S containing 2.01×10²⁴ atoms is 107.01 g.