Question

Find the number of atoms of argon in 12.0 L of argon at STP

Answer 1

To calculate the number of atoms of argon in 12.0 L of argon gas at STP, we find the number of moles in that volume and use Avogadro's number to convert moles to atoms, resulting in approximately 3.23 x 10^23 atoms.

Step-by-step explanation:

To find the number of atoms of argon in 12.0 L of argon gas at standard temperature and pressure (STP), we first determine the number of moles of argon, and then use Avogadro's number to find the total atoms. At STP, which is 0°C and 1 atm, one mole of any gas occupies 22.4 L. Therefore,

• Number of moles of argon = Volume at STP / Molar volume = 12.0 L / 22.4 L/mol
• Number of moles of argon = 0.536 moles (approximately)
• Since one mole of any substance contains approximately 6.022 x 10^23 atoms (Avogadro's number), the number of argon atoms = 0.536 moles x 6.022 x 10^23 atoms/mole.
• Total number of argon atoms in 12.0 L at STP = 3.23 x 10^23 atoms (approximately).

Thus, there are approximately 3.23 x 10^23 atoms of argon in 12.0 L of argon gas at STP.

Answer 2

3.25x10^23mol

Step-by-step explanation:

1 mole of argon = 22.4dm^3

X mole of argon = 12.0L

X 22.4 = 12.0

X = 12.0/22.4

X = 0.54mol

1 mol of argon contains 6.02x10^23 atom

Therefore 0.54 mole will contain X

Therefore X = 6.02x10^23 x 0.54

= 3.25x10^23mol