Question

Use the molar volume of a gas at STP to determine the volume (in L) occupied by 23.2 g of argon at STP. Express the volume in liters to three significant figures.

a) Ideal gas law
b) Boyle's law
c) Charles's law
d) Avogadro's law

Answer 1

To find the volume occupied by 23.2 g of argon at STP, we convert the mass to moles using the molar mass of argon and then multiply the number of moles by the molar volume of 22.4 L/mol. The result is approximately 13.0 L.

Step-by-step explanation:

To determine the volume occupied by 23.2 g of argon at standard temperature and pressure (STP), we can utilize the property of molar volume. The molar volume of any gas at STP is 22.4 liters per mole (L/mol). First, we need to convert the mass of argon to moles using the molar mass of argon, which is approximately 39.95 g/mol.

The calculation is as follows:

• Number of moles = mass (g) / molar mass (g/mol) = 23.2 g / 39.95 g/mol
• Number of moles of argon ≈ 0.5807 mol

Next, using Avogadro's law, we can calculate the volume occupied by argon at STP by multiplying the number of moles by the molar volume:

• Volume (L) = number of moles * molar volume (L/mol)
• Volume of argon ≈ 0.5807 mol * 22.4 L/mol
• Volume of argon ≈ 13.009 L

Therefore, 23.2 g of argon occupies approximately 13.0 liters at STP.