Question

A mixture of 0.200 g of H₂, 1.00 g of N₂, and 0.820 g of Ar is stored in a closed container at STP. Find the volume of the container, assuming that the gases exhibit ideal behavior.

a) 5.22 L
b) 6.47 L
c) 7.89 L
d) 9.13 L

Answer 1

To find the volume of the gas mixture at STP, calculate the number of moles of each gas using their molar masses, sum up the total moles, and then multiply by the molar volume of a gas at STP, which is 22.4 L/mol.

Step-by-step explanation:

The question involves calculating the volume of a gas mixture containing hydrogen (H₂), nitrogen (N₂), and argon (Ar) at standard temperature and pressure (STP), which is assuming ideal gas behavior.

To find the total volume, you would first determine the number of moles of each gas using their respective molar masses (H₂ = 2.02 g/mol, N₂ = 28.0 g/mol, Ar = 39.95 g/mol), then apply the ideal gas law where the volume of 1 mole of any gas at STP is 22.4 liters. The calculation would look something like this:

Moles of H₂ = 0.200 g / 2.02 g/mol, Moles of N₂ = 1.00 g / 28.0 g/mol, Moles of Ar = 0.820 g / 39.95 g/mol

Add the moles of each gas to get the total moles in the container. Then multiply the total moles by 22.4 L/mol to find the volume of the container. By performing these calculations, you can determine which of the multiple-choice options (a-d) is correct.