The Ideal Gas Law Video Lessons

Concept: Boyle's Law

# Problem: When 0.550 g of neon is added to a 750-cm3 bulb containing a sample of argon, the total pressure of the gases is found to be 1.46 atm at a temperature of 320 K.Find the mass of the argon in the bulb.

###### FREE Expert Solution

We’re being asked to calculate the mass of argon in a 750 cm3 container at 320 K.

The container consists of a gas mixture of argon (Ar), and neon (Ne).

We’re going to calculate the mass of carbon dioxide in grams using the following steps:

Step 1. Calculate the total number of moles of gas present in the container using the ideal gas equation.

$\overline{){\mathbf{PV}}{\mathbf{=}}{\mathbf{nRT}}}$

P = pressure, atm
V = volume, L
n = moles, mol
R = gas constant = 0.08206 (L·atm)/(mol·K)
T = temperature, K

Step 2. Calculate the number of moles of argon.
Step 3. Calculate the mass of argon.

###### Problem Details

When 0.550 g of neon is added to a 750-cm3 bulb containing a sample of argon, the total pressure of the gases is found to be 1.46 atm at a temperature of 320 K.

Find the mass of the argon in the bulb.