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.

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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.

PV=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.

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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.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Ideal Gas Law concept. You can view video lessons to learn The Ideal Gas Law. Or if you need more The Ideal Gas Law practice, you can also practice The Ideal Gas Law practice problems.