The Ideal Gas Law Video Lessons

Concept: Boyle's Law

# Problem: Into a 5.00 L container at 18oC are placed 0.200 mol H2, 20.0 g CO2, and 14.00 g O2. Calculate the total pressure in the container and the partial pressure of each gas.

87% (21 ratings)
###### FREE Expert Solution

We’re being asked to calculate for the partial pressure of H2, CO2, and O2 in a 5.00-L container and the total pressure in the container.

We’re going to calculate the pressure of each gas first 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

Rearranging the ideal gas equation:

$\frac{\mathbf{P}\overline{)\mathbf{V}}}{\overline{)\mathbf{V}}}\mathbf{=}\frac{\mathbf{nRT}}{\mathbf{V}}\phantom{\rule{0ex}{0ex}}\overline{){\mathbf{P}}{\mathbf{=}}\frac{\mathbf{nRT}}{\mathbf{V}}}$

87% (21 ratings)
###### Problem Details

Into a 5.00 L container at 18oC are placed 0.200 mol H2, 20.0 g CO2, and 14.00 g O2. Calculate the total pressure in the container and the partial pressure of each gas.

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.

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Our expert Chemistry tutor, Dasha took 8 minutes and 23 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Henricks' class at KSU.