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