We’re being asked to calculate the mass of carbon dioxide in a 10.0 L container at 25°C.
The container consists of a mixture of oxygen gas (O2), nitrogen gas, and carbon dioxide (CO2).
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.
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 carbon dioxide.
Step 3. Calculate the mass of carbon dioxide.
A mixture of oxygen gas, nitrogen gas, and carbon dioxide in a 10.0 L container at 25°C has a total pressure of 12.5 atm. If there are 30.0 g each of oxygen and nitrogen, how many grams of carbon dioxide are present?
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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.
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Based on our data, we think this problem is relevant for Professor Larsen's class at UH.