We’re given equal moles of H2, N2, O2, and He in separate 1-L containers at the same temperature. We’re being asked which container has the highest pressure, assuming each gas behaves ideally.
Recall that the ideal gas law is:
Samples containing equal numbers of moles of H 2, N2, O2, and He are placed into separate 1 L containers at the same temperature. Assuming each gas behaves ideally, which container has the highest pressure?
e. All the gases would all exhibit the same pressure.
Frequently Asked Questions
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 Kinetic Molecular Theory concept. You can view video lessons to learn Kinetic Molecular Theory. Or if you need more Kinetic Molecular Theory practice, you can also practice Kinetic Molecular Theory practice problems.
What is the difficulty of this problem?
Our tutors rated the difficulty ofSamples containing equal numbers of moles of H 2, N2, O2, an...as medium difficulty.
How long does this problem take to solve?
Our expert Chemistry tutor, Dasha took 2 minutes and 13 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 Czernuszewicz's class at UH.