Multiple Choice
Which of the following best explains why the pressure of a fixed amount of gas decreases as altitude increases in Earth's atmosphere, assuming temperature remains constant?
30
views
7. Gases
The Ideal Gas Law Applications
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Under which conditions of temperature and pressure does oxygen gas behave least like an ideal gas?
A
Low temperature and low pressure
B
Low temperature and high pressure
C
High temperature and low pressure
D
High temperature and high pressure
Verified step by step guidance1
Recall that ideal gas behavior assumes negligible intermolecular forces and that gas particles occupy no volume. Deviations occur when these assumptions fail.
Understand that at low temperatures, gas particles have less kinetic energy, so intermolecular attractions become more significant, causing deviations from ideal behavior.
Recognize that at high pressures, gas particles are forced closer together, making the finite volume of particles and intermolecular forces more important, leading to non-ideal behavior.
Combine these insights: oxygen gas behaves least like an ideal gas under conditions where intermolecular forces and particle volume cannot be ignored, which is at low temperature and high pressure.
Therefore, the conditions of low temperature and high pressure cause oxygen gas to deviate most from ideal gas behavior.
4:09mWatch next
Master Ideal Gas Law Relationships with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
The Ideal Gas Law Applications practice set
Problem sets built by lead tutorsExpert video explanations