Which of the following assumptions of the kinetic molecular theory of gases is not valid for real gases at high pressure?
A) The volume of the gas particles is much smaller than the distance between the gas particles.
B) The gas particles behave like hard, spherical objects in a state of constant, random motion.
C) The average kinetic energy of the gas particles depends upon temperature of the gas only.
D) The gas particles move in a straight line until they collide with another particle or the walls of the container.
E) All of the above are valid for real gases at high pressure.
If all of the flasks of gas shown are the same size, at the same temperature, and contain the same number of molecules, in which flask will the molecules be moving slowest?
A Flask 1
B Flask 2
C Flask 3
D Flask 4
Each of these flasks contains the same number of molecules. In which container is the pressure lowest?
Each of these flasks is the same size and at the same temperature. In which flask will diffusion occur most slowly?
A flask 1
Each of these flasks is the same size and at the same temperature. Which one contains the fewest molecules?
Each of these flasks contains the same number of gas molecules. In which would the pressure be highest?
C Flask 4
D Flask 3
Four different flasks contain gas samples at 298 K. In which of the following samples will the gas molecules be moving the fastest?
A CO2
B H2
C N2
D O2
If all of the following flasks are the same size, at the same temperature, and contain the same number of molecules, in which flask will the pressure be highest?
E All have the same pressure
Which of the following changes to a system WILL NOT result in an increase in pressure?
A Raising the temperature
B Adding more gas molecules
C Increasing the volume of the container
D Decreasing the volume of the container
Gas pressure is caused by:
A intermolecular forces
B gas molecules colliding with surfaces
C gas molecules hitting other gas molecules
D gas molecules condensing to a liquid
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