A hydrogen molecule (diameter 1.0 * 10-8 cm), traveling at the rms speed, escapes from a 4000 K furnace into a chamber containing cold argon atoms (diameter 3.0 * 10-8 cm) at a density of 4.0 * 10^19 atoms/cm3. (a) What is the speed of the hydrogen molecule? (b) If it collides with an argon atom, what is the closest their centers can be, considering each as spherical? (c) What is the initial number of collisions per second experienced by the hydrogen molecule?
Kinetic Theory of Gas
The Kinetic Theory of gases is a classical model of gases, according to which gases are composed of molecules/particles that are in random motion. While undergoing this random motion, kinetic energy in molecules can assume random velocity across all directions. It also says that the constituent particles/molecules undergo elastic collision, which means that the total kinetic energy remains constant before and after the collision. The average kinetic energy of the particles also determines the pressure of the gas.
P-V Diagram
A P-V diagram is a very important tool of the branch of physics known as thermodynamics, which is used to analyze the working and hence the efficiency of thermodynamic engines. As the name suggests, it is used to measure the changes in pressure (P) and volume (V) corresponding to the thermodynamic system under study. The P-V diagram is used as an indicator diagram to control the given thermodynamic system.
A hydrogen molecule (diameter 1.0 * 10-8 cm), traveling at
the rms speed, escapes from a 4000 K furnace into a chamber containing
cold argon atoms (diameter 3.0 * 10-8 cm) at a density of
4.0 * 10^19 atoms/cm3. (a) What is the speed of the hydrogen molecule?
(b) If it collides with an argon atom, what is the closest their
centers can be, considering each as spherical? (c) What is the initial
number of collisions per second experienced by the hydrogen molecule?
Trending now
This is a popular solution!
Step by step
Solved in 4 steps with 1 images
