Kinetic Molecular Theory
Presentation
•
Chemistry
•
11th Grade
•
Practice Problem
•
Medium
+2
Standards-aligned
Daaiyah White
Used 31+ times
FREE Resource
2 Slides • 6 Questions
1
Kinetic Molecular Theory Review
Gases consist of tiny particles (atoms or molecules)
The particles are in constant random motion, colliding with the walls of the container. These collisions are elastic because no energy is lost as particles collide.
The average kinetic energy of the gas particles is directly proportional to the Kelvin temperature of the gas. If temperature increase the kinetic energy will increase (more faster). If temperature decreases the kinetic energy will decrease (move slower).
2
The kinetic molecular theory also describes how gases move.
Compression: gases can be compressed (reduce volume)
Expansion: when volume is increase gases spread and expand
Diffusion: the random motion of gases cause a mixture of particles through one another
Effusion: gas will find opportunity to move in effusion gas escapes through a tiny opening.
Gas Behaviors
3
Multiple Choice
According to the kinetic-molecular theory, particles of matter
are in constant motion.
have different colors.
have different shapes.
are always liquid
4
Multiple Choice
The kinetic-molecular theory explains the behavior of
gases only
liquids and gases
solids and liquids
solids, liquids, and gases
5
Multiple Choice
Two moving steel balls collide and their total energy after the collision is the same as before. This is an example of
effusion
an elastic collision
expansion
compression
6
Multiple Choice
Which is an example of gas diffusion?
inflating a flat tire
a tea bag being placed into hot water
the odor of perfume spreading throughout a room
all of the above
7
Multiple Choice
Kinetic energy is direction proportional to temperature. If temperature increases the kinetic energy of a substance will...
increase
decrease
remain the same
none of these
8
Multiple Choice
Which is an example of effusion?
oxygen and gasoline fumes mixing in an automobile carburetor
helium dispersing into a room after a balloon pops
he aroma of a cooling pie spreading across a room
air slowly escaping from a pinhole in a tire
Kinetic Molecular Theory Review
Gases consist of tiny particles (atoms or molecules)
The particles are in constant random motion, colliding with the walls of the container. These collisions are elastic because no energy is lost as particles collide.
The average kinetic energy of the gas particles is directly proportional to the Kelvin temperature of the gas. If temperature increase the kinetic energy will increase (more faster). If temperature decreases the kinetic energy will decrease (move slower).
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