Chapter 7 - Gases, Liquids And Solids Flashcards
Kinetic Theory of Gases⚡️
Why is there no change in energy of the particles after collisions of particles?
Collisions between particles or with the walls of the container are perfectly elastic.
Kinetic Theory of Gases⚡️
Why do gases exert a pressure?
Gases consist of tiny particles moving in rapid, random, straight-line motion until they collide with one another or the walls of the container.
Kinetic Theory of Gases ⚡️
Gas particles have mass but no volume why?
A corollary of this is that the distance between the gas particles are very large compared to the size of the particles themselves.
Kinetic Theory of Gaeses⚡️
Attractive or Repulsive forces between gas particles are…..
Negligible
Kinetic Theory of Gaeses⚡️
As the temperature increases..
The average kinetic energy of the particles increase.
KE= 0.5 mv^2
The Physical Gas Laws
A hypothetical gas whose molecules occupy negligible space and have no interactions.
The Physical Gas Laws
Collisions between molecules are perfectly elastic.
The Physical Gas Laws
Zero
The Physical Gas Laws
Nope, there is no attractive forces on one another.
Is it possible for ideal gases to come in liquid or solid forms?
Nope, this is because a solid/liquid will need an attractive force to hold them together.
When does The Physical Gas Laws
When real gases are at approximately room temperature and pressure.
When do The Physical Gas Laws
When gases are at very low temperatures and high pressures, when they are near to liquefying or condensing, because intermolecular forces become significant.
What happens at high temperatures and low pressures?
Molecules have very little interaction with ones other at High temperatures as they move faster and at low pressures they are very far apart and have fewer collisions with the container and each other. This lack of intermolecular attractions make real gases behave like an ideal has.
FORMULA HEUEHUEHE
n=v/22.71
Pressure is the force on a unit area.
P=F/A
