Kinetic Theory Flashcards
What are the assumptions of kinetic theory?
1) The molecules move at random direction
2) There is a random distribution of energy among molecules
3) There is no attraction between molecules
4) The molecules occupy negligible volume compared to the volume of the container
5) The collisions between molecules are elastic therefore energy is conserved
6) The duration of collision is negligible compared to the duration between collisions
Define mole
The number of particles contained in 12g of carbon-12
Define Avogadro’s constant
The number of particles in 1 mole
What is an ideal gas?
A theoretical concept where under certain circumstances real gases will approximate to the behaviour of an ideal gas
What do ideal gases obey?
They obey the equation of state
What are the equations of state?
Boyles Law:
pV = constant
Charles Law:
V/t = constant
Pressure Law:
p/t = constant
How can the equation of state be summarised?
pV/t = constant
What is the constant’s value dependant on, in the equations of state?
The value of the constant was dependant on the mass
What is the constant for gases at low enough pressure and if 1 mole is considered?
Universal molar gas constant = R
What is the ideal gas equation?
pV = nRT
What equation is used when the number of particles is given?
pV = NkT
What is the equation for moles?
n = N/NA
What is the equation linking the universal molar gas constant and Boltzmann constant?
K = R/NA
Derive the pV = NkT equation
pV = nRT
n=N/NA
pV = NRT/NA
k=R/NA
pV = NkT
What is the total kinetic energy of a number of moles?
Ke = 3nRT/2
