20.3 Kinetic Theory of Gas

Question 1

What is the ROOT MEAN SQUARE SPEED?

Answer 1

all particles in an ideal gas have a spectrum of varying speeds, however after collisions the speed changes however the distribution of speed does not

the root mean squared is a way to calculate the mean speed of the particles

if temperature is raised then so is the root mean square speed

Question 2

ROOT MEAN SQUARE SPEED Equation

Answer 2

Crms = (C1^2 + C2^2 + …….. + CN^2 / N)^0.5

C1, C2, C3, etc and CN all represent the different speeds of the particles while N represents the number of molecules in the gas

Question 3

What are the ASSUMPTIONS made about gases for KINETIC THEORY to apply?

Answer 3

• the volume of the particles is negligible to the volume of the gas
• they do not attract each other
• they move randomly and continually
• their collisions are elastic
• time of collisions with container is shorter than time between collisions

Question 4

What is the KINETIC THEORY EQUATION?

Answer 4

pV = 1/3Nm(Crms)^2

PressureVolume = 1/3Number of * Mass of * Root Mean
Particles Gas Squared
Speed

Question 5

MEAN KINETIC ENERGY OF A MOLECULE OF A GAS

Answer 5

total Ek of all particles / total number of particles

0. 5mCrms^2
1. 5Mass of GasRoot Mean Squared Speed^2

Question 6

MEAN KINETIC ENERGY OF A MOLECULE IN AN IDEAL GAS

Answer 6

2/3kT

2/3Boltzman ConstantTemperature (K)

Question 7

INTERNAL ENERGY Equation

Answer 7

3/2nR*T

3/2number of molesMolar Gas Constant*Temperature
(K)
This is also the equation for total Ek of all moles in ideal gas