Chapter 3.2 Flashcards
Avogadro’s constant
6.02*10^23
Equation for number of moles with N particles
n = N/NA
NA = Avogadro’s constant
Atomic mass unit (u)
1/12 of the mass of one atom of carbon-12
Molar mass
The sum of the atomic masses of the atoms making up the molecules
What is the number of particles in one mole of a substance and what is its mass?
Contains a number of particles that are equal to Avogadro’s constant and mass is equal to the molar mass of the substance
Pressure definition and equation
The normal force applied per unit area
p = F/A
Value of one atmosphere (atm) in Pascals
1.013*10^5 Pa
Ideal gas assumptions
The molecules are point particles with negligible volume
The molecules obey the laws of mechanics
There are no forced between the molecules except when they collide
The duration of collision is negligible compared to the time between collisions
The collisions of the molecules with each other and with the container walls are elastic
Molecules have a range of speeds and move randomly
When may a real gas be approximated by an ideal gas?
When the density is low
Why is there pressure on the walls from gas molecules?
When a molecule collides with a container wall there is a change of momentum which means a force was acted on it by the wall. Newton’s third law states that the wall should have felt an equal and opposite force
What does the equation of state link together?
Pressure, volume, temperature and number of moles
Boyle’s law
At constant temperature and with a fixed quantity of gas, pressure is inversely proportional to volume
Charles’ law
At constant pressure, volume is proportional to temperature
Gay-Lussac/Amontons’ law
At constant volume, pressure is proportional to temperature
Equation of state
pV = nRT
