Modelling a gas Flashcards
Mole
A quantity of substance with the same number of particles as 12 grams of carbon -12.
Avogadro’s constant
6.02 x 1023
Formula for no. of particles
n = N / NA
no. of moles= No. of particles/Avogadro’s no.
Formula for mass, molecular mass and moles
n = m/μ
no. of moles = mass/ molecular mass
Pressure definition
Force acting perpendicularly per unit area
Pressure in solids when force is at an angle
P = F cos θ /A
Pressure in liquids
P = heg
Pressure = height x density x gravity
Properties of an ideal gas
- Molecules are point particles, each with negligible volume
- Molecules obey the laws of mechanics
- No forces between molecules except during collisions
- Duration of collisions is negligible compared to time between collisions
- Collisions between molecules and with the walls of the container are perfectly elastic
- Molecules move randomly with a range of speeds
- Do not change state
Properties of a real gas that prevent them from being ideal gases
- Forces between molecules
- Molecules have definite volume
- They condense before zero
- Condense at high pressure and low temperature
Pressure-volume (Boyle’s) law
For a gas with contsant temperature and mass, pressure is inversely proportional to volume
Pressure-volume law equation
p=k/V
p1 V1 = p2 V2
Volume-temperature (Charle’s) law
The volume of a fixed mass of gas at constant pressure is directly proportional to its absolute temperature
Volume-temperaure law equation
V = kT
V1 / T1 = V2 / T2
What is absolute zero?
0 Kelvin. When particles are not moving
Pressure- temperature (Gay-Lussac’s) law
Pressure of a fixed mass of gas, at constant volume, is direcly proportional to absolute temperature
Pressure-temperature law equation
P = kT
p1 / T1 = p2 / T2
Isobar
Line joining points at the same pressure
Isothermal
Line joining points at the same temperature
Combined gas law
p1 V1 / T1 = p2 V2 / T2
Equation of state of an ideal gas
pV = nRT
p = pressure (pa)
V= volume (m3)
n = no. of moles
R = 8.31
T = Temperature (K)
Value of R (universal gas constant)
R = 8.31 J/Kmol
Kinetic energy of 1 molecule of gas (2 equations)
EK = 1/2 mc2
EK = 3/2 KB T
c = root mean square speed (r.m.s)
c2 = mean square speed
KB = R/NA (Boltzmann’s constant)
Pressure of a gas
p = 1/3 ec2
e = density (kg/m3)
Internal energy(U)
U = 3/2 nRT