ideal gas Flashcards
define ideal gas
a gas which obeys the equation Pv=nRT at all temperature, volume and pressure
state the ideal gas equation
P v = n R T
p=pressure, pascal
v=volume, m^3
n= mole
R=gas constant
T=temperature, K
what is another way of representing the ideal gas equation apart from Pv=nRT
P v = N k T
P=pressure, pascal
v=volume, m^3
N=total number of molecules
k=Boltzmann constant
T=temperature, K
equation for Boltzmann constant, k
k = R/NA
R=gas constant
NA=Avagadro’s constant
what the relationship between pressure, volume and temperature
P V ∝ T
P1 * V1 / T1 = P2 * V2 / T2
state the assumption of the kinetic theory of gas (all gases)
- there is no attractive or repulsive forces btw particle
- the particles are in constant random motion
- the particles undergo perfect elastic collision
- the volume of molecules is negligible compare to the volume around them
- There are a very large number of molecules that are identical
- duration of collision is negligible
why is there pressure
gas collide and rebound from container due to movement => change of momentum => force was exerted => provided pressure on the wall of container (P = F/A)
equation for root mean square speed, C r.m.s
C = √(<C^2>)
where <C^2> is average speed squared, unit m^2/s^2
why is there C r.m.s
in 3D space, velocity can be negative or positive => squared to get magnitude => average => squared root to get average speed
what is gas equation in respect to <c^2>
P v = 1/3 * N * m * <c^2>
m=mass of one particle
N=total number of particles
what equation of pressure interms of <c^2>
p = 1/3 *ρ * <c^2>
define translation kinetic energy
the kinetic energy of molecule as determined by their temperature
what is the equation for the average translational kinetic energy of one molecule of an ideal gas:
Ek = 1/2 * m * <c^2> = 3/2 k *T
what is the relation btw Cr.m.s and tempeature
C r.m.s ∝ √(T) directly proportional to square root of T
define mole
amount of substance containing same number of particles as 12 g of carbon 12 atoms
