38 terms

# ENGG 201, Midterm

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Terms in PVm = RT
P - Pressure
Vm - Molar Volume (v/n)
R - Universal Gas Constant (8.314 J/molK)
T - Temperature
Dalton's Law
Total pressure in a vessel equals sum of pressures that the gases exert in other vessels.
Amagat's Law
At constant T and P total volume of a gas is equal to volume of each component of the gas.
All gasses act ideal...
At very low P, very high T
Partial Pressure of each component of a gas
Pi = YiP, where Yi is mol fraction of that gas
Average Molar Mass of Gas
Sum of YiMi, where Yi is mol fraction of component and Mi is molar mass of component
Balance Equation
Accumulation = Input + Generation - Output (Input = Output when CV, no chemical reaction)
Diameter of a Molecule (1Å)
10 x 10⁻¹⁰m
Ek = m/2 c²
m - mass
c² - x+y+z velocity squared
√(c²) = √(3RT/M)
Root Mean Square Velocity (average velocity of gas particles)
R - Universal Gas Constant
T - Temperature
M - Molar Mass
Boltzmann Constant
k = R/Na = 1.3805x10⁻²³ J/K
Cmp < C < √(C²)
Always check: Most probably velocity < Mean Velocity < Root Mean Square Velocity
c = √(8RT/∏M)
Mean Velocity (speed)
R - Universal Gas Constant
M - Molar Mass
Cmp = root(2RT/M)
Most probable velocity (speed)
Cv = (∂Q/∂T)v = (3/2) R
Constant Volume Heat Capacity
Cp = (∂Q/∂T)p = (5/2)R
Constant Pressure Heat Capacity
Cp Cv relationship for ideal gases
Cp = Cv + R
Cp/Cv = 1.667
λ = (kT) / (∏σ²P√2)
Mean Free Path (λ) - Average distance molecule travels between two successive collisions

σ - collision diameter
k - Boltzmann Constant (1.3805x10⁻²³ J/K or (kg.m²/s²)/K
σ
Collision Diameter - Distance between centers of two colliding molecules at which point repulsive forces become large enough to reverse motion.
λ = μ/P √(∏RT/2M)
Mean Free Path (λ) - Average distance molecule travels between two successive collisions

μ - Viscosity
μ = (M/Na ∏σ²) √(RT/∏M)
Viscosity

Na - Avogadro's Number (6.022x10²³ mol⁻¹)
Na

6.022x10²³ mol⁻¹
μ
Viscosity
λ
Mean Free Path (λ) - Average distance molecule travels between two successive collisions
ρn
Number Density - Molecules/unit volume

ρn = Na/Vm

ρn = P/(KT)
λ = 1 / (∏σ²√2)(ρn)
Mean Free Path (λ) - Average distance molecule travels between two successive collisions

ρn - Number Density
σ - Collision Diameter
PVm = Na k T
Ideal gas equation for a mole of ideal gas
∂ = (kT/P)¹/³
Mean distance between molecules

∂³ = volume occupied by a molecule
∂ = (1/ρn)¹/³
Mean distance between molecules

∂³ = volume occupied by a molecule
(ρn c)/4
Collisions/unit area
Flux
Amount of molecules/unit area/unit time

molecules/m² s
Viscosity
μ - The resistance to deformation or resistance to flow exhibited by a fluid.

Measure of transfer of momentum of a substance.

μ is a constant coefficient of viscosity for a substance.

Viscosity is ONLY a function of T, not P!
Thermal Conductivity
Correlate the transport of heat energy of a substance
Diffusivity
Correlate the transport of mass within a substance
κ = μ(Cv/M)
Thermal conductivity

κ - Proportionality constant for thermal conductivity
Cv - Molar heat capacity
μ - Viscosity
Dab = [(RT)/(P Na ∏ σ²)]√(RT/∏M)
Molecular Diffusion - Diffusivity

Net transport of a substance from one region to another within a single phase, in absence of bulk movement or agitation.

Dab - Diffusion Coefficient
σ - Collision Diameter
Number Density
ρn = (P Na)/(RT)

Na implied at 1 molecule if not stated
Mass of molecule
M/Na

M - molar mass