This preview has intentionally blurred sections. Sign up to view the full version.
View Full Document
Unformatted text preview: Equations ax 2 + bx + c = 0 and x = b ± √ b 2 4 ac 2 a Quadratic Equation PV = nRT Ideal Gas Law P T = ∑ i P i Dalton’s law of partial pressures parenleftbigg P + an 2 V 2 parenrightbigg ( V nb ) = nRT van der Waals equation Z = 1 + B V m + C V 2 m + D V 3 m + ··· Virial Equation Z = 1 + B ′ P + C ′ P 2 + D ′ P 3 + ··· Virial Equation E trans = 3 2 RT N A = 3 2 k B T Average kinetic energy v rms = radicalbigg 3 k B T m = radicalbigg 3 RT M Rootmeansquare velocity dN N = 4 πc 2 parenleftBig m 2 πk B T parenrightBig 3 / 2 e − mc 2 / 2 k B T dc Maxwell speed distribution c = radicalbigg 8 k B T πm = radicalbigg 8 RT π M Average or mean speed c mp = radicalbigg 2 k B T πm = radicalbigg 2 RT π M most probable speed Z 1 = √ 2 πd 2 c N V Collision frequency Z 11 = √ 2 2 πd 2 c parenleftBig N V parenrightBig 2 Binary collision frequency λ = 1 √ 2 πd 2 ( N/V ) Mean free path η = m c 3 √ 2 πd 2 Gas viscosity r 1 r 2 = radicalbigg M 2 M 1 Graham’s laws of diffusion and effusion N 2 N 1 = e − Δ E/k B T Boltzmann distribution law w = integraldisplay pdV expansion work w = nRT ln V 2 V 1 = nRT ln P 1 P 2 work of isothermal, reversible ideal gas expansion Δ U = q + w First law of Thermodynamics dU = d ¯ q + d ¯ w First law of Thermodynamics H = U + PV Definition of Enthalpy C v = parenleftBig...
View
Full
Document
This note was uploaded on 07/17/2008 for the course CHEM 520 taught by Professor Grandinetti during the Spring '08 term at Ohio State.
 Spring '08
 GRANDINETTI
 Physical chemistry, Partial Pressure, pH

Click to edit the document details