Physical Chemistry: Thermodynamics and Heat Transfer - Prof. Marc Sher, Study notes of Physics

Download Physical Chemistry: Thermodynamics and Heat Transfer - Prof. Marc Sher and more Study notes Physics in PDF only on Docsity! TC = T(K) – 273.15 ΔL = α L0 ΔT ΔV = β V0 ΔT for a solid, β = 3α Atoms/mole = 6.02 x 1023 Mass of proton = 1.67 x 10-27 kg. = 1 u Mass of atom in u is equal to the grams/mole PV = NkT k = 1.38 x 10-23 J/K PV = nRT R = kNA = 8.31 J/(K-mol) = 0.082 Liter-atm/(K-mol) 1 Liter = 10-3 m3 1 atm. = 1.01 x 105 Pa Ktr = (3/2)kT = (1/2)m(v2)rms xrms = (2Dt)1/2 Arms = (Σ Ai2)1/2 1 cal = 4.186 J Q = m c ΔT (water: c = 1 cal/g-K = 4.186 kJ/kg-K) At constant volume: Q = n CV ΔT monatomic gas: CV = (3/2)R, diatomic: CV = (5/2)R Phase transitions: Q = mL (L(fusion of water) = 80 cal/g, L(vap. of water) = 540 cal/g) Conduction: Q/t = (κ A ΔT)/d Radiation: Q/t = eσAT4 σ = 5.7 x 10-8 W/m2K4 Thermodyamics: ΔU = n CV ΔT ΔU = Q + W W = -PΔV Process W Q ΔU Constant Volume (isochoric) 0 n CV ΔT n CV ΔT Constant Pressure (isobaric) -nRΔT n(Cv + R) ΔT n CV ΔT Constant Temperature (isothermal) -nRT ln(Vf/Vi) nRT ln(Vf/Vi) 0 Adiabatic (no heat transfer) W 0 W Wnet = QIN – QOUT efficiency: e = Wnet/QIN = 1 - QOUT/ QIN Reversible engine: e = 1 – TC/TH Coeff. of performance: K = QC/Wnet Entropy: ΔS = Q/T S = k lnΩ 1st Law: ΔU = Q + W 2nd Law: Entropy of a closed system increases with time 3rd Law: can’t reach absolute zero