University:
San Jose State University
Course:
CHEM 1A | General Chemistry
Academic year:

2023
Views:

449

Pages:

1
Author:

Norbiemumhy

Thermodynamic Process Open System: Exchange of matter and energy with surroundings Closed System: Exchange of energy only with surroundings Isolated System: No exchange of matter or energy with surroundings Types of Processes Isothermal: ΔT = 0 Isochoric: ΔV = 0 Adiabatic: ΔQ = 0 Isobaric: ΔP = 0 Cyclic: ΔU = 0 First Law of Thermodynamics ΔU = Q + W (ΔU = internal energy, Q = heat, W = work done) Work Done W = -Pext(V2 - V1) Heat Capacity Q = CΔT Cp = Cm + R Q = CsmΔT (for molar heat capacity) Enthalpy ΔH = ΔU + nRΔT ΔHsol = ΔHlattice + ΔHhyd Gibbs Energy ΔG° = ΔH° - TΔS = -RT ln K Third Law of Thermodynamics Entropy of a pure crystalline substance at 0 K is zero.