One of the challenges of using the second law of thermodynamics to determine if a process is spontaneous is that we must determine the entropy change for the system and the entropy change for the surroundings. Figure A31 Psychrometric chart at 1 atm total pressure Table A32 One-dimensional isentropic compressible-flow functions for an ideal gas with k 1.4 Table A33 One-dimensional normal-shock functions for an ideal gas with k 1.4 Table A34 Rayleigh flow functions for an ideal gas with k 1.
Relate standard free energy changes to equilibrium constants.Drag or click the locator to display the values of the temperature and pressure as well as the -value for various light hydrocarbons. Explain how temperature affects the spontaneity of some processes For light hydrocarbons, the approximate -values can be determined from DePriester charts, which have been fit to the following equation:, where the constants, ,, ,, and are tabulated 1.The DePriester charts SO check this quite well (see Figures 8. Calculate free energy change for a process using free energies of formation for its reactants and products.The hydrocarbon Kvalues are obtained from the charts of Procedure 8Al.l and corrected for the presence of hydrogen. Strong acids are listed at the top left hand corner of the table and have Ka values >1. Define Gibbs free energy, and describe its relation to spontaneity The hydrogen K-values are obtained from a chart on which the system temperature and pressure and the MABP of the hydrogen-free liquid are parameters.