STANDARD-STATES: TRUE OR FALSE? (1 +1 +1 +1 + 2 + 2 + 2 = 10 pts) 1. Consider the expression seen in class for the standard state of a real liquid solution as a function of molar concentration. The standard-state potential of the solution component i, denoted as ui, is the chemical potential of species i, denoted as ui, at pressure P = 1 bar and 1 molar (1 M) concentration of species i when the activity coefficient y = 1, at any given temperature. 2. The temperature of thermodynamic standard states is often 25 degrees C, but it may also be a different temperature. 3. The numerical value of thermodynamic standard states of ideal-gas and liquid solutions depends on the total pressure. 4. The numerical value of thermodynamic standard states of ideal-gas and liquid solutions depends on the concentration of the species in solution. 5. At 1 molar concentration of species i in a liquid solution and P = 1 bar, it is unlikely that the solution exhibits ideal behavior. Therefore, the standard state is a fictitious state that is nonetheless an important and useful reference state in thermodynamics. 6. For a chemical or biochemical process, the difference in standard-state chemical potentials between reactants and products (Au or AG in kcal/mol) can be determined from the equilibrium constant of the process, at constant total pressure P= 1 bar, at any given temperature. 7. For a chemical or biochemical process, the difference in standard-state enthalpies (AH in kcal mol!) and entropies between reactants and products (AS in kcal moll K-?) can be determined from the equilibrium constants of the process measured at different temperatures, at constant total pressure P= 1 bar