PLQ 16: Free Energy Calculations 19-5

Which one of the following statements is always true about the equilibrium constant for a reaction if the standard free energy change for the reaction is negative? K = 0 K > 1 K < 1 K = 1 K < 0

K > 1

True or False. If ΔG° is negative, then products are favored at equilibrium.

True

True or False. Even if a system starts out with all reactants and products in their standard states, as soon as the reaction begins, standard state conditions no longer exist.

True

For the following reaction, Kp = 0.113 at 25°C, and the standard free energy change is 5.4 kJ/mol. If Todd does an experiment where the initial pressures are PN2O4 = 0.453 atm and PNO2 = 0.122 atm, what are the correct units of the free energy change of the reaction? N2O4(g) → 2 NO2(g) J/K J atm/K-mol kJ/mol J/K-mol

kJ/mol

ow is the standard free energy change related to the equilibrium constant? ΔG° = ΔG + RT ln K ΔG = K −TΔS ΔG° = −RT ln K ΔG = qrev/T + ln K ΔG = rate f/rate r + RT ln K

ΔG° = −RT ln K