If you calculate a value for DG8 for a reaction using the values of DG8f in Appendix 4
Chapter 17, Problem 17.25(choose chapter or problem)
If you calculate a value for DG8 for a reaction using the values of DG8f in Appendix 4 and get a negative number, is it correct to say that the reaction is always spontaneous? Why or why not? Free energy changes also depend on concentration. For gases, how is G related to the pressure of the gas? What are standard pressures for gases and standard concentrations for solutes? How do you calculate DG for a reaction at nonstandard conditions? The equation to determine DG at nonstandard conditions has Q in it: What is Q? A reaction is spontaneous as long as DG is negative; that is, reactions always proceed as long as the products have a lower free energy than the reactants. What is so special about equilibrium? Why dont reactions move away from equilibrium?
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