Show that in a process at constant temperature and pressure, the Gibbs free energy change of a system, `DeltaG=-TDeltaS_("total")`.

Define Gibb’s free energy.

What is Gibb’s free energy?

State the condition of spontaneity and equilibrium in terms of Gibbs free energy change of a system.

Change in Gibb’s free energy is given by

Why is Gibbs free energy called 'free energy' ?

DeltaG of the system alone provides a criterion for the spontaneity of a process at constant temperature & pressure, DeltaG system lt 0 (spontaneous) DeltaG system = 0 (equilibrium) DeltaG system gt 0 {(non-spontaneous) Again DeltaG^@ is related to the equilibrium constant as follows : DeltaG^@ = 2.303 RT log K_e If both DeltaH and Delta S are negative, the reaction will be spontaneous

Change in internal energy of a system is

For a chemical reaction occurring at constant temperature and pressure show that DeltaG=-TDeltaS_("univ") , where DeltaG= change in free energy of the system and DeltaS_("univ") =change in entropy of the universe. Using this equation explain when a reaction at a constant temperature and pressure will be (i) spontaneous (ii) non-spontaneous (iii) at equilibrium.

For a process at a particular temperature and pressure, DeltaG=DeltaH-TDeltaS . It can be written as: -DeltaG=T[-(DeltaH)/(T)+DeltaS] . What does the quantity within the bracket indicate?