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?

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

How DeltaG is related to DeltaH and DeltaS ? What is the meaning of DeltaG = 0 ?

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

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.

At a particular temperature and pressure, when will the changes in entropy of the system (DeltaS_(sys)) and the surroundings (DeltaS_("surr")) be equal but the opposite in sign in a chemical reaction? In this condition, what will the value of DeltaG be? Will the reaction be spontaneous in this condition?

Which condition does not satisfy the spontaneity criteria ofa reaction at constant temperature and pressure (1) Delta H lt 0, DeltaS lt 0 , (2) Delta Hgt0,DeltaS lt 0 (3) DeltaH gt 0,DeltaS gt0 , (4) DeltaH lt0,DeltaS gt0 ?

At a certain temperature and pressure, ammonia gas is spontaneously adsorbed on the surface of finely divided charcoal. Predict the sign (+//-) of DeltaG, DeltaH and DeltaS in the process.

Which one of the following relation or expression is true for a spontaneous process of DeltaG=0,DeltaH=TDeltaS,DeltaG gt0,DeltaGlt0 ?

At a given temperature and pressure, for a chemical reaction DeltaH lt 0 & DeltaS lt 0 . Is the spontaneously of this reaction dependent upon temperature? If it depends and if the reaction reaches equilibrium at a temperature of T_(e), then will the reaction be spontaneous below or above T_(e) ?