Establish `DeltaG = DeltaH- TDeltaS`.

(i) Spontaneity of a process can be determined from the entropy change and also from the Gibbs free energy change. But the Gibbs free energy change in more useful than entropy change to determine the spontaneity of a process. Explain it. (ii) Show that Gibbs energy change of a system at certain temperature and pressure, DeltaG=DeltaH-TDeltaS .

(i) What do you mean by heat of reaction at constannt volume and heat of reaction at constant pressure? (ii) Establish the relation DeltaH=DeltaU=DeltanRT for a chemical reaction in gaseous state.

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?

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

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

What will be the signs of the following thermodynamic quantities for the adsorption of a gas on a solid at constant temperature and pressure? DeltaG, DeltaS, DeltaH .

Give an example of a reaction for each of the following relations between DeltaH and DeltaU : (i) DeltaU lt DeltaH (ii) DeltaU gt DeltaH (iii) DeltaU=DeltaH .