The standard reaction Gibbs energy for a chemical reaction at an absolute temperature T is given by $$\Delta $$_rG^o = A – BT

Where A and B are non-zero constants. Which of the following is TRUE about this reaction?

For the chemical reaction X $$\rightleftharpoons$$ Y, the standard reaction Gibbs energy depends on temperature T (in K) as $$\Delta $$_rG^o (in kJ mol^–1) = 120 $$ - {3 \over 8}$$ T.

The major component of the reaction mixture at T is :

Two blocks of the same metal having same mass and at temperature T₁ and T₂, respectively, are brought in contact with each other and allowed to attain thermal equilibrium at constant pressure. The change in entropy, $$\Delta $$S, for this process is :

The process with negative entropy change is :