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 equilibrium,
2H₂O $$\rightleftharpoons$$ H₃O⁺ + OH^$$-$$, the value of $$\Delta $$G^o at 298 K is approximately :

The reaction, MgO(s) + C(s) $$ \to $$ Mg(s) + CO(g), for which $$\Delta $$_rH^o + 491.1 kJ mol^–1 and $$\Delta $$_rS^o = 198.0 JK^–1 mol^–1, is not feasible at 298 K. Temperature above which reaciton will be feasible is :

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 :