If `Delta G^(@)gt 0` for a reaction then :

DeltaH gt DeltaE for the reaction

If Delta G for a reaction is negative , the change is

Delta G^(0) and Delta H^(0) for a reaction at 300K is -66.9kJmol^(-1) and -41.8kJmol^(-1) respectively. Delta S^(0) for the same reaction at 300K is

For the reaction, 2A (s) + 2B (g)to C (g) + D(s) at 298K Delta U ^(@) =-10.5KJ and Delta S ^(@)=-44.10 JK^(-1) Calculate Delta G ^(@) for the reaction (in Joules).

For the reaction, 2A (s) + 2B (g)to C (g) + D(s) at 298K Delta U ^(@) =-10.5KJ and Delta S ^(@)=-44.10 JK^(-1) Calculate Delta G ^(@) for the reaction (in Joules).

Delta G^(@) of reversible reaction at its equilbrium is