For a reaction `DeltaG^@`= -51.4 KJ/mol and `Delta H^@`= 49.4 KJ/mol at 300K, then value of `DeltaS^@` in J/K is

For a reaction DeltaH = -158.73KJ//mol, DeltaS= -58.1J//K , T= 298K then value of DeltaG (in KJ) is

For a reaction, DeltaH = 9.08 kJ mol^-1 and DeltaS =35.7 J K^-1 mol^-1 at 298 K. Which of the following is CORRECT for the reaction at 298 K?

In a chemical reaction DeltaH is 150 kJ and DeltaS is 100 J K^(-1) at 300 K then DeltaG is :-

In a chemical reaction, Delta H = 150 kJ and Delta S = 100 JK^(-1) at 300 K. Therefore, Delta G will be

For the reaction 2NO_2 (g) hArr N_2O_4(g) , when DeltaS = - 176.0 J K^(-1)mol^(-1) and DeltaH = - 57. 8 kJ mol^(-1) , the magnitude of Delta G at 298 K for the reaction is __________ kJ mol^(-1) . (Nearest integer)

For a given reaction, Delta H = 35.5 kJ mol^(-1) and Delta S = 83.6 JK^(-1) mol(-1) . The reaction is spontaneous at : (Assume that Delta H and Delta S do not vary with temperature)