For KCl,`Delta_LH = 699 kJ//mol^-I` and `Delta_(hyd)H = -681.8 kJ//mol^-1`. What will be its enthalpy of solution?

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?

For vaporization of water at 1bar, DeltaH=40.63kJ mol^(-1) and DeltaS = 108.8 JK ^(-1) mol^(-1) At what temperature, DeltaG=0 ?

For a certain reaction DeltaH = - 25 kJ and DeltaS = - 40 JK^(-1) . At what temperature will it change from spontaneous to non-spontaneous reaction?

For a certain reaction, DeltaH^@ =- 224 kJ and DeltaS^@=- 153 JK^(-1) . At what temperature will it change from spontaneous to non-spontaneous?

For the reaction Ag_(2)O(s)rarr 2Ag(s)+1//2O_(2)(g) the value of Delta H=30.56 KJ mol^(_1) and Delta S = 66 JK^(-1)mol^(-1) . The temperature at which the free energy change for the reaction will be zero is :-

For a certain reaction, DeltaH^@ =- 219 kJ and DeltaS^@ = - 21 JK^(-1) Determine whether the reaction is spontaneous or nonspontaneous.