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

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

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

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 rection, 2A (g) + B (g) rarr 2D(g) DeltaU_288^0 = - 10.5 kJ and DeltaS^0 = - 44.1 J . Calculation for DeltaG^0 for the reaction and predict whether the reaction is spontaneous or not.

The values of DeltaH and Delta S of a certain reaction are -400 kJ mol^-1 and -20 kJ mol^-1 K^-1 respectively. The temperature below which the reaction is spontaneous is _________.

If for a reaction, DeltaH is negative and DeltaS is positive then the reaction 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?

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