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

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

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 _________.

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 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?

What is the effect of change of temperature on the rate of reaction?