For vaporization of water at 1 atmospheric pressure the values of `DeltaH` and `DeltaS` are `40.63KJmol^(-1)` and `108JK^(-1)mol^(-1)` , respectively. The temperature when Gibbs energy change `(DeltaG)` for this transformation will be zero is

For vaporization of water at 1 atmospheric pressure, the values of DeltaH and DeltaS are 40.63 "kJ mol"^(-1) and 108.8 "JK"^(-1) mol^(-1) respectively. The temperature when Gibbs energy change (DeltaG) for this transformation will be zero , is :

For vaporization of water at 1 atmospheric pressure the values of Delta H and Delta S are 50.63 kJ mol^9-1) and 118.8 JK ^(-1) mol^(-1) respectively. The temperature when Gibbs energy change (Delta G) for this transformation will be zero, is

For vaporization of water at 1 atmospheric pressure the values of Delta H and Delta S are 50.63 kJ mol^-1 and 118.8 JK ^(-1) mol^(-1) respectively. The temperature when Gibbs energy change (Delta G) for this transformation will be zero, is

For a certain reaction X rarr Y the value of DeltaH and DeltaS are 50.50KJ mol^(-1) and 100.03JK^(-1) respectively. The temperature at which DeltaG=0 is

The values of Delta H and Delta S in vaporisation of water at 1 atm pressure are 40.63 " kJ mol"^(-1) and 108.8 J. K^(-1). " mol"^(-1) respectively. At what temperature the free energy change of the reaction will be zero ? What will be the sign of Delta G below that temperature ?