Gibbs-Helmoholtz equation relates the free energy change to the enthalpy and entropy changes of the process as
`(DeltaG)_(PT) = DeltaH - T DeltaS`
The magnitude of `DeltaH` does not change much with the change in temperature but the enrgy factor `T DeltaS` changes appreciably. Thus, spontaneity of a process depends very much on temperature.
For the reaction at `298K, 2A +B rarr C`
`DeltaH = 100 kcal` and `DeltaS = 0.020 kcal K^(-1)`. If `DeltaH` and `DeltaS` are assumed to be constant over the temperature range, at what temperature will the reaction become spontaneous?

Options

A. total pressure increased to 1.3 atm
B. total pressure increased by 0.3 atm
C. difference in mercury level is 228 mm
D. Total pressure increased by 0.3 cm of Hg

Answer

A, B, C