Gibbs Helmholtz equation relates the enthalpy, entropy and free energy change of the process at constant pressure and temperature as
`DeltaG=DeltaH-TDeltaS ” (at constant P, T)”`
In General the magnitude of `DeltaH` does not change much with the change in temperature but the terms `TDeltaS` changes appreciably. Hence in some process spontaneity is very much dependent on temperature and such processes are generally known as entropy driven process.
When `CaCO_(3)` is heated to a high temperature it decomposes into CaO and `CO_(2)`, however it is quite stable at room temperature. It can be explained by the fact that
A. `Delta_(r )H` dominates the term `TDeltaS` at high temperature
B. the term `TDeltaS` dominates the `Delta_(r )H` at high temperature
C. at high temperature both `Delta_(r )S` and `Delta_(r )H` becomes negative
D. thermodynamics can not say anything about spontaneity

Gibbs Helmholtz equation relates the enthalpy, entropy and free energy change of the process at constant pressure and temperature as
`DeltaG=DeltaH-TDeltaS ” (at constant P, T)”`
In General the magnitude of `DeltaH` does not change much with the change in temperature but the terms `TDeltaS` changes appreciably. Hence in some process spontaneity is very much dependent on temperature and such processes are generally known as entropy driven process.
The Dissolution of `CaCl_(2).6H_(2)O` in a large volume of water is endothermic to the extent of 3.5 kcal `”mol”^(-1)` and `DeltaH` for the reaction is -23.2 kcal `”mol”^(-1)`.
`CaCl_(2)(s)+6H_(2)O(l)rarrCaCl_(2).6H_(2)O(s)`
Select the correct statement :
A. `DeltaH_(“solution”)` for anhydrous `CaCl_(2)` is – 19.7 kcal/mol and the process is enthalpy driven
B. `DeltaH_(“solution”)` for anhydrous `CaCl_(2)` is – 19.7 kcal/mol and the process is entropy driven
C. Dissolution of `CaCl_(2).6H_(2)O` in water is enthalpy driven process
D. The `Delta_(r )S` the reaction `CaCl_(2)(s)+6H_(2)O(l)rarrCaCl_(2).6H_(2)O(s)` is negative

Gibbs Helmholtz equation relates the enthalpy, entropy and free energy change of the process at constant pressure and temperature as
`DeltaG=DeltaH-TDeltaS ” (at constant P, T)”`
In General the magnitude of `DeltaH` does not change much with the change in temperature but the terms `TDeltaS` changes appreciably. Hence in some process spontaneity is very much dependent on temperature and such processes are generally known as entropy driven process.
Fro the reaction at 298 K, `A_(2)B_(4)rarr2AB_(2)`
`DeltaH=2″ kJ”` and `DeltaS` = 20 J/K at constant P and T, the reaction will be
A. spontaneous and entropy driven
B. spontaneous and enthalpy driven
C. non-spontaneous
D. at equilibrium