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 thatA. `Delta_(r )H` dominates the term `TDeltaS` at high temperatureB. the term `TDeltaS` dominates the `Delta_(r )H` at high temperatureC. at high temperature both `Delta_(r )S` and `Delta_(r )H` becomes negativeD. thermodynamics can not say anything about spontaneity