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.
When `CaCO_(3)` is heated to a high temperature, it undergoes decomposition into `CaO` and `CO_(2)` whereas it is quite stable at room temperature. The most likely explanation of its is

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 25^(2)C, X_(2)O_(4)(l) rarr 2XO_(2) DeltaH = 2.0 kcal and DeltaS = 20 cal K^(-1) . the reaction would be

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 energy factor T DeltaS changes appreciably. Thus, spontaneity of a process depends very much on temperature. For the reaction at 25^(0)C, X_(2)O_(4)(l) rarr 2XO_(2) DeltaH = 2.0 kcal and DeltaS = 20 cal K^(-1) . the reaction would be

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. A reaction has value of DeltaH - 20 kcal at 200K , the reaction is spontaneous, below this temperature, it is not. the values DeltaG and DeltaS at 400K are, respectively

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 energy factor T DeltaS changes appreciably. Thus, spontaneity of a process depends very much on temperature. A reaction has value of DeltaH = 20 kcal at 200K , the reaction is spontaneous, below this temperature, it is not. the values DeltaG and DeltaS at 200K are, respectively

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. The enthalpy change for a certain reaction at 300K is -15.0 kcal mol^(-1) . The entropy change under these conditions is -7.2 cal K^(-) mol^(-1) . The free enegry change for the reaction and its spontaneous//nonspontaneous character will be

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. The enthalpy change for a certain reaction at 300K is -15.0 kcal mol^(-1) . The entropy change under these conditions is -7.2 cal K^(-) mol^(-1) . The free enegry change for the reaction and its spontaneous//nonspontaneous character will be

Free energy change is related to enthalpy and entropy changes as:

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 kcla K^(-1) . If DeltaH and DeltaS are assumed to be constant over the temperature range, at what temperature will the reaction become spontaneous?

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?

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. The dissolution of CaCI_(2).6H_(2)O in a large volume of water is endothermic to the extent of 3.5 kcal mol^(-1) . For the reaction. CaCI_(2)(s) +6H_(2)O(l) rarrCaCI_(2).6H_(2)O(s) DeltaH is -23.2 kcal . The heat of solution of anhydrous CaCI_(2) in large quantity of water will be