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
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
`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
Text Solution
Verified by Experts
The correct Answer is:
A
`(DeltaG)_(PT)=2000-(20xx298)`
`=-3960 " J"//"mol"`
`=-3960 " J"//"mol"`
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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 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
Knowledge Check
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 :
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. 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
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
The relation DeltaG=DeltaH-TDeltaS was given by
The relation DeltaG=DeltaH-TDeltaS was given by
A
Boltzmann
B
Faraday
C
Gibbs-Helmholtz
D
Thomson
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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. 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
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?
The relation DeltaG=DeltaH-TDeltaS was given by
The equilibrium constant of a reaction is. The standard free energy change of the reaction temperature is