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Gibbs-Helmholtz equation is………….. ....

Gibbs-Helmholtz equation is………….. .

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`DeltaG= DeltaH - T DeltaS`
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State and explain Gibbs Helmholtz equation.

Write Gibbs Helmholtz equation giving meanings of the symbols used.

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. 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. 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 :

Statement: In the case of an ideal gas the changes in Gibbs and Helmholtz free energies are equal to each other ( DeltaG=DeltaA ) for isothermal reversible process. Explanation: There is no change in internal energies and enthalpies for ideal gas at constant temperature.

PRADEEP-THERMODYNAMICS-FILL IN THE BLANKS
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  2. For triatomic gases such as CO(2) the ratio (C(p))/(C(v)) is equal to ...

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  3. Bomb calorimeter is used to determine the value of ...............

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  4. For exothermic reactions, the enthalpy of products is"…........" than...

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  5. The enthalpy of combustionof 1 mole of H(2) to form H(2)O(l) is"…........

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  6. The heat produced from the complete combustion of 1 g of fuel or food ...

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  7. The allotropic form of sulphur for which standard enthalpy of formatio...

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  8. The enthalpy of solution of sodium chloride is 4 kJ mol^(-1) and its e...

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  9. The enthalpies of solution of anhydrous CuSO(4) and hydrated CuSO(4). ...

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  10. The bond energy of H(2) is found to be 435 kJ mol^(-1). Therefore, th...

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  11. Enthalpy of dissociation of H(2)O molecules into H^(+) and OH^(-) ions...

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  12. For an endothermic process to be spontaneous, the factor T Delta S sho...

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  13. Why is the enthalpy of sublimation equal to the sum of enthalpy of fus...

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  14. The expression for the entropy change when a gas expands from volume V...

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  15. Gibbs-Helmholtz equation is………….. .

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  16. In terms of work, the decrease in free energy during a process is equa...

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  17. Free energy change ( DeltaG) is related to the total entropy change (D...

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  18. A reaction is nono-spontaneous at high temperature but became spontan...

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  19. Standard free energy change(Delta G^(@)) of a reaction is related to i...

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  20. Entropy of perfectly crystalline solid is taken as zero at 0 K.

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