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What is significance of T DeltaS in Delt...

What is significance of `T DeltaS` in `DeltaG = DeltaH - T DeltaS`?

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To understand the significance of \( T \Delta S \) in the equation \( \Delta G = \Delta H - T \Delta S \), we can break it down step by step. ### Step-by-Step Solution: 1. **Understanding the Equation**: The equation \( \Delta G = \Delta H - T \Delta S \) is known as the Gibbs free energy equation. It relates the change in Gibbs free energy (\( \Delta G \)) to the change in enthalpy (\( \Delta H \)) and the change in entropy (\( \Delta S \)) at a given temperature \( T \). 2. **Identifying the Terms**: ...
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Derive the equation, DeltaG = DeltaH - T DeltaS .

What is Gibbs free energy ? Derive the relation, Delta_G = DeltaH - T Delta S . Discuss the free energy criterion for the spontaneity of a process.

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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 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 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

Free enegry , G = H - TS , is state function that indicates whther a reaction is spontaneous or non-spontaneous. If you think of TS as the part of the system's enegry that is disordered already, then (H -TS) is the part of the system's energy that is still ordered and therefore free to cause spontaneous change by becoming disordered. Also, DeltaG = DeltaH - T DeltaS From the second law of thermodynamics, a reaction is spontaneous if Delta_("total")S is positive, non-spontaneous if Delta_("total")S is negative, and at equilibrium if Delta_('total")S is zero. Since, -T DeltaS = DeltaG and since DeltaG and DeltaS have opposite sings, we can restate the thermodynamic criterion for the spontaneity of a reaction carried out a constant temperature and pressure. IF DeltaG lt 0 , the reaction is spontaneous. If DeltaG gt 0 , the reaction is non-spontaneous. If DeltaG = 0 , the reaction is at equilibrium. Read the above paragraph carefully and answer the following questions based on the above comprehension. For the spontaneity of a reaction, which statement is true?

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. 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) . For the reaction. CaCl_(2)(s) +6H_(2)O(l) rarrCaCl_(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

Free enegry , G = H - TS , is state function that indicates whther a reaction is spontaneous or non-spontaneous. If you think of TS as the part of the system's enegry that is disordered already, then (H -TS) is the part of the system's energy that is still ordered and therefore free to cause spontaneous change by becoming disordered. Also, DeltaG = DeltaH - T DeltaS From the second law of thermodynamics, a reaction is spontaneous if Delta_("total")S is positive, non-spontaneous if Delta_("total")S is negative, and at equilibrium if Delta_('total")S is zero. Since, -T DeltaS = DeltaG and since DeltaG and DeltaS have opposite sings, we can restate the thermodynamic criterion for the spontaneity of a reaction carried out a constant temperature and pressure. IF DeltaG lt 0 , the reaction is spontaneous. If DeltaG gt 0 , the reaction is non-spontaneous. If DeltaG = 0 , the reaction is at equilibrium. Read the above paragraph carefully and answer the following questions based on the above comprehension. A particular reaction has a negative value for the free energy change. Then at ordinary temperature

Free enegry , G = H - TS , is state function that indicates whther a reaction is spontaneous or non-spontaneous. If you think of TS as the part of the system's enegry that is disordered already, then (H -TS) is the part of the system's energy that is still ordered and therefore free to cause spontaneous change by becoming disordered. Also, DeltaG = DeltaH - T DeltaS From the second law of thermodynamics, a reaction is spontaneous if Delta_("total")S is positive, non-spontaneous if Delta_("total")S is negative, and at equilibrium if Delta_('total")S is zero. Since, -T DeltaS = DeltaG and since DeltaG and DeltaS have opposite sings, we can restate the thermodynamic criterion for the spontaneity of a reaction carried out a constant temperature and pressure. IF DeltaG lt 0 , the reaction is spontaneous. If DeltaG gt 0 , the reaction is non-spontaneous. If DeltaG = 0 , the reaction is at equilibrium. Read the above paragraph carefully and answer the following questions based on the above comprehension. Which of the following is true for the reaction? H_(2)O(l) hArr H_(2)O(g) at 100^(@)C and 1 atmosphere

CENGAGE CHEMISTRY ENGLISH-THERMODYNAMICS-Exercises (Subjective)
  1. For which of the following processes is DeltaS negative?

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  2. Predict DeltaH gt DeltaU or DeltaH lt DeltaU. a. C("graphite") +O(2)...

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  3. What is significance of T DeltaS in DeltaG = DeltaH - T DeltaS?

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  4. What is the physical significance of free energy?

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  5. How does T DeltaS determine the spontaneity of process?

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  6. N(2)(g) +3H(2)(g) rarr 2NH(3): DeltaH =- 92 kJ is Haber's process for...

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  7. The energy released in the neutralisation of H(2)SO(4) and KOH is 59.1...

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  8. CH(4)(g) +2O(2)(g) rarr CO(2)(g) +2H(2)O(l), DeltaH =- 890 kJ what i...

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  9. H(2)(g) +Cl(2)(g) rarr 2HCl(g) +185 kJ. State whether this reaction is...

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  10. The heat of neutralization of a strong acid by a strong base is a cons...

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  11. Explain why heat of neutralisation of strong acid and weak base is les...

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  12. Find the enthalpy of formation of hydrogen flouride on the basis of fo...

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  13. Calculate the enthalpy of formation of water, given that the bond ener...

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  14. Calculate the resonance enegry of NO(2) ( :O-N=O: ) The measured ent...

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  15. Boiling point of an organic compound is 310K. Its enthalpy of vaporisa...

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  16. Predict whether the following reaction is possible or not at 300k. 2...

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  17. Calculate the standard free energy change for the reaction: H(2)(g)...

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  18. Calculate the entropy change for the following reaction H(2)(g) +CI(...

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  19. Heat of neutralisation between HCI and NaOH is 13.7kcal and between HC...

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  20. Find the heat of formation of ethyl alcohol for following data C(s) ...

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