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The thermodynamic property that measures...

The thermodynamic property that measures the extent of molecular disorder is called entropy. The direction of a spontaneous process for which the energy is constant is always the one that increases the molecular disorder. Entropy change of phase transformation can be calculated using Trouton's formula `(DeltaS= (DeltaH)/(T))`. In the reversible adiabatic process, however, `DeltaS` will be zero. The rise in temperature in isobaric and isochoric conditions is found to increase the randomness or entropy of the system. `DeltaS= 2.303 C log (T_(1)//T_(2)), (C = C_(P) or C_(V))`
If water in an insulated vessel at `-10^(@)C`, suddenly freezes, the entropy change of the system will be

A

`+10 JK^(-1) mol^(-1)`

B

`-10 J K^(-1) mol^(-1)`

C

zero

D

equal to that of sourroundings

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The correct Answer is:
C
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The thermodynamic property that measures the extent of molecular disorder is called entropy. The direction of a spontaneous process for which the energy is constant is always the one that increases the molecular disorder. Entropy change of phase transformation can be calculated using Trouton's formula (DeltaS= (DeltaH)/(T)) . In the reversible adiabatic process, however, DeltaS will be zero. The rise in temperature in isobaric and isochoric conditions is found to increase the randomness or entropy of the system. DeltaS= 2.303 C log (T_(1)//T_(2)), (C = C_(P) or C_(V)) The entropy change in an adiabatic process is

The thermodynamic property that measures the extent of molecular disorder is called entropy. The direction of a spontaneous process for which the energy is constant is always the one that increases the molecular disorder. Entropy change of phase transformation can be calculated using Trouton's formula (DeltaS= (DeltaH)/(T)) . In the reversible adiabatic process, however, DeltaS will be zero. The rise in temperature in isobaric and isochoric conditions is found to increase the randomness or entropy of the system. DeltaS= 2.303 C log (T_(1)//T_(2)), (C = C_(P) or C_(V)) The melting point of a solid is 300K and its latent heat of fusion is 600 cal mol^(-1) . The entropy change for the fusion of 1 mole of the soli (in cal K^(-1) ) at the same temperature would be:

The entropy change in adiabatic process is

For an isothermal reversible phase transition process , Delta S is

The entropy value at temperature T is

AAKASH SERIES-CHEMICAL THERMODYNAMICS-Practice Sheet- Exercise-III
  1. Some statements are given with regard to entropy. The incorrect statem...

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  2. 2H(2(g)) + O(2(g)) rarr 2H(2)O((l)) , DeltaH= -ve and DeltaG= -ve. The...

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  3. Based on the third law of themodynamics, the entropy can be obtained u...

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  4. When charcoal burns in air signs of DeltaH and DeltaS "are " 2C((s)) +...

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  5. DeltaS("surr") " for " H(2) + 1//2O(2) rarr H(2)O, DeltaH -280 kJ at 4...

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  6. The direct conversion of A to B is difficult, hence it is carried out ...

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  7. The incorrect statement according to second law of themodynamics is

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  8. Entropy of a system depends upon

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  9. Which processes involve increase in entropy?

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  10. Which statements are correct as per laws of thermodynamics?

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  11. For A rarr B, DeltaH= 3.5 kcal mol^(-1), DeltaS= 10 cal mol^(-1) K^(-1...

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  12. The change in Gibbs free energy of the system along provides a criteri...

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  13. The change in Gibbs free energy of the system along provides a criteri...

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  14. The thermodynamic property that measures the extent of molecular disor...

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  15. The thermodynamic property that measures the extent of molecular disor...

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  16. The thermodynamic property that measures the extent of molecular disor...

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  17. Match the following columns

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  18. Match the following columns

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  19. A quantity of 4.0 moles of an ideal gas at 20^(@)C expands isothermall...

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  20. In how many of the following entropy increases? {:((a) N(2(g)) + 3H(...

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