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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

zero

B

always positive

C

always negative

D

sometimes positive and sometimes negative

Text Solution

Verified by Experts

The correct Answer is:
A
Adiabatic `rArr a = 0`
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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

How does entropy changes with the transformation at different temperature?