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Considering entropy (S) as a thermodynam...

Considering entropy `(S)` as a thermodynamics parameter, the criterion for the spontaneity of any process is

A

`DeltaS_("system") + DeltaS_("surrounding") gt 0 `

B

`DeltaS_("system") - DeltaS_("surrounding") gt0`

C

`DeltaS_("system") gt 0`

D

`DeltaS_("surrounding") gt 0`

Text Solution

Verified by Experts

The correct Answer is:
A
For spontaneous process, `DeltaS` must be positive .
In reversible process
`DeltaS_("system") + DeltaS_("surrounding")=0`
Hence, system is present in equilibrium . (i.e., it is not spontaeous process)
While in irreversible process
`DeltaS_("system") + DeltaS_("surrounding") gt 0`
Hence, in the process `DeltaS` is positive.
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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?

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. One mole of ice si converted to liquid at 273 K, H_(2)O(s) and H_(2)O(l) have entropies 38.20 and 60.03 J mol^(-1) dg^(-1) . Enthalpy change in the conversion will be