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Statement-1: For a process to be spontan...

Statement-1: For a process to be spontaneous, `Delta G` as well as `Delta S` has to be less than zero.
Statement-2 : For spontaneous change, `Delta S_("total") gt 0`

A

Statement-1 is true, Statement-2, is true, Statement -2 is a correct explanation for statement-1

B

Statement-1 is true, Statement-2, is true, Statement -2 is not a correct explanation for statement-1

C

Statement-1 is true, Statement-2 is false

D

Statement-1 is false, Statement-2 is true

Text Solution

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The correct Answer is:
D
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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

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  6. Statement-1 : Many endothermic reactions that are not spontaneous at r...

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  7. Statement: In the case of an ideal gas the changes in Gibbs and Helmho...

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  11. Statement-1 : The amount of heat change during the isothermal free exp...

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  12. Statement-1: The enthalpy of formation of H(2)O(l)is greater than of H...

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  13. Statement-1: Heat of neutralisation of H(3)PO(4) with NaOH is more tha...

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  15. Staetement -1: The magniyude of the work involed in an isothermal expa...

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  16. Statement -1: For every chmical reaction at equilibrium , standard Gid...

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  17. Statement-1: There is a natural asymmetry between work to heat and con...

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  18. Statement -1: Entropy change in reversible adiabatic expansion of an i...

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