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Free energy change ( DeltaG) is related ...

Free energy change ( `DeltaG)` is related to the total entropy change `(DeltaS_("total") `viz`DeltaS_("system") + DeltaS_("surrounding"))` as `"....................."`.

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To relate the free energy change (ΔG) to the total entropy change (ΔS_total), we can follow these steps: ### Step-by-Step Solution: 1. **Understanding Free Energy Change**: The free energy change (ΔG) is defined by the equation: \[ \Delta G = \Delta H - T \Delta S ...
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Free energy change is related to enthalpy and entropy changes as:

In a reversible process, DeltaS_("system") + DeltaS_("surrounds") is:

The total entropy change (DeltaS_("total")) for the system and surrounding of a spontaneous process is given by

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The relationship between the free energy change (DeltaG) and entropy change (DeltaS) at constant temperature (T) si

Free energy, G=H-TS, is a state function that includes whether a reaction is spontaneous or non-spontaneous. If you think of TS as the part of the system's energy 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-TDeltaS To see what this equation for free energy change has to do with spontaneity let us return to relationship. DeltaS_("total")=DeltaS_("sys")+DeltaS_("surr") = DeltaS + DeltaS_("surr") (It is generally understood that symbols without subscript refer to the system not the surroundings.) DeltaS_("surr")=-(DeltaH)/T , where DeltaH is the heat gained by then system at constant pressure. DeltaS_("total") = DeltaS -(DeltaH)/T rArr TDeltaH_("total")=DeltaH-TDeltaS rArr -TDeltaS_("total") =DeltaH-TDeltaS i.e. DeltaG=-TDeltaS_("total") From second law of thermodynamics, a reaction is spontaneous if DeltaS_("total") is positive, non-spontanous if DeltaS_("total") is negative and at equilibrium if DeltaS_("total") is zero. Since, -TDeltaS=DeltaG and since DeltaG and DeltaS have opposite signs, we can restate the thermodynamic criterion for the spontaneity of a reaction carried out at constant temperature and pressure. If DeltaG lt 0 , the reaction is spontaneous. If DeltaG gt 0 , the reaction is non-spontanous. If DeltaG=0 , the reaction is at equilibrium. In the equation, DeltaG=DeltaH-TDeltaS , temperature is a weighting factor that determine the relative importance of enthalpy contribution to DeltaG . Read the above paragraph carefully and answer the following questions based on above comprehension: If an endothermic reaction is non-spontaneous at freezing point of water and becomes feasible at its boiling point, then

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