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For a given reaction DeltaG obtained was...

For a given reaction `Delta`G obtained was having positive sign convention. State whether the reaction was spontaneous or non-spontaneous.

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To determine whether the reaction is spontaneous or non-spontaneous based on the sign of ΔG, we can follow these steps: ### Step-by-Step Solution: 1. **Understanding ΔG**: The Gibbs free energy change (ΔG) is a thermodynamic potential that can predict the spontaneity of a reaction. 2. **Sign of ΔG**: - If ΔG < 0 (negative), the reaction is spontaneous. ...
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For reaction, 2K_((g))+L_((g))rarr2M_((g)),DeltaU^(@)=-"10.5 KJ and "DeltaS^(@)=-"44.1 J K"^(-1) . Calculate DeltaG^(@) for the reaction and predict whether the reaction will be spontaneous or non-spontaneous?

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

AAKASH INSTITUTE ENGLISH-THERMODYNAMICS-ASSIGNMENT (Section -D) Assertion-Reason Type Questions
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  2. A : C("diamond") rightarrow C("graphite") Delta H and Delta U are sam...

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  3. A: Specific heat is an intensive property R: Heat capacity is an ext...

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  4. A: All reactions which are exothermic are spontaneous R: All reactio...

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  5. A: Enthalpy of neutralisation of 1 equivalent each of HCl and H(2)SO(...

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  6. DeltaU is state function but heat and work are not state funcitons.

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  7. A : Dissolution of sugar in water proceed via increases in entropy R...

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  8. A : For an isolated system Delta G = - TDeltaS("total") R: For an i...

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  9. A: Combustion is an exothermic process. R: Combustion is a spontaneo...

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  10. A: Total enthalpy change of a multistep process is sum of Delta H(1) ...

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  11. A : Bond energy is equal to enthalpy of formation with negative sign. ...

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  12. A: Delta H is positive for endothermic reactions. R : If total entha...

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  13. A : The energy of the universe is constant, whereas the entropy of the...

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  14. A: A non- spontaneous process becomes spontaneous when coupled with a ...

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  15. A: An ideal crystal has more entropy than a real crystal. R: An idea...

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  16. A: Work done in an irreversible isothermal process at constant volume ...

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