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Statement-1: Decrease of free energy dur...

Statement-1: Decrease of free energy during the process under constant temperature and pressure provides a measure of its spontaneity.
Statement -2: A spontaneous change must have +ve sign of `DeltaS_("system").`

A

Statement-1 is True, Statement -2 is True, Statement-2 is a correct explanation for Statement-1.

B

Statement -1 is True ,Starement -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:
c
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The change in Gibbs free energy (DeltaG) of the system along provides a criterion for the spontaneity of a process at constant temperature and pressure. A change in the free energy of a system at constant temperature and pressure will be: DeltaG_("system")=DeltaH_("system")-TDeltaS_("system") At constant temperature and pressure: DeltaG_("system")lt0 (Spontaneous) DeltaG_("system")=0 (equilibrium) DeltaG_("system")gt0 (non-spontaneous) Free energy is related to the equilibrium constant as: DeltaG^(@)=2.303RTlog_(10)K_(e) . Q. For a reaction to be spontaneous at all temperature.

The change in Gibbs free energy (DeltaG) of the system along provides a criterion for the spontaneity of a process at constant temperature and pressure. A change in the free energy of a system at constant temperature and pressure will be: DeltaG_("system")=DeltaH_("system")-TDeltaS_("system") At constant temperature and pressure: DeltaG_("system")lt0 (Spontaneous) DeltaG_("system")=0 (equilibrium) DeltaG_("system")gt0 (non-spontaneous) Free energy is related to the equilibrium constant as: DeltaG^(@)=2.303RTlog_(10)K_(e) . Q. If b oth DeltaH and DeltaS are negative, the reaction will be spontaneous:

Knowledge Check

  • Assertion(A) : Decrease of free energy during the process under particular conditions provides a measure of its spontaneity. Reason(R ) : A spontaneous change must have +ve sign of DeltaS_("total") .

    A
    Both `A`and `R` are true and `R` is the correct explantion of `A`
    B
    Both `A`and `R` are true and `R` is not a correct explantion of `A`
    C
    `A` is true but `R` is false
    D
    `A` is false but `R` is true

  • The changes in gibbs energy (Delta G) of a system for a process at constant temperature and pressure is

    A
    `Delta G = Delta H // TS`
    B
    `Delta G = T Delta S // Delta H`
    C
    `Delta G = Delta H - T Delta S`
    D
    `Delta G = Delta S - T Delta H`

  • The change in Gibbs free energy of the system alone provides a criterion for the spontaneity of a process at constant temperature and pressure. A change in the free energy of a system at constant temperature and pressure will be : DeltaG_("system")=DeltaH_("system")-T DeltaS_(system") For a system in equilibrium, DeltaG=0 , under conditions of contant....

    A
    Temperature and pressure
    B
    Temperature and volume
    C
    Pressure and volume
    D
    Energy and volume

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    The change in Gibbs free energy (DeltaG) of the system along provides a criterion for the spontaneity of a process at constant temperature and pressure. A change in the free energy of a system at constant temperature and pressure will be: DeltaG_("system")=DeltaH_("system")-TDeltaS_("system") At constant temperature and pressure: DeltaG_("system")lt0 (Spontaneous) DeltaG_("system")=0 (equilibrium) DeltaG_("system")gt0 (non-spontaneous) Free energy is related to the equilibrium constant as: DeltaG^(@)=2.303RTlog_(10)K_(e) . Q. A reaction has positive values of DeltaH and DeltaS . From this you can deduce that the reaction:

    The change in Gibbs free energy of the system alone provides a criterion for the spontaneity of a process at constant temperature and pressure. A change in the free energy of a system at constant temperature and pressure will be : DeltaG_("system")=DeltaH_("system")-T DeltaS_(system") The free energy for a reaction having DeltaH=31400 cal, DeltaS=32 cal L^(-1) mol^(-1) at 1000^(@)C

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    Statement 1: For every chemical reaction at equilibrium, standard Gibbs energy of reaction is zero, and Statement 2: At constant temperature and pressure, chemical reactions are spontaneous in the direction of decreasing Gibbs energy.

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