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Under what conditions will the reaction ...

Under what conditions will the reaction ocçur, if
i) both 'Delta H' and 'Delta S' are positive
ii) both 'Delta H' and 'Delta S' are negative

Answer

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For a reversible reaction at equilibrium Delta S _(syst) + Delta S _(surr) is

Free energy, G=- TS, is a state funtion that indicates whether a reaction is spontaneous or non-spontaneous if you think of TS as the part of the system's energy that is discordered already, then (H-TS) is the part of system's energy that is still orderd and therefore free to cause spontaneous change by becoming disorder Also, Delta G = Delta H - T Delta S Form the second law of thermodyamics, a reaction is spontaneous if Delta _("total") S is + ve, nonspontaneous if Delta _("total")S is negative and at equilibrium if Delta_(total)S is zero. Since, - T Delta S= Delta C and since Delta G and Delta S have oposite single we can restate the themodynmaic creation for the spontaneity of a reaction oout at constant temperature and pressure. If Delta G lt 0, the reaction is spontaneous. If Delta G gt 0, the reaction is non-spontaneous. If Delta G =0, the reaction is at equilibrium. Which of the following is trur for the reaction ? H _(2) O (1) hArr H _(2) O (g) at 100^(@) C and 1 atmosphere

Knowledge Check

  • The relation 'Delta G=Delta H-T Delta S' was given by

    A
    Boltzman
    B
    Faraday
    C
    Gibbs'Helmholtz
    D
    Thomson

  • Assertion : If both Delta H ^(@) and Delta S ^(@) are positive then reaction will be spontaneous at high temperature. Reason : All processes with positive entropy change are spontaneous.

    A
    and (R) are correct and (R) is the correct explanation of(A).
    B
    If both (A) and (R) are correct, but (R) is not the correct explanation of(A).
    C
    If(A) is correct, but (R) is incorrect.
    D
    If both (A) and (R) are incorrect.

  • Assertion : There is no reaction known for which Delta G is positive, yet it is spontaneous. Reason : For photochemical reaction, DeltaG is negative,

    A
    and (R) are correct and (R) is the correct explanation of(A).
    B
    If both (A) and (R) are correct, but (R) is not the correct explanation of(A).
    C
    If(A) is correct, but (R) is incorrect.
    D
    If both (A) and (R) are incorrect.

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    Free energy, G=- TS, is a state funtion that indicates whether a reaction is spontaneous or non-spontaneous if you think of TS as the part of the system's energy that is discordered already, then (H-TS) is the part of system's energy that is still orderd and therefore free to cause spontaneous change by becoming disorder Also, Delta G = Delta H - T Delta S Form the second law of thermodyamics, a reaction is spontaneous if Delta _("total") S is + ve, nonspontaneous if Delta _("total")S is negative and at equilibrium if Delta_(lot)S is zero. Since, - T Delta S= Delta C and since Delta G and Delta S have oposite single we can restate the themodynmaic creation for the spontaneity of a reaction oout at constant temperature and pressure. If Delta G lt 0, the reaction is spontaneous. If Delta G gt 0, the reaction is non-spontaneous. If Delta G =0, the reaction is at equilibrium. A particular reaction ha a negative value for the free enregy charge. Then at ordinary temmperature

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