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30 July, 09:35

For a chemical reaction to be spontaneous at all temperatures, which of the following conditions must be met? a. ΔS° > 0, ΔH° > 0 b. ΔS° > 0, ΔH° < 0 c. ΔS° < 0, ΔH° < 0 d. ΔS° 0 e. It is not possible for a reaction to be spontaneous at all temperatures.

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  1. 30 July, 09:46
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    b. ΔS° > 0, ΔH° < 0

    Explanation:

    According the equation of Gibb's free energy -

    ∆°G = ∆°H - T∆°S

    ∆°G = is the change in gibb's free energy

    ∆°H = is the change in enthalpy

    T = temperature

    ∆°S = is the change in entropy.

    And, the sign of the Δ°G, determines whether the reaction is Spontaneous or non - Spontaneous or at equilibrium,

    i. e.,

    if

    Δ°G <0, the reaction is SpontaneousΔ°G> 0, the reaction is non - Spontaneous Δ°G = 0, the reaction is at equilibrium

    The reaction has the value for ∆°H 0 i. e., positive

    Now,

    ∆°G = ∆°H - T∆°S

    = ( - ∆°H) - T ( + ∆°S)

    = ( - ∆°H) - T (∆°S)

    ∆°G = negative

    Hence,

    Δ°G < 0, the reaction is Spontaneous.
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