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18 February, 06:46

Based on the standard free energies of formation, which of the following reactions represent a feasible way to synthesize the product?

A. N2 (g) + H2 (g) →N2H4 (g); ΔG∘f=159.3 kJ/mol

B. 2Na (s) + O2 (g) →Na2O2 (s); ΔG∘f=-447.7kJ/mol

C. C (s) + 2S (s) →CS2 (g); ΔG∘f=67.1 kJ/mol

D. Ca (s) + 12O2 (g) →CaO (s); ΔG∘f=-604.0 kJ/mol

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  1. 18 February, 07:03
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    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 ΔG, determines whether the reaction is Spontaneous or non Spontaneous or at equilibrium,

    i. e.,

    if

    • ΔG < 0, the reaction is Spontaneous

    • ΔG > 0, the reaction is non Spontaneous

    • ΔG = 0, the reaction is at equilibrium

    a.

    N₂ (g) + H₂ (g) → N₂H₄ (g); ΔG⁰f = 159.3 kJ/mol

    ΔG > 0, the reaction is non Spontaneous, the reaction is not feasible in the forward direction

    b.

    2Na (s) + O₂ (g) → Na₂O₂ (s); ΔG⁰ f = - 447.7kJ/mol

    ΔG < 0, the reaction is Spontaneous, the reaction is feasible in the forward direction.

    c.

    C (s) + 2S (s) → CS₂ (g); ΔG⁰f = 67.1 kJ/mol

    ΔG > 0, the reaction is non Spontaneous, the reaction is not feasible in the forward direction

    d.

    Ca (s) + 12 O₂ (g) → CaO (s); ΔG⁰f = - 604.0 kJ/mol

    ΔG < 0, the reaction is Spontaneous, the reaction is feasible in the forward direction.
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