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9 February, 09:09

Be sure to answer all parts. Write equations for the oxidation of Fe and of Al. Use ΔG o f to determine whether either process is spontaneous at 25°C. (a) Equation for oxidation of iron: ΔG o rxn : kJ Is the oxidation of iron spontaneous at 25°C? yes no (b) Equation for the oxidation of aluminum: ΔG o rxn : kJ Is the oxidation of aluminum spontaneous at 25°C? yes no

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  1. 9 February, 09:25
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    (a) Fe (s) ⇒ Fe²⁺ (aq) + 2 e⁻

    ΔG° = - 85 kJ

    Spontaneous

    (b) Al (s) ⇒ Al³⁺ (aq) + 3 e⁻

    ΔG° = - 480 kJ

    Spontaneous

    Explanation:

    (a) The equation for the oxidation of iron is:

    Fe (s) ⇒ Fe²⁺ (aq) + 2 e⁻ E° = 0.44 V

    We can calculate the standard Gibbs free energy (ΔG°) using the following expression.

    ΔG° = - n. F. E°

    where,

    n are the moles of electrons transferred

    F is the Faraday's constant

    ΔG° = - 2 mol * (96,468 * 10⁻³ kJ/V. mol) * 0.44 V = - 85 kJ

    ΔG° < 0, which means that the reaction is spontaneous.

    (b) The equation for the oxidation of aluminum is:

    Al (s) ⇒ Al³⁺ (aq) + 3 e⁻ E° = 1.66 V

    ΔG° = - 3 mol * (96,468 * 10⁻³ kJ/V. mol) * 1.66 V = - 480 kJ

    ΔG° < 0, which means that the reaction is spontaneous.
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