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27 April, 10:23

Which species in each pair is a better oxidizing agent under standard-state conditions? (a) br2 au3 + (b) h2 ag + (c) cd2 + cr3 + (d) o2 in acidic media o2 in basic media?

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  1. 27 April, 12:01
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    (a) Au³⁺; (b) Ag⁺; (c) Cd²⁺; (d) O₂ in acidic media

    Explanation:

    You've had Trends in the Periodic Table. Now, here are Trends in Standard Reduction Potentials.

    The strength of oxidizing agents increases from bottom to top on the left-hand side. The strength of reducing agents increases from top to bottom on the right-hand side.

    Thus, for each pair of half reactions, we need to look only at which one has the more positive standard reduction potential.

    (a) Br₂/Au³⁺

    Au³⁺ (aq) + 3e⁻ ⟶ Au (s) 1.498 V

    Br₂ (ℓ) + 2e⁻ ⟶ 2Br⁻ (aq) 1.066 V

    Au³⁺ is the stronger oxidizing agent.

    (b) H₂/Ag⁺

    Ag⁺ (aq) + e⁻ ⟶ Au (s) 0.7996 V

    H₂ (g) + 2e⁻ ⟶ 2H⁻ (aq) - 2.33 V

    Ag⁺ is the stronger oxidizing agent.

    (c) Cd²⁺/Cr³⁺

    Cd²⁺ (aq) + e⁻ ⟶ Cd (s) - 0.4030 V

    Cr³⁺ (aq) + 3e⁻ ⟶ Cr (s) - 0.744 V

    Cd²⁺ is the stronger oxidizing agent.

    (d) O₂, H⁺/O₂, OH⁻

    O₂ (g) + 4H⁺ (aq) + 4e⁻ ⟶ 2H₂O (ℓ) 1.224 V

    O₂ (g) + H₂O (ℓ) + 4e⁻ ⟶ 4OH⁻ (aq) 0.401 V

    O₂ in acid is the stronger oxidizing agent.
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