Question

Consider the following half cell reactions with corresponding standard reduction potentials.
(A) \[\mathrm{Cl}_{2(\mathrm{g})}+2\mathrm{e}^{-}\rightarrow2\mathrm{Cl}_{(\mathrm{aq})}^{-},\mathrm{E}^{0}=+1.36\mathrm{V}\]
(B) \[\mathrm{Al^{+3}(aq)}+3\mathrm{e^{-}}\to\mathrm{Al_{(s)},E^{o}}=+1.66\mathrm{V}\]
(C) \[\mathrm{Na^{+}}_{(aq)}+\mathrm{e^{-}}\rightarrow\mathrm{Na}_{(s)},\mathrm{E^{o}}=-2.71\mathrm{V}\]
(D) \[\mathrm{Cu^{+2}}_{(aq)}+2\mathrm{e^{-}}\to\mathrm{Cu_{(s)}},\mathrm{E^{o}}=+0.377\mathrm{V}\]
The strongest oxidizing and reducing agents respectively are -

विकल्प

• Al⁺³ and Na⁺

• Na⁺ and Cl₂

• Cl₂ and Na

• Cu⁺² and Al⁺³

Answer 1

Al⁺³ and Na⁺

Explanation:

Al⁺³ has the largest (positive) standard reduction potential, hence it is the strongest oxidising agent. Na⁺ has the lowest value of standard reduction potential, hence it is the strongest reducing agent.