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Examine the following half-reactions and select the strongest reducing agent among the substances listed in the answers. 

 

(A)Br-(aq)

(B)Ca2+(aq)

(C)Pb(s)

(D)Pt(s)

(E)Ca(s)

 

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Related questions

which of the following pairs of substances could be used to construct a single redox electrode

Examine the following half-reactions and select the strongest oxidizing agent among the substances.

[PtCl4] 2– (aq) + 2e– Pt(s) + 4Cl– (aq) E° = 0.755 V

RuO4(s) + 8H+ (aq) + 8e– Ru(s) + 4H2O(l) E° = 1.038 V

FeO4 2– (aq) + 8H+ (aq) + 3e– Fe3+(aq) + 4H2O(l) E° = 2.07 V

H4XeO6(aq) + 2H+ (aq) + 2e– XeO3(aq) + 3H2O(l) E° = 2.42 V

A) [PtCl4] 2– (aq) B) RuO4(s) C) HFeO4 – (aq) D) H4XeO6(aq) E) Cl– (aq)

The study guide says the answer is D) H4XeO6(aq) but isn't this one being oxidized? So how can it be the strongest oxidizing agent?

Please help!

Examine the following half-reactions and select the strongest oxidizing agent among the species listed.

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Sr 2+(aq) + 2e- = Sr (s) E= -2.89 V

Co 2+(aq) + 2e- = Co (s) E= -0.28 V

a. Co 2+(aq)

b. Fe (s)

c. Fe 2+ (aq)

d. Sr 2+ (aq)

e. Cr 2+ (aq)

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