Given: Zn^2+ (aq) + 2e^- rightarrow Zn(s); E^degree = -0.76 V Cu^2+ (aq) + 2e^-

Question

Given: Zn^2+ (aq) + 2e^- rightarrow Zn(s); E^degree = -0.76 V Cu^2+ (aq) + 2e^- rightarrow Cu(s); E degree = 0.34 V Cr_2O_7^2- (aq) + 14H^+(aq) + 6e^- rightarrow 2Cr^3+(aq) + H_2O(l) + 7 H_2O(l); E degree = 1.33 V Which of the following species is the strongest oxidizing agent? A) Zn^2+ B) Zn C) Cu D) Cr_2O_7^2-?- E) Cr^3+ Given: Pb^2 + (aq) + 2e^- rightarrow Pb(s); E degree = -0.13 V Mg^2+ (aq) + 2e^- rightarrow Mg(s), E degree = - 2.38 V Ag^+ (aq) + e^- rightarrow Ag(s); E degree = 0.80 V 2H^+ (aq) + 2e^- rightarrow H_2(g); E degree = 0.00 V Under standard-state conditions, which of the following species is the best reducing agent? A) Pb B) Mg^2+ C) Ag^+ D) Ag E) H_2

Explanation / Answer

Ans 35- Using reduction table , more the negative value of standard reduction potential , the element is strong reducing reagend and weak oxidising agent, if we reserve the equation the sign of standard potential also changes

So, option D is correct hence it is most positive.

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