Suppose the reference electrode for Table 6M.1 were the standard calomel electrode, Hg₂Cl₂/Hg, Cl₂([Cl₂] = 1.00 mol · L^–1), with its E° set equal to 0. Under this system, what would be the potential for

(a) The standard hydrogen electrode;

(b) The standard Cu²⁺/Cu redox couple?

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TABLE 6M.1 Standard Potentials at 25 °C* Species Oxidized form is strongly oxidizing F₂/F Aut/Au Ce*+/Ce³+ MnO₂ ,H+/Mn²+,H₂O Cl₂/cl Cr₂O,²,H+/Cr³+,H₂O O₂, H*/H₂O Br₂/Br NO,,H+/NO,H₂O Ag+/Ag Fe³+/Fe²+ 1₂2/1 O2, H₂O/OH Cu²+/Cu AgCl/Ag,Cl- H+/H₂ Fe³+/Fe O₂, H₂O/HO₂ ,OH™ Pb²+/Pb Sn²+ /Sn Fe²+/Fe Zn²+/Zn H₂O/H₂,OH™ Al³+ /Al Mg²+/Mg Nat/Na K+/K Lit/Li Reduced form is strongly reducing Reduction half-reaction F₂(g) +2 e Aut(aq) +e Ce¹+(aq) +e Ce³+ (aq) MnO, (aq) + 8 H+(aq) + 5 eMn²+ (aq) + 4 H₂O (1) Cl₂(g) + 2e →2 Cl(aq) Cr₂O7² (aq) + 14 H+ (aq) + 6 e2 Cr³+ (aq) + 7 H₂O(1) Oz(g)+4H*(aq)+4e —+2H,O(l) 2 F¯ (aq) Au(s) Br₂(1) + 2 e2 Br (aq) NO, (aq) + 4H+(aq) + 3 e Ag+ (aq) + e Fe³+ (aq) +e→→→ Fe²+ (aq) AgCl (s) + e 2 H (aq) + 2 e Fe³+ (aq) + 3 e NO(g) + 2 H₂O(1) Ag(s) Iz(s) + 2 e 2 (aq) O₂(g) + 2 H₂O(1) + 4e4 OH (aq) →→→ Cu(s) 2+ Cu²+ (aq) + 2 e Fe²+(aq) + 2 e Zn²+ (aq) + 2 e →→→ Ag(s) + Cl¯(aq) H₂(g) Fe(s) O₂(g) + H₂O(1) + 2 eHO₂ (aq) + OH¯ (aq) Pb²+(aq) + 2e →→→→ Pb(s) Sn²+ (aq) + 2e →→→→Sn(s) →→→→Fe(s) Zn(s) 2 H₂O(l) + 2 eH₂(g) + 2 OH(aq) Al³+ (aq) + 3 e- →→→→ Al(s) Mg²+ (aq) + 2 e→→→→→→ Mg(s) Na (aq) + e→→→→→→→ Na(s) K+(aq) +e →→→ K(s) Lit(aq) +eLi(s) +2.87 +1.69 +1.61 +1.51 Eº/V +1.36 +1.33 +1.23; +0.82 at pH = 7 +1.09 +0.96 +0.80 +0.77 +0.54 +0.40; +0.82 at pH = 7 +0.34 +0.22 0, by definition -0.04 -0.08 -0.13 -0.14 -0.44 -0.76 -0.83; -0.42 at pH = 7 -1.66 -2.36 -2.71 -2.93 -3.05