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Use standard reduction potentials to find the equilibrium constant for the following reaction at 25 "C. Round your answer to 2 significant digits. 0₂(g) + 411¹(ag) 4Fe²(aq)21.0(-4Fe (ag) Note: Reference the Standard reduction potentials at 25 C table for additional information. TABLE 19.1 Standard Reduction Potentials at 25°C* Half-Reaction E°(V)

Use standard reduction potentials to find the equilibrium constant for the following reaction at 25 "C. Round your answer to 2 significant digits. 0₂(g) + 411¹(ag) 4Fe²(aq)21.0(-4Fe (ag) Note: Reference the Standard reduction potentials at 25 C table for additional information. TABLE 19.1 Standard Reduction Potentials at 25°C* Half-Reaction E°(V)

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Use standard reduction potentials to find the equilibrium constant for the following reaction at 25 °C. Round your answer to 2 significant digits. O₂(g) + 411' (aq) 4Fe(aq)211,0(+4Fe³+ (aq) Note: Reference the Standard reduction potentials at 25 C table for additional information. K 0.P Increasing strength as oxidizing agent X TABLE 19.1 Standard Reduction Potentials at 25°C* Half-Reaction F₂(g) + 2e2F (aq) O,(g) + 2H*(aq) + 2eO₂(g) + H₂O Cot(aq) +ẻ — Cot(aq) H₂O₂(aq) + 2H(aq) + 2e2H₂O PbO₂(s) + 4H(aq) + SO (aq) + 2e PbSO4(s) + 2H₂O Ce+ (aq) + e Ce³(aq) MnO4 (aq) + 8H(aq) + 5e Mn²+ (aq) + 4H₂O Au³+ (aq) + 3e →→→ Au(s) Cl₂(g) + 2e →→→ 2CT (aq) Cr₂O (aq) + 14H*(aq) + 6e2Cr³+ (aq) + 7H₂O Mn² (aq) + 2H₂O MnO₂(s) + 4H(aq) + 2e O₂(g) + 4H (aq) + 4e →→→ 2H₂O Br₂(l) + 2e →2Br (aq) NO3(aq) + 4H* (aq) + 3e¯ 2Hg²+ (aq) + 2e Hg (aq) + 2e Ag (aq) + e- Ag(s) Fe (aq) →→→ Fe²+ (aq) O₂(g) + 2H(aq) + 2e- MnO4 (aq) + 2H₂O + 3e 1₂(s) + 2e21 (aq) O₂(g) + 2H₂O + 4e →→→40H(aq) Cu²+ (aq) + 2e →→→ Cu(s) - Hg2+ (aq) Be²+ (aq) + 2e Mg²+ (aq) + 2e 2Hg(1) H₂(g) Pb(s) AgCl(s) +eAg(s) + Cl(aq) Cu (aq) → Sn²+ (aq) SO (aq) + 4H* (aq) + 2e SO₂(g) + 2H₂O Cu²+ (aq) + e Sn (aq) + 2e7 2H*(aq) + 2e Pb²+ (aq) + 2e Sn²+ (aq) + 2e Ni²+ (aq) + 2e 2+ Co²+ (aq) + 2e - Co(s) PbSO4(s) + 2e Cd²+ (aq) + 2e Fe2+ (aq) + 2e7 Cr³+ (aq) + 3e Zn²+ (aq) + 2e 2H₂O + 2e Mn²+ (aq) + 2e AP+ (aq) + 3e →→→Sn(s) -Ni(s) - Cd(s) -> Fe(s) -Cr(s) →→→ Zn(s) →→Pb(s) + SO (aq) -> Al(s) →→→ Be(s) H₂(g) + 2OH(aq) →Mn(s) Mg(s) Na (aq) + e - Na(s) Ca²+ (aq) + 2e -Ca(s) Sr² (aq) + 2e7 Ba²+ (aq) + 2e K'(aq) + e Lit (aq) + e → NO(g) + 2H₂O -Sr(s) →→Ba(s) H_O_aq) MnO₂(s) + 4OH(aq) → > K(s) → Li(s) E°(V) +2.87 +2.07 +1.82 +1.77 +1.70 +1.61 +1.51 +1.50 +1.36 +1.33 +1.23 +1.23 +1.07 +0.96 +0.92 +0.85 +0.80 +0.77 +0.68 +0.59 +0.53 +0.40 +0.34 +0.22 +0.20 +0.15 +0.13 = 0.00 -0.13 -0.14 -0.25 -0.28 -0.31 -0.40 -0.44 -0.74 -0.76 -0.83 -1.18 -1.66 -1.85 -2.37 -2.71 Increasing strength as reducing agent -2.87 -2.89 -2.90 -2.93 -3.05 *For all half-reactions the concentration is 1 M for dissolved species and the pressure is 1 atm for gases. These are the standard-state values.
Transcribed Image Text:Use standard reduction potentials to find the equilibrium constant for the following reaction at 25 °C. Round your answer to 2 significant digits. O₂(g) + 411' (aq) 4Fe(aq)211,0(+4Fe³+ (aq) Note: Reference the Standard reduction potentials at 25 C table for additional information. K 0.P Increasing strength as oxidizing agent X TABLE 19.1 Standard Reduction Potentials at 25°C* Half-Reaction F₂(g) + 2e2F (aq) O,(g) + 2H*(aq) + 2eO₂(g) + H₂O Cot(aq) +ẻ — Cot(aq) H₂O₂(aq) + 2H(aq) + 2e2H₂O PbO₂(s) + 4H(aq) + SO (aq) + 2e PbSO4(s) + 2H₂O Ce+ (aq) + e Ce³(aq) MnO4 (aq) + 8H(aq) + 5e Mn²+ (aq) + 4H₂O Au³+ (aq) + 3e →→→ Au(s) Cl₂(g) + 2e →→→ 2CT (aq) Cr₂O (aq) + 14H*(aq) + 6e2Cr³+ (aq) + 7H₂O Mn² (aq) + 2H₂O MnO₂(s) + 4H(aq) + 2e O₂(g) + 4H (aq) + 4e →→→ 2H₂O Br₂(l) + 2e →2Br (aq) NO3(aq) + 4H* (aq) + 3e¯ 2Hg²+ (aq) + 2e Hg (aq) + 2e Ag (aq) + e- Ag(s) Fe (aq) →→→ Fe²+ (aq) O₂(g) + 2H(aq) + 2e- MnO4 (aq) + 2H₂O + 3e 1₂(s) + 2e21 (aq) O₂(g) + 2H₂O + 4e →→→40H(aq) Cu²+ (aq) + 2e →→→ Cu(s) - Hg2+ (aq) Be²+ (aq) + 2e Mg²+ (aq) + 2e 2Hg(1) H₂(g) Pb(s) AgCl(s) +eAg(s) + Cl(aq) Cu (aq) → Sn²+ (aq) SO (aq) + 4H* (aq) + 2e SO₂(g) + 2H₂O Cu²+ (aq) + e Sn (aq) + 2e7 2H*(aq) + 2e Pb²+ (aq) + 2e Sn²+ (aq) + 2e Ni²+ (aq) + 2e 2+ Co²+ (aq) + 2e - Co(s) PbSO4(s) + 2e Cd²+ (aq) + 2e Fe2+ (aq) + 2e7 Cr³+ (aq) + 3e Zn²+ (aq) + 2e 2H₂O + 2e Mn²+ (aq) + 2e AP+ (aq) + 3e →→→Sn(s) -Ni(s) - Cd(s) -> Fe(s) -Cr(s) →→→ Zn(s) →→Pb(s) + SO (aq) -> Al(s) →→→ Be(s) H₂(g) + 2OH(aq) →Mn(s) Mg(s) Na (aq) + e - Na(s) Ca²+ (aq) + 2e -Ca(s) Sr² (aq) + 2e7 Ba²+ (aq) + 2e K'(aq) + e Lit (aq) + e → NO(g) + 2H₂O -Sr(s) →→Ba(s) H_O_aq) MnO₂(s) + 4OH(aq) → > K(s) → Li(s) E°(V) +2.87 +2.07 +1.82 +1.77 +1.70 +1.61 +1.51 +1.50 +1.36 +1.33 +1.23 +1.23 +1.07 +0.96 +0.92 +0.85 +0.80 +0.77 +0.68 +0.59 +0.53 +0.40 +0.34 +0.22 +0.20 +0.15 +0.13 = 0.00 -0.13 -0.14 -0.25 -0.28 -0.31 -0.40 -0.44 -0.74 -0.76 -0.83 -1.18 -1.66 -1.85 -2.37 -2.71 Increasing strength as reducing agent -2.87 -2.89 -2.90 -2.93 -3.05 *For all half-reactions the concentration is 1 M for dissolved species and the pressure is 1 atm for gases. These are the standard-state values.
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