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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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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