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Calculate the corrosion rate Cr in units of mm/y, and the electrochemical rate in µg/cm2.s and mol/cm2s  for a low carbon steel plate (1cmx1cm) immersed in sea water. Given data I=110 µA (current), ρ=7.87  g/cm3 and Aw=55.85 g/mol. (F= 96500 A.s/mol)

Calculate the corrosion rate Cr in units of mm/y, and the electrochemical rate in µg/cm2.s and mol/cm2s  for a low carbon steel plate (1cmx1cm) immersed in sea water. Given data I=110 µA (current), ρ=7.87  g/cm3 and Aw=55.85 g/mol. (F= 96500 A.s/mol)

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.124QP: An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for...
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Calculate the corrosion rate Cr in units of mm/y, and the electrochemical rate in µg/cm2.s and mol/cm2s 
for a low carbon steel plate (1cmx1cm) immersed in sea water. Given data I=110 µA (current), ρ=7.87 
g/cm3 and Aw=55.85 g/mol. (F= 96500 A.s/mol)

 

Table 20.1 Standard reduction potentials at 25°C* Increasing strength as oxidizing agent Half-Reaction Li*(aq) + e K+ (aq) + e Ba²+ (aq) + 2e Sr+ (aq) + 2e7 Ca²+ (aq) + 2e Na (aq) + e - Mg²+ (aq) + 2e- Be²+ (aq) + 2e Al³+ (aq) + 3e Mn²+ (aq) + 2e 2H₂O +2e Zn²+ (aq) + 2e™ Cr³+ (aq) + 3e Fe²+ (aq) + 2e Cd²+ (aq) + 2e PbSO₂ (s) + 2e™ Co²+ (aq) + 2e Ni²+ (aq) + 2e Sn²+ (aq) + 2e- Pb²+ (aq) + 2e 2H(aq) + 2e Sn¹+ (aq) + 2e - Li(s) K(s) - Ba(s) Sr(s) Mg(s) Be(s) →Al(s) →→→ Ca(s) - Na(s) →→→ Mn(s) - H₂(g) + 2OH(aq) Zn(s) Cr(s) Fe(s) Cd(s) Pb(s) + SO (aq) → Co(s) Ni(s) Sn(s) Pb(s) H₂(g) Sn²+ (aq) Cu²+ (aq) + e - Cu*(aq) SO (aq) + 4H*(aq) + 2e SO₂(g) + 2H₂O AgCl(s) + e - Ag(s) + Cl(aq) Cu²+ (aq) + 2e →→ Cu(s) O₂(g) + 2H₂O + 4e¯ - 40H (aq) [₂(s) + 2e →→→ 21 (aq) MnO, (aq) + 2H₂O + 3e7 - MnO₂ (s) + 4OH(aq) O₂(g) + 2H*(aq) + 2e →→→→ HyO,(aq) Fe²+ (aq) Fe³+ (aq) + e- Ag (aq) + e Hg(aq) + 2e Ag(s) 2Hg²+ (aq) + 2e 2Hg(/) - NO3(aq) + 4H+ (aq) + 3e →→→→ NO(g) + 2H₂O 2Br (aq) Hg+ (aq) Br₂() +2e7 O₂(g) + 4H(aq) + 4e¯→→→→→→ 2H₂O MnO₂ (s) + 4H*(aq) + 2e Mn²+ (aq) + 2H₂O Cr₂O² (aq) + 4H*(aq) + 6e¯→→→→→ 2Cr²³¹+ (aq) + 7H₂O Cl₂(g) + 2e2C1 (aq) Au³+ (aq) + 3e →→→ Au(s) MnO, (aq) + 8H(aq) + Se→→→→→→ Mn²+ (aq) + 4H₂O Ce+ (aq) + e Ce³+ (aq) PbO₂ (s) + 4H*(aq) + SO² (aq) + 2e 2H₂O H₂O₂(aq) + 2H+ (aq) + 2e →→→→ Co¹³+ (aq) + e cơ (ag) PbSO₂ (s) + 2H₂O 8°(V) -3.05. -2.93 -2.90 -2.89 -2.87 -2.71 -2.37 -1.85 -1.66 -1.18 -0.83 -0.76 -0.74 -0.44 -0.40 -0.31 -0.28 -0.25 -0.14 -0.13 0.00 +0.13 +0.15 +0.20 +0.22 +0.34 +0.40 +0.53 +0.59 +0.68 +0.77 +0.80 +0.85 +0.92 +0.96 +1.07 +1.23 +1.23 +1.33 +1.36 +1.50 +1.51 +1.61 +1.70 +1.77 +1.82 +2.07 +2.87 Increasing strength as reducing agent O(g) + 2H(aq) + 2e → O₂(g) + H₂O(l) F₂(g) + 2e →→→→ 2F (aq) *For all half reactions the concentration is 1 M for dissolved species and the pressure is I atm for gases.
Transcribed Image Text:Table 20.1 Standard reduction potentials at 25°C* Increasing strength as oxidizing agent Half-Reaction Li*(aq) + e K+ (aq) + e Ba²+ (aq) + 2e Sr+ (aq) + 2e7 Ca²+ (aq) + 2e Na (aq) + e - Mg²+ (aq) + 2e- Be²+ (aq) + 2e Al³+ (aq) + 3e Mn²+ (aq) + 2e 2H₂O +2e Zn²+ (aq) + 2e™ Cr³+ (aq) + 3e Fe²+ (aq) + 2e Cd²+ (aq) + 2e PbSO₂ (s) + 2e™ Co²+ (aq) + 2e Ni²+ (aq) + 2e Sn²+ (aq) + 2e- Pb²+ (aq) + 2e 2H(aq) + 2e Sn¹+ (aq) + 2e - Li(s) K(s) - Ba(s) Sr(s) Mg(s) Be(s) →Al(s) →→→ Ca(s) - Na(s) →→→ Mn(s) - H₂(g) + 2OH(aq) Zn(s) Cr(s) Fe(s) Cd(s) Pb(s) + SO (aq) → Co(s) Ni(s) Sn(s) Pb(s) H₂(g) Sn²+ (aq) Cu²+ (aq) + e - Cu*(aq) SO (aq) + 4H*(aq) + 2e SO₂(g) + 2H₂O AgCl(s) + e - Ag(s) + Cl(aq) Cu²+ (aq) + 2e →→ Cu(s) O₂(g) + 2H₂O + 4e¯ - 40H (aq) [₂(s) + 2e →→→ 21 (aq) MnO, (aq) + 2H₂O + 3e7 - MnO₂ (s) + 4OH(aq) O₂(g) + 2H*(aq) + 2e →→→→ HyO,(aq) Fe²+ (aq) Fe³+ (aq) + e- Ag (aq) + e Hg(aq) + 2e Ag(s) 2Hg²+ (aq) + 2e 2Hg(/) - NO3(aq) + 4H+ (aq) + 3e →→→→ NO(g) + 2H₂O 2Br (aq) Hg+ (aq) Br₂() +2e7 O₂(g) + 4H(aq) + 4e¯→→→→→→ 2H₂O MnO₂ (s) + 4H*(aq) + 2e Mn²+ (aq) + 2H₂O Cr₂O² (aq) + 4H*(aq) + 6e¯→→→→→ 2Cr²³¹+ (aq) + 7H₂O Cl₂(g) + 2e2C1 (aq) Au³+ (aq) + 3e →→→ Au(s) MnO, (aq) + 8H(aq) + Se→→→→→→ Mn²+ (aq) + 4H₂O Ce+ (aq) + e Ce³+ (aq) PbO₂ (s) + 4H*(aq) + SO² (aq) + 2e 2H₂O H₂O₂(aq) + 2H+ (aq) + 2e →→→→ Co¹³+ (aq) + e cơ (ag) PbSO₂ (s) + 2H₂O 8°(V) -3.05. -2.93 -2.90 -2.89 -2.87 -2.71 -2.37 -1.85 -1.66 -1.18 -0.83 -0.76 -0.74 -0.44 -0.40 -0.31 -0.28 -0.25 -0.14 -0.13 0.00 +0.13 +0.15 +0.20 +0.22 +0.34 +0.40 +0.53 +0.59 +0.68 +0.77 +0.80 +0.85 +0.92 +0.96 +1.07 +1.23 +1.23 +1.33 +1.36 +1.50 +1.51 +1.61 +1.70 +1.77 +1.82 +2.07 +2.87 Increasing strength as reducing agent O(g) + 2H(aq) + 2e → O₂(g) + H₂O(l) F₂(g) + 2e →→→→ 2F (aq) *For all half reactions the concentration is 1 M for dissolved species and the pressure is I atm for gases.
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