Fabrication of cerium-doped lead dioxide anode with improved electrocatalytic activity and its application for removal of Rhodamine B

2013 ◽  
Vol 228 ◽  
pp. 806-814 ◽  
Author(s):  
Qin Li ◽  
Qiu Zhang ◽  
Hao Cui ◽  
Liang Ding ◽  
Zhongbo Wei ◽  
...  
Keyword(s):  
Rhodamine B ◽  
Electrocatalytic Activity ◽  
Lead Dioxide ◽  
Lead Dioxide Anode

The Lead Dioxide Anode. II. The Kinetics and Participation of the Lead Dioxide Electrode in Electrochemical Oxidation Reactions in Sulfuric Acid

1989 ◽  
Vol 42 (9) ◽  
pp. 1527 ◽  
Author(s):  
TH Randle ◽  
AT Kuhn
Keyword(s):  
Sulfuric Acid ◽  
Electrochemical Oxidation ◽  
Maximum Rate ◽  
Lead Dioxide ◽  
Chemical Oxidation ◽  
Oxidation Reactions ◽  
Electrochemical Regeneration ◽  
Electrode Surfaces ◽  
Lead Dioxide Electrode ◽  
Lead Dioxide Anode

Lead dioxide is a strong oxidizer in sulfuric acid, consequently electrochemical oxidation of solution species at a lead dioxide anode may occur by a two-step, C-E process (chemical oxidation of solution species by PbO2 followed by electrochemical regeneration of the reduced lead dioxide surface). The maximum rate of each step has been determined in sulfuric acid for specified lead dioxide surfaces and compared with the rates observed for the electrochemical oxidation of cerium(III) and manganese(II) on the same electrode surfaces. While the rate of electrochemical oxidation of a partially reduced PbO2 surface may be sufficient to support the observed rates of CeIII and MnII oxidation at the lead dioxide anode, the rate of chemical reaction between PbO2 and the reducing species is not. Hence it is concluded that the lead dioxide electrode functions as a simple, 'inert' electron-transfer agent during the electrochemical oxidation of CellI and MnII in sulfuric acid. In general, it will most probably be the rate of the chemical step which determines the feasibility or otherwise of the C-E mechanism.

Lead Dioxide Anode for Commercial Use

1958 ◽  
Vol 105 (2) ◽  
pp. 100 ◽  
Author(s):  
J. C. Grigger ◽  
H. C. Miller ◽  
F. D. Loomis
Keyword(s):  
Lead Dioxide ◽  
Commercial Use ◽  
Lead Dioxide Anode

An unusual 32-membered copper(ii) metallomacrocube based on a Cu4O3X cubic core: photocatalytic, electrocatalytic, and magnetic properties

2016 ◽  
Vol 52 (23) ◽  
pp. 4294-4297 ◽  
Author(s):  
Sisi Feng ◽  
Fei Jia ◽  
Liping Lu ◽  
Zhongping Li ◽  
Shuo Zhang
Keyword(s):  
Magnetic Properties ◽  
Rhodamine B ◽  
Electrocatalytic Activity ◽  
Organic Pollutant ◽  
Catalytic Performance ◽  
Nitrite Reduction ◽  
Good Electrocatalytic Activity ◽  
Excellent Catalytic Performance

The first Cu32 cluster featuring a multi-cubane (Cu4O3X) structure exhibited excellent catalytic performance in the degradation of organic pollutant rhodamine B, good electrocatalytic activity for nitrite reduction, and strong antiferromagnetic interactions.

The Lead Dioxide Anode. I. A Kinetic Study of the Electrolytic Oxidation of Cerium(III) and Manganese(II) in Sulfuric Acid at the Lead Dioxide Electrode

1989 ◽  
Vol 42 (2) ◽  
pp. 229 ◽  
Author(s):  
TH Randle ◽  
AT Kuhn
Keyword(s):  
Sulfuric Acid ◽  
Platinum Electrode ◽  
Lead Dioxide ◽  
Chemical Oxidation ◽  
Oxidation Reactions ◽  
Heterogeneous Chemical ◽  
Lead Dioxide Anode ◽  
Direct Support ◽  
Electrolytic Oxidation ◽  
Step Mechanism

The electrolytic oxidation reactions of cerium(III) and manganeseII) in sulfuric acid have been used as probes to investigate the mechanism of the lead dioxide anode. The kinetics observed for such reactions at the lead dioxide surface provide no direct support for the proposal that the lead dioxide anode functions by a sequential 'two-step' mechanism (heterogeneous chemical oxidation of solution species followed by electrochemical oxidation of the reduced lead dioxide surface); rather the kinetics show characteristics similar to those observed previously for the oxidation of cerium(III) and manganese(II) at the platinum electrode, suggesting that the lead dioxide surface functions as a simple, 'inert' electron-transfer agent.

Anodic Synthesis of α-PbO2-CeO2-TiO2 Composite Materials from Colloidal Electrolyte: Morphology, Composition and Structure of PbO2-Matrix Composites

2011 ◽  
Vol 308-310 ◽  
pp. 728-733
Author(s):  
Bu Ming Chen ◽  
Zhong Cheng Guo ◽  
Hui Huang
Keyword(s):  
Electrocatalytic Activity ◽  
Fine Particles ◽  
Surface Composition ◽  
Lead Dioxide ◽  
Solid Particles ◽  
Matrix Composites ◽  
Pure Lead ◽  
Surface Areas ◽  
The Matrix ◽  
Unit Cells

During electrodepositing pure lead dioxide, the electrocatalytic activity of PbO2 electrodes, as well as their stability, can often be considerably enhanced by the incorporation of some fine particles added to the electrodeposition. The morphology, crystal phase, surface composition, microstructure, of the electrode were characterized by means of SEM, XRD and EDS. SEM-EDS analysis showed the addition of solid particles could inhibit the growth of α-PbO2 unit cells, improving the specific surface areas of coating surface.Under all condition, the matrix was highly oriented α-PbO2. The electrocatalytic activity of the prepared materials has been tested in Zn2+ 50g L-1, H2SO4 150g L-1 solution. It showed that the electrocatalytic activity of the A1/conductive coating/α-PbO2-3.71 wt.% TiO2-2.12 wt.% CeO2 anode is the best.

Oxygen overpotential of graphite-substrate lead dioxide anode

1965 ◽  
Vol 10 (12) ◽  
pp. 1185-1187 ◽  
Author(s):  
M.S.V. Pathy ◽  
H.V.K. Udupa
Keyword(s):  
Lead Dioxide ◽  
Graphite Substrate ◽  
Lead Dioxide Anode

The effect of Cobalt on the Kinetics of Oxygen evolution at a Lead Dioxide anode in Sulphuric Acid

1959 ◽  
Vol 12 (2) ◽  
pp. 127 ◽  
Author(s):  
DFA Koch
Keyword(s):  
Sulphuric Acid ◽  
Oxygen Evolution ◽  
Current Density ◽  
Lead Dioxide ◽  
Kinetic Constants ◽  
Kcal Mole ◽  
Lead Dioxide Anode ◽  
Kinetics Of ◽  
Evolution Of Oxygen ◽  
Rate Determining Steps

The overpotential (n)-log current density (log i) curves for the evolution of oxygen at a lead dioxide anode in 2N H2SO4 both in the absence and presence of cobaltous sulphate in solution have been used to determine the electrode kinetic constants α ; i0 for a series of temperatures and also ΔH0*:. At 25 �C in the absence of cobalt α=O.59, i0= 10-11, and ΔH0*= 15 kcal mole-1 When 13 mg/l cobaltous sulphate is added α= 1.0, i0= 10-15, and ΔH0*:=29 kcal mole-1. Possible mechanisms for the reaction are discussed on the basis of these values and the rate determining steps suggested (where M represents the PbO2 surface) are M +H2O =MOH +H+ +e in the absence of cobalt and 2CoOH++ = 2Co++ +H2O + O in its presence.

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