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Assembly of a Cost-Effective Anode Using Palladium Nanoparticles for Alkaline Fuel Cell Applications.

Feliciano-Ramos I, Casañas-Montes B, García-Maldonado MM, Menéndez CL, Mayol AR, Díaz-Vázquez LM, Cabrera CR - J Chem Educ (2015)

Bottom Line: In this laboratory experiment, the student selects a cost-effective anode for fuel cells by comparing three different working electrodes.The GC and CP were modified with palladium nanoparticles (PdNP) suspensions.With this activity, fundamental electrochemical concepts were reinforced.

View Article: PubMed Central - PubMed

Affiliation: Department of Chemistry and Center for Advanced Nanoscale Materials, University of Puerto Rico , Río Piedras Campus, P.O. Box 23346, San Juan, Puerto Rico 00931-3346, United States.

ABSTRACT

Nanotechnology allows the synthesis of nanoscale catalysts, which offer an efficient alternative for fuel cell applications. In this laboratory experiment, the student selects a cost-effective anode for fuel cells by comparing three different working electrodes. These are commercially available palladium (Pd) and glassy carbon (GC) electrodes, and a carbon paste (CP) electrode that is prepared by the students in the laboratory. The GC and CP were modified with palladium nanoparticles (PdNP) suspensions. The electrodes efficiencies were studied for ethanol oxidation in alkaline solution using cyclic voltammetry techniques. The ethanol oxidation currents obtained were used to determine the current density using the geometric and surface area of each electrode. Finally, students were able to choose the best electrode and relate catalytic activity to surface area for ethanol oxidation in alkaline solution by completing a critical analysis of the cyclic voltammetry results. With this activity, fundamental electrochemical concepts were reinforced.

No MeSH data available.


Cyclicvoltammogram of CP/PdNP (solid line), GC/PdNP (dashed line),and Pd (dotted line) electrodes in 1.0 M ethanol and 1.0 M KOH solution.
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fig3: Cyclicvoltammogram of CP/PdNP (solid line), GC/PdNP (dashed line),and Pd (dotted line) electrodes in 1.0 M ethanol and 1.0 M KOH solution.

Mentions: Figure 3 shows cyclicvoltammograms of theethanol oxidation using an alkaline medium, i.e., 1.0 M ethanol and1.0 M KOH. Students observed two peaks: the first peak appears inthe potential region from −0.50 to 0.00 V vs Ag/AgCl duringthe forward scan (positive direction). At positive potentials, theformation of PdO blocks the catalytic activity for ethanol oxidation.12−14 In the reverse scan (negative direction), PdO is reduced to metallicpalladium starting at −0.30 V, returning the ethanol oxidationcatalysis, and showing an anodic peak again. Students observed thissecond peak in the region between −0.30 and −0.60 Vvs Ag/AgCl in 1.0 M ethanol and 1.0 M KOH solution. This voltammetryexperiment showed that both peaks are anodic, a typical ethanol oxidationbehavior in alkaline conditions. We are not showing reduction peaks.


Assembly of a Cost-Effective Anode Using Palladium Nanoparticles for Alkaline Fuel Cell Applications.

Feliciano-Ramos I, Casañas-Montes B, García-Maldonado MM, Menéndez CL, Mayol AR, Díaz-Vázquez LM, Cabrera CR - J Chem Educ (2015)

Cyclicvoltammogram of CP/PdNP (solid line), GC/PdNP (dashed line),and Pd (dotted line) electrodes in 1.0 M ethanol and 1.0 M KOH solution.
© Copyright Policy
Related In: Results  -  Collection

License
Show All Figures
getmorefigures.php?uid=PMC4325606&req=5

fig3: Cyclicvoltammogram of CP/PdNP (solid line), GC/PdNP (dashed line),and Pd (dotted line) electrodes in 1.0 M ethanol and 1.0 M KOH solution.
Mentions: Figure 3 shows cyclicvoltammograms of theethanol oxidation using an alkaline medium, i.e., 1.0 M ethanol and1.0 M KOH. Students observed two peaks: the first peak appears inthe potential region from −0.50 to 0.00 V vs Ag/AgCl duringthe forward scan (positive direction). At positive potentials, theformation of PdO blocks the catalytic activity for ethanol oxidation.12−14 In the reverse scan (negative direction), PdO is reduced to metallicpalladium starting at −0.30 V, returning the ethanol oxidationcatalysis, and showing an anodic peak again. Students observed thissecond peak in the region between −0.30 and −0.60 Vvs Ag/AgCl in 1.0 M ethanol and 1.0 M KOH solution. This voltammetryexperiment showed that both peaks are anodic, a typical ethanol oxidationbehavior in alkaline conditions. We are not showing reduction peaks.

Bottom Line: In this laboratory experiment, the student selects a cost-effective anode for fuel cells by comparing three different working electrodes.The GC and CP were modified with palladium nanoparticles (PdNP) suspensions.With this activity, fundamental electrochemical concepts were reinforced.

View Article: PubMed Central - PubMed

Affiliation: Department of Chemistry and Center for Advanced Nanoscale Materials, University of Puerto Rico , Río Piedras Campus, P.O. Box 23346, San Juan, Puerto Rico 00931-3346, United States.

ABSTRACT

Nanotechnology allows the synthesis of nanoscale catalysts, which offer an efficient alternative for fuel cell applications. In this laboratory experiment, the student selects a cost-effective anode for fuel cells by comparing three different working electrodes. These are commercially available palladium (Pd) and glassy carbon (GC) electrodes, and a carbon paste (CP) electrode that is prepared by the students in the laboratory. The GC and CP were modified with palladium nanoparticles (PdNP) suspensions. The electrodes efficiencies were studied for ethanol oxidation in alkaline solution using cyclic voltammetry techniques. The ethanol oxidation currents obtained were used to determine the current density using the geometric and surface area of each electrode. Finally, students were able to choose the best electrode and relate catalytic activity to surface area for ethanol oxidation in alkaline solution by completing a critical analysis of the cyclic voltammetry results. With this activity, fundamental electrochemical concepts were reinforced.

No MeSH data available.