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Electrolysis03:00

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In a galvanic cell, the electrical work is done by a redox system on its surroundings as electrons produced by the spontaneous redox reactions are transferred through an external circuit. Alternatively, an external circuit does work on a redox system by imposing a voltage sufficient to drive an otherwise nonspontaneous reaction in a process known as electrolysis. For instance, recharging a battery involves the use of an external power source to drive the spontaneous (discharge) cell reaction in...
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Electrodeposition is a technique used to separate an analyte from interferents by electrochemical processes. Here, the analyte is a metal ion that can be deposited on an electrode immersed in the sample solution. The electrochemical setup consists of an anode and a cathode. When an electric current is applied to the setup, oxidation occurs at the anode. At the cathode, which consists of a large metal surface, metal ions undergo reduction and deposit onto the surface.
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Potentiometry: Membrane Electrodes01:15

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Membrane electrodes, also known as p-ion electrodes, use membranes that selectively interact with free analyte ions, generating a potential difference across the membrane. The resulting membrane potential, known as the asymmetry potential, is not zero even when analyte concentrations on both sides of the membrane are equal. The membrane's response is typically not selective to a single analyte but proportional to the concentration of all ions in the sample solution capable of interacting at...
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Electrogravimetric Analysis: Overview01:30

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Electrogravimetric analysis measures the weight of an analyte deposited electrolytically onto a suitable working electrode. This method involves applying a potential to a pre-weighed electrode submerged in a solution, which results in the desired substance being deposited through reduction at the cathode or oxidation at the anode. The electrode's weight is recorded after deposition, and the difference in weight gives the analyte's weight in the solution.
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Controlled-potential coulometry, also known as potentiostatic coulometry, employs a three-electrode system in which the working electrode's potential is precisely regulated using a potentiostat. Platinum working electrodes are utilized for positive potentials, while mercury pool electrodes are favored for extremely negative potentials. The platinum counter electrode is separated from the analyte using a membrane or salt bridge to avoid interference in the analysis.
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Controlled-Current Coulometry: Overview01:27

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Controlled current coulometry, also known as amperostatic coulometry, is a technique used in electrochemical analysis to measure the quantity of a substance through the controlled passage of current. It involves the application of a constant current to an electrochemical cell containing the analyte of interest. As the current flows through the cell, the analyte undergoes a redox reaction at the electrode surface, resulting in a charge transfer. By monitoring the time required for a certain...
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Electrolyte Effects in Membrane-Electrode-Assembly CO Electrolysis.

Qiucheng Xu1,2, Bjørt Óladóttir Joensen1, Nishithan C Kani1

  • 1Surface Physics and Catalysis (SurfCat) Section, Department of Physics, Technical University of Denmark, Kongens Lyngby, 2800 Kgs., Denmark.

Angewandte Chemie (International Ed. in English)
|March 19, 2025
PubMed
Summary
This summary is machine-generated.

Membrane-electrode-assembly (MEA)-based carbon monoxide electrolysis (COE) can produce valuable C2+ products. This study shows moderate pH electrolytes, like potassium carbonate, yield high ethanol and propanol yields, outperforming highly alkaline conditions.

Keywords:
Anodic oxidationCO electrolysisElectrocatalysisElectrolyte effectMembrane‐electrode assembly

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Area of Science:

  • Electrochemistry
  • Catalysis
  • Sustainable Chemistry

Background:

  • Membrane-electrode-assembly (MEA)-based carbon monoxide electrolysis (COE) shows promise for producing C2+ products.
  • High performance in COE is typically achieved under strongly alkaline conditions (pH ≥ 14).
  • The necessity of extreme pH for optimal COE performance remains an open question.

Purpose of the Study:

  • To investigate the effect of different electrolytes (potassium bicarbonate, potassium carbonate, potassium hydroxide) on MEA-based COE performance.
  • To understand the influence of pH and anodic oxidation on the selectivity of liquid products.
  • To identify optimal conditions for producing ethanol and propanol via COE.

Main Methods:

  • MEA-based CO electrolysis was performed using various electrolytes (KHCO3, K2CO3, KOH).
  • Electrolyte concentration and pH were adjusted to study their effects on product selectivity.
  • Durability tests were conducted to assess the stability of the system.

Main Results:

  • Significant partial current densities for ethanol (189 ± 5 mA cm⁻²) and propanol (89 ± 4 mA cm⁻²) were achieved using 0.5 M K2CO3.
  • Moderate pH conditions in K2CO3 electrolytes favored high yields of ethanol and propanol.
  • Anodic oxidation was identified as detrimental to MEA-based COE performance for C2+ production.

Conclusions:

  • Optimal MEA-based COE performance, particularly for ethanol and propanol, can be achieved under moderate alkaline conditions (e.g., 0.5 M K2CO3).
  • A moderate local alkaline environment and resistance to anodic oxidation are key factors for high selectivity.
  • Minimizing anodic oxidation is crucial for enhancing durability and efficiency in MEA-based COE for valuable product synthesis.