Electrochemical production of hydrogen

The two electrodes must be electrically connected to each other, allowing for a flow of electrons that leave the metal of the anode and flow through this connection to the ions at the surface of the cathode. For example, the oxidizable substance e. Such tabulations are referenced to the standard hydrogen electrode SHE.

Anderson, and Thomas Kinney of Lynntech, Inc. In turn, the molecular iodine and the sodium hydroxide can be reacted together to regenerate sodium iodide, which can be recycled through the cell or otherwise be used in another electrolysis reaction.

Moving on to stepFIG. Water splitting Many technologies have been explored but it should be noted that as of "Thermal, thermochemical, biochemical and photochemical processes have so far not found industrial applications.

With the objective of reducing the cost of hydrogen production, renewable sources of energy have been targeted to allow electrolysis. In order to obtain hydrogen for use in such applications, hydrogen can be produced through an assortment of techniques, including through the electrolysis of water, the reaction of a metal with an acid, the steam reformation of natural gas, the partial oxidation of hydrocarbons, and through several other methods.

However, peroxides under alkaline conditions show poor stabilities and are not useful in disinfection applications. To provide a better understanding of the described systems and methods, the electrochemical cell is described below in more detail.

Steam reforming There are four main sources for the commercial production of hydrogen: The electrochemical cell of claim 1wherein the oxidizable substance is selected from an halide ion, a chalcogenide ion, a manganese oxide ion, and an aluminum oxide ion.

In addition to the aforementioned components and characteristics, the described cell 10 can comprise any other suitable component or characteristic.

The electrochemical cell of claim 1wherein the anolyte comprises an alkali metal salt of the oxidizable substance. This can deliver benefits for an oil refinery because it is more efficient than separate hydrogensteam and power plants. Also sodium hypoiodite decomposition is dependant on temperature.

In this regard, some examples of suitable cathode materials include, without limitation, nickel, stainless steel, graphite, a nickel-cobalt-ferrous alloy e.

The electrochemical cell of claim 14wherein the regeneration cell comprises a metal-oxide catalyst to facilitate the reaction of molecular iodine and the alkali hydroxide to form the alkali metal iodide. Some examples of suitable oxidizable substances include, but are not limited to, an iodide ion, a sulfide ion, a manganese oxide ion, an aluminum oxide ion, and any other suitable oxidizable substance that has an oxidation potential that is higher than that of oxygen evolution from water.

For instance, in some instances, the overall cell voltage for the oxidation and reduction of traditional water electrolysis is about 1.

It is used to calculate the maximum possible electrical energy that could be obtained from a chemical reaction. Said differently, the anolyte can comprise any suitable oxidizable substance that allows the open circuit cell voltage for the production of hydrogen to be less than a voltage selected from about 1.

The electrochemical cell of claim 1wherein the anolyte comprises a material selected from a non-aqueous solvent and a solid-state conductive additive.

The catalyst mix containing a diquaternary ammonium compound enabled not only higher concentration of hydrogen peroxide but also higher current efficiency, improved energy efficiency, and catalyst stability.

In some embodiments in which the anolyte 20 comprises an aqueous solution, the anode 25 comprises a dimensionally stable anode, which may include, but is not limited to, a rhenium dioxide and titanium dioxide on a titanium substrate, and a rhenium dioxide and tantalum pentoxide on a titanium substrate.

To provide a better understanding of the manner in which the cell may function, FIGS. The downside to this process is that its major byproducts are CO, CO2 and other greenhouse gases. In addition to the oxidizable substance, the anolyte can also comprise any other suitable material.

With respect to the alkali cation selective membrane, the membrane can comprise virtually any suitable alkali cation selective membrane.

In between these electrodes is the electrolytewhich contains ions that can freely move. The electrochemical cell of claim 1wherein the oxidizable substance is alkali metal iodide, the oxidized product is molecular iodine, and the reduced product is alkali hydroxide.

The hydrogen evolution reaction (HER, 2 H + + 2 e − → H 2) is at the center of electrochemical water splitting. It is a classic example of a two-electron transfer reaction with one catalytic intermediate and offers the potential to free up H 2.

Hydrogen can be produced using a number of different processes. Thermochemical processes use heat and chemical reactions to release hydrogen from organic materials such as fossil fuels and biomass.

Water (H 2 O) can be split into hydrogen (H 2) and oxygen (O 2) using electrolysis or solar energy.

US9297084B2 - Electrochemical production of hydrogen - Google Patents

Hydrogen Electrochemical Production presents different avenues of hydrogen production for energy applications, including current developments and future perspectives, using an interdisciplinary approach. Small-scale decentralized electrochemical production of H 2 O 2 via a two-electron Electrochemical production of H 2 O 2 through ORR with cheap, stable, and earth abundant carbon catalysts provides a clean and sustainable way to replace the current energy-intensive industrial anthraquinone process.

Electrochemical Oxygen Reduction for the Production of Hydrogen Peroxide Previous Article A Crystal with Nearly % of Its Body Weight in Water Next Article 2D Spectroscopy Helps Visualize the Influence of Spectral Motion on Chromophore Response.

Once separated, hydrogen can be used along with oxygen from the air in a fuel cell to create electricity through an electrochemical process.


Production Hydrogen can be produced from diverse, domestic resources including fossil fuels, biomass, and water electrolysis with electricity.

Electrochemical production of hydrogen
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Hydrogen production - Wikipedia