Name a device used for electrolysis of water?

  1.  it may be but electrode is used as this work
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Brownlee Electrolsis Apparatus used for electrolysis of water.

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Electrolysis of water

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Simple setup for demonstration of electrolysis of water at home

Electrolysis of water is the decomposition of water (H2O) into oxygen (O2) and hydrogen gas (H2) due to anelectric current being passed through the water.

Principle

An electrical power source is connected to two electrodes, or two plates (typically made from some inert metal such as platinum or stainless steel) which are placed in the water. Hydrogen will appear at the cathode (the negatively charged electrode, where electrons enter the water), and oxygen will appear at theanode (the positively charged electrode). Assuming ideal faradaic efficiency, the amount of hydrogen generated is twice the number of moles of oxygen, and both are proportional to the total electrical charge conducted by the solution. However, in many cells competing side reactions dominate, resulting in different products and less than ideal faradaic efficiency.

Electrolysis of pure water requires excess energy in the form of overpotential to overcome various activation barriers. Without the excess energy the electrolysis of pure water occurs very slowly or not at all. This is in part due to the limited self-ionization of water. Pure water has an electrical conductivityabout one millionth that of seawater. Many electrolytic cells may also lack the requisite electrocatalysts. The efficiency of electrolysis is increased through the addition of an electrolyte (such as a salt, an acid or a base) and the use of electrocatalysts.

Currently the electrolytic process is rarely used in industrial applications since hydrogen can currently be produced more affordably from fossil fuels.

History

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Device invented by Johann Wilhelm Ritter to develop the electrolysis of water

Jan Rudolph Deiman and Adriaan Paets van Troostwijk used in 1789 an electrostatic machine to produce electricity which was discharged on gold electrodes in a Leyden jar with water. In 1800 Alessandro Volta invented the voltaic pile, and a few weeks later William Nicholson and Anthony Carlisle used it for the electrolysis of water. When Zénobe Gramme invented the Gramme machine in 1869 electrolysis of water became a cheap method for the production of hydrogen. A method of industrial synthesis of hydrogen and oxygen through electrolysis was developed by Dmitry Lachinov in 1888.

Equations

In pure water at the negatively charged cathode, a reduction reaction takes place, with electrons (e) from the cathode being given to hydrogen cations to form hydrogen gas (the half reaction balanced with acid):

Reduction at cathode: 2 H+(aq) + 2e → H2(g)

At the positively charged anode, an oxidation reaction occurs, generating oxygen gas and giving electrons to the anode to complete the circuit:

Anode (oxidation): 2 H2O(l) → O2(g) + 4 H+(aq) + 4e

The same half reactions can also be balanced with base as listed below. Not all half reactions must be balanced with acid or base. Many do, like the oxidation or reduction of water listed here. To add half reactions they must both be balanced with either acid or base.

Cathode (reduction): 2 H2O(l) + 2e → H2(g) + 2 OH-(aq)

Anode (oxidation): 4 OH- (aq) → O2(g) + 2 H2O(l) + 4 e

Combining either half reaction pair yields the same overall decomposition of water into oxygen and hydrogen:

Overall reaction: 2 H2O(l) → 2 H2(g) + O2(g)

The number of hydrogen molecules produced is thus twice the number of oxygen molecules. Assuming equal temperature and pressure for both gases, the produced hydrogen gas has therefore twice the volume of the produced oxygen gas. The number of electrons pushed through the water is twice the number of generated hydrogen molecules and four times the number of generated oxygen molecules.

Thermodynamics of the process

Decomposition of pure water into hydrogen and oxygen at standard temperature and pressure is not favorable in thermodynamic terms.

Anode (oxidation): 2 H2O(l) → O2(g) + 4 H+(aq) + 4e Eo
ox = -1.23 V (Eo
red = 1.23 )[4])

Cathode (reduction): 2 H+(aq) + 2e → H2(g)  Eo
red = 0.00 V

Thus, the standard potential of the water electrolysis cell is -1.23 V at 25 °C at pH 0 (H+ = 1.0 M). The potential is changed to -0.82 V at 25 °C at pH 7 (H+ = 1.0×10−7 M) based on the Nernst Equation. However, electrolysis will not generally proceed at these voltages, as the electrical input must provide the full amount of enthalpy of the H2-O2 products (286 kJ per mol). This takes the theoretical and real observed threshold of electrolysis to (-)1.48 V.

The negative voltage indicates the Gibbs free energy for electrolysis of water is greater than zero for these reactions. This can be found using the G = -nFEequation from chemical kinetics, where n is the moles of electrons and F is the Faraday constant. The reaction cannot occur without adding necessary energy, usually supplied by an external electrical power source.

Electrolyte selection

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Hoffman voltameter connected to adirect current power supply

If the above described processes occur in pure water, H+ cations will accumulate at the anode and OH anions will accumulate at the cathode. This can be verified by adding a pH indicator to the water: the water near the anode is acidic while the water near the cathode is basic. The negative hydroxyl ions that approach the anode mostly combine with the positive hydronium ions (H3O+) to form water. The positive hydronium ions that approach the negative cathode mostly combine with negative hydroxyl ions to form water. Relatively few hydronium (hydroxyl) ions reach the cathode (anode). This can cause concentration over potential at both electrodes.

Pure water is a fairly good insulator since it has a low auto ionization, Kw = 1.0 x 10−14 at room temperature and thus pure water conducts current poorly, 0.055 µS·cm−1. Unless a very large potential is applied to cause an increase in the auto ionization of water the electrolysis of pure water proceeds very slowly limited by the overall conductivity.

If a water-soluble electrolyte is added, the conductivity of the water rises considerably. The electrolyte disassociates into cations and anions; the anions rush towards the anode and neutralize the buildup of positively charged H+ there; similarly, the cations rush towards the cathode and neutralize the buildup of negatively charged OH there. This allows the continued flow of electricity.[5]

Care must be taken in choosing an electrolyte, since an anion from the electrolyte is in competition with the hydroxide ions to give up an electron. An electrolyte anion with less standard electrode potential than hydroxide will be oxidized instead of the hydroxide, and no oxygen gas will be produced. A cationwith a greater standard electrode potential than a hydrogen ion will be reduced in its stead, and no hydrogen gas will be produced.

The following cations have lower electrode potential than H+ and are therefore suitable for use as electrolyte cations: Li+Rb+K+Cs+Ba2+Sr2+Ca2+Na+, and Mg2+Sodium and lithium are frequently used, as they form inexpensive, soluble salts.

If an acid is used as the electrolyte, the cation is H+, and there is no competitor for the H+ created by disassociating water. The most commonly used anion is sulfate (SO2−
4), as it is very difficult to oxidize, with the standard potential for oxidation of this ion to the peroxodisulfate ion being −2.05 volts.

Strong acids such as sulfuric acid (H2SO4), and strong bases such as potassium hydroxide (KOH), and sodium hydroxide (NaOH) are frequently used as electrolytes due to their strong conducting abilities.

A solid polymer electrolyte can also be used such as Nafion and when applied with a special catalyst on each side of the membrane can efficiently split the water molecule with as little as 1.5 Volts.

Techniques

Fundamental demonstration

Two leads, running from the terminals of a battery, are placed in a cup of water with a quantity of electrolyte to establish conductivity in the solution. Using NaCl (table salt) in an electrolyte solution results in chlorine gas rather than oxygen due to a competing half-reaction. With the correct electrodes and correct electrolyte[clarification needed] hydrogen and oxygen gases will stream from the oppositely charged electrodes. Oxygen will collect at the anode and hydrogen will collect at the cathode.

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Match test used to detect the presence of hydrogen gas

Hofmann voltameter

Main article: Hofmann voltameter

The Hofmann voltameter is often used as a small-scale electrolytic cell. It consists of three joined upright cylinders. The inner cylinder is open at the top to allow the addition of water and the electrolyte. A platinum electrode is placed at the bottom of each of the two side cylinders, connected to the positive and negative terminals of a source of electricity. When current is run through the Hofmann voltameter, gaseous oxygen forms at the anode (positive) and gaseous hydrogen at thecathode(negative). Each gas displaces water and collects at the top of the two outer tubes, where it can be drawn off with a stopcock.

[edit]Industrial electrolysis

Many industrial electrolysis cells are very similar to Hofmann voltameters, with complex platinum plates or honeycombs as electrodes. Generally the only time hydrogen is intentionally produced from electrolysis is for specific point of use application such as is the case with oxyhydrogen torches or when extremely high hydrogen purity or oxygen is desired. The vast majority of hydrogen is produced from hydrocarbons and as a result contains trace amounts ofcarbon monoxide among other impurities. The carbon monoxide impurity can be detrimental to various systems including many fuel cells.

[edit]High pressure electrolysis

Main article: High pressure electrolysis

High pressure electrolysis is the electrolysis of water with a compressed hydrogen output around 120-200 Bar (1740-2900 psi).[6] By pressurising the hydrogen in the electrolyser the need for an external hydrogen compressor is eliminated, the average energy consumption for internal compression is around 3%.[7]

[edit]High-temperature electrolysis

Main article: High-temperature electrolysis

High-temperature electrolysis (also HTE or steam electrolysis) is a method currently being investigated for water electrolysis with a heat engine. High temperature electrolysis may be preferable to traditional room-temperature electrolysis because some of the energy is supplied as heat, which is cheaper than electricity, and because the electrolysis reaction is more efficient at higher temperatures.[8][9]

[edit]Applications

About four percent of hydrogen gas produced worldwide is created by electrolysis. The majority of this hydrogen produced through electrolysis is a side product in the production of chlorine. This is a prime example of a competing side reaction.

2 NaCl + 2 H2O → Cl2 + H2 + 2 NaOH

The electrolysis of brine (saltwater), a water sodium chloride mixture, is only half the electrolysis of water since the chloride ions are oxidized to chlorinerather than water being oxidized to oxygen. The hydrogen produced from this process is either burned (converting it back to water), used for the production ofspecialty chemicals, or various other small scale applications.

Water electrolysis is also used to generate oxygen for the International Space Station.[10][11]

[edit]Efficiency

The electrolysis of water requires a minimum of 286 kJ of electrical energy input to dissociate each mole. Since each mole of water requires two moles of electrons, the specific electrical energy required is 143 kJ/mole (8.9×1023 eV/mole). It follows then that a minimum electrical power input per ampere is implied, namely 1.48 W/ampere. In turn, the minimum electrolytic potential for electrolysis of water of 1.48 V (not 1.23 V). Thus, any current (I) at applied voltage (V) greater than 1.48 V is an overvoltage and results in waste heat which can be estimated as I×(V-1.48).[12]

Water electrolysis does not convert 100% of the electrical energy into the chemical energy of hydrogen. The process requires more extreme potentials than what would be expected based on the cell's total reversible reduction potentials. This excess potential accounts for various forms of overpotential by which the extra energy is eventually lost as heat. For a well designed cell the largest overpotential is the reaction overpotential for the four electron oxidation of water to oxygen at the anode. An effective electro catalyst to facilitate this reaction has not been developed. Platinum alloys are the default state of the art for this oxidation. Developing a cheap effective electro catalyst for this reaction would be a great advance (see also[13]). In 2008, a group led by Daniel Nocera announced the development of an electro catalyst composed of the abundant metal cobalt and phosphate.[14] Other researchers are pursuing carbon-based catalysts.[15]

The simpler two-electron reaction to produce hydrogen at the cathode can be electro catalyzed with almost no reaction over potential by platinum or in theory a hydrogenase enzyme. If other, less effective, materials are used for the cathode then another large over potential must be paid.

The energy efficiency of water electrolysis varies widely with the numbers cited below on the optimistic side. Some report 50–80%. These values refer only to the efficiency of converting electrical energy into hydrogen's chemical energy. If one considers simply the electrical energy input to an electrolyser and the enthalpy of combustion of the H2 product (therefore the energy input and the energy output of the system), then efficiency of 95% is achievable (using platinum catalysts and PEM technology, with H2 production occurring at 1.55V, with ideal Faraday efficiency being achieved). This value of 95% correctly refers to the higher heating value (HHV) of H2. Confusingly, the lower heating value of H2 (LHV) is occasionally used to calculate the efficiency for electroysers, and often for fuel cells. However, it is technically correct to always use HHV, as this value represents the total amount of enthalpy available from the H2 product (which is the enthalpy released during the combustion reaction of H2 with O2). This is generally observed correctly with electrolysis calculations, since LHV if used would give lower efficiency values for electrolysis. However, with fuel cells, LHV gives apparently higher efficiency’s thus promoting the fuel cell and has crept into use; although LHV can be used to 'approximately' benchmark the reaction at the fuel cell electrodes, it is not the true overall efficiency of the fuel cell itself. This can become confusing and therefore only HHV should ever be used for calculations (since LHV is arbitrarily used to disregard the energy released (lost) during to the cooling and latent heat of vapourisation of the reaction products, which is not used in the basic fuel cell reaction).

On a more general note to consider, the energy lost in generating the electricity for the electrolyser is not included in this figure. For instance, when considering a power plant that converts the heat of nuclear reactions into hydrogen via electrolysis, the total efficiency may be closer to 30–45%,[19] although the inefficiencies of power plants in turning heat into electrical energy is not usually included in efficiency, so the former measure of 50–80% efficient is probably a more realistic efficiency.

 

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voltameter, voltmeter , galvanometer etc

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voltameter
 
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Brownlee electrolsis apparatus is used for electrolysis of water

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