DLW-bgkt Report

1 AIR BOOSTER

1.1 HHO GENERATOR

Hydrogen fuel enhancement is the process of using a mixture of hydrogen and

conventional hydrocarbon fuel in an internal combustion engine, typically in a car or

truck, in an attempt to improve fuel economy, power output, or both. Methods include

hydrogen produced through an electrolysis, storing hydrogen on the vehicle as a second

fuel, or reforming conventional fuel into hydrogen with a catalyst.

There has been a great deal of research into fuel mixtures, such as gasoline and nitrous

oxide injection. Mixtures of hydrogen and hydrocarbons are no exception. These sources

say that contamination from exhaust gases has been reduced in all cases, and they suggest

that a small efficiency increases is sometimes possible.

The Hydrogen Generator is a piece of equipment which when installed correctly can

help to increase the performance of a car or motorcycle, or truck and reduces the

harmful emissions dramatically. It does this by using some current from the cars battery

and alternator to fracture water into a mixture of hydrogen and oxygen gasses called hho

hydroxy gas which is then added to the air which is being drawn into the engine. The

hho gas improves the quality of the fuel burn inside the engine cylinders, this can

increase the engine power, cleans old carbon deposits off the inside of an old engine,

reduces the unwanted exhaust emissions or smog and can improve the miles per gallon

that your vehicle gets.provided that the fuel computer does not try to pump excess fuel

into the engine when it detects the much extra oxygen in the exhaust and the improved

quality of the exhaust.This hydrogen generator is easy to make and the components

don’t cost much.

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1.2 ELECTROLYSIS OF WATER

Electrolysis of water is the decomposition of water (H2O) into oxygen (O2) and hydrogen

gas (H2) due to an electric current being passed through the water.

This technique can be used to make hydrogen fuel (hydrogen gas) and breathable oxygen;

though currently most industrial methods make hydrogen fuel from natural gas instead.

FIGURE NO. 1- ELECTROLYSIS OF WATER

2. INTRODUCTION

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2.1 HISTORY

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.

2.2 PRINCIPLE

An electrical power source is connected to two electrodes, or two plates (typicly made

from some inert metal such as platinum, stainless steel or iridium) 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 the anode (the positively charged

electrode). Assuming ideal faradaic efficiency, the amount of hydrogen generated is

twice the amount 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 over potential 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 conductivity about one millionth that of seawater.

Many electrolytic cells may also lack the requisite electro catalysts. 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 electro catalysts.

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Currently the electrolytic process is rarely used in industrial applications since hydrogen

can currently be produced more affordably from fossil fuels.

3.EQUATIONS INVOLVED

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:

Oxidation at anode: 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−

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FIG NO. 2-Diagram showing the overall chemical equation.

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.

4.THERMODYNAMICS

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−    

E0OX = -1.23 V

E0RED= 1.23

Cathode (reduction): 2 H+(aq) + 2e− → H2(g)    

E0RED = 0.00 V

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Thus, the standard potential of the water electrolysis cell is -1.23 V at 25 °C at pH 0 (H+

= 1.0 M). At 25 °C with pH 7 (H+ = 1.0×10−7 M), the potential is unchanged based on the

Nernst equation. The thermodynamic standard cell potential can be obtained from

standard-state free energy calculations to find ΔG° and then using the equation: ΔG°= -

nFE°(where E° is the cell potential). In practice when an electrochemical cell is "driven"

toward completion by applying reasonable potential, it is kinetically controlled. Therefore

activation energy, ion mobility (diffusion) and concentration, wire resistance, surface

hindrance including bubble formation (causes electrode area blockage), and entropy,

require a greater applied to potential to overcome these factors.

5.ELECTROLYTE SELECTION

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 a concentration overpotential at both electrodes.

Pure water is a fairly good insulator since it has a low autoionization, 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 autoionization of water the

electrolysis of pure water proceeds very slowly limited by the overall conductivity.

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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.

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 cation with 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 (SO4-2), as it is

very difficult to oxidize, with the standard potential for oxidation of this ion to the

peroxydisulfate 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. There are also a number of other solid electrolyte systems that

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have been trialled and developed with a number of electrolysis systems now available

commercially that use solid electrolytes.

6.ELECTROLYSIS TECHNIQUE

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, such as baking soda,

hydrogen and oxygen gases will stream from the oppositely charged electrodes. Oxygen

will collect at the positively-charged electrode (anode) and hydrogen will collect at the

negatively-charged electrode (cathode). Note that hydrogen is positively charged in the

H2O molecule, so it ends up at the negative electrode. (And vice versa for oxygen.)

Note that an aqueous solution of water with chloride ions will, when electrolysed, either

result in either OH− if the concentration of Cl− is low, OR in chlorine gas being

preferentially discharged if the concentration of Cl− is greater than 25% by mass in the

solution.

7.EFFICIENCY

7.1 THERMODYNAMICS

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The electrolysis of water in standard conditions requires a theoretical minimum of 237 kJ

of electrical energy input to dissociate each mole of water, which is the standard Gibbs

free energy of formation of water. It also requires energy to overcome the change in

entropy of the reaction. Therefore, the process cannot proceed below 286 kJ per mol if no

external heat/energy is added.

Since each mole of water requires two moles of electrons, and given that the Faraday

constant F represents the charge of a mole of electrons (96485 C/mol), it follows that the

minimum voltage necessary for electrolysis is about 1.23 V. However, observing the

entropy component (and other losses), voltages over 1.48 V are required for the reaction

to proceed at practical current densities (the thermoneutral voltage).

In the case of water electrolysis, Gibbs free energy represents the minimum work

necessary for the reaction to proceed, and the reaction enthalpy is the amount of energy

(both work and heat) that has to be provided so the reaction products are at the same

temperature as the reactant (i.e. standard temperature for the values given above). An

electrolyser operating at 1.48 V would be 100% efficient.

7.2 OVERPOTENTIAL

Real water electrolysers require higher voltages for the reaction to proceed. The part that

exceeds 1.23 V is called overpotential or overvoltage, and represents any kind of loss and

non ideality in the electrochemical process.

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For a well designed cell the largest overpotential is the reaction overpotential for the four-

electron oxidation of water to oxygen at the anode; electrocatalysts can facilitate this

reaction, and platinum alloys are the state of the art for this oxidation. Developing a

cheap, effective electrocatalyst for this reaction would be a great advance, and is a topic

of current research, there are many approaches among them a 30 year old recipe for

molybdenum sulfide, graphene quantum dots, carbon nanotubes and perovskite.The

simpler two-electron reaction to produce hydrogen at the cathode can be electrocatalyzed

with almost no overpotential by platinum, or in theory a hydrogenase enzyme. If other,

less effective, materials are used for the cathode (e.g. graphite), large overpotentials will

appear.

7.3 INDUSTRIAL USE

Efficiency of modern hydrogen generators is measured by power consumed per standard

volume of hydrogen (MJ/m3), assuming standard temperature and pressure of the H2. A

100%-efficient electrolyser would consume 11.7 MJ/m3; the lower the actual power used,

the higher efficiency.

Electrolyser vendors provide efficiencies based on enthalpy. To assess the claimed

efficiency of an electrolyser it is important to establish how it was defined by the vendor

(i.e. what enthalpy value, what current density, etc).

There are two main technologies available on the market, alkaline and proton exchange

membrane (PEM) electrolysers. Alkaline electrolysers are cheaper in terms of investment

(they generally use nickel catalysts), but less efficient; PEM electrolysers, conversely, are

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more expensive (they generally use expensive platinum-group metal catalysts) but are

more efficient and can operate at higher current densities, and can be therefore be

possibly cheaper if the hydrogen production is large enough. Reported working

efficiencies are in the range 60-75% for alkaline and 65–90% for PEM.

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8.HHO GENERATOR(AIR BOOSTER)

Fossil fuels currently constitute 82% of the global total primary energy sources and oil

makes 31.5 % of this. Of the global oil production, 62.2% is consumed by the transport

sector. Thus, the automotive industry is the largest consumer of fossil oil. Studies

have also shown that the demand for oil and gas is rising exponentially and

indications are that fossil fuels will not outlast the century if current habits are not

curtailed. Hence, in response to the growing fuel prices and the increasing pressures for

a cleaner "greener" society, the automotive industry has made efforts to reduce

emissions and increase fuel efficiency. These efforts have primarily focussed on

emissions reductions using catalytic converters, reducing vehicle weight, using

alternative structural materials, improving engine management and fuel supply

systems, incorporating the stop - start technology and introducing alternative sources of

energy such as hydrogen fuel cells, biofuels and others. Governments and

municipalities have also made efforts through the development and implementation of

legislation.

As regulations become more restrictive and global fossil fuel prices increase, the

search for more sustainable sources of transportation fuels becomes more urgent. The

current research into alternative energy sources for motor vehicles is mainly

concentrated around electric/battery powered cars, hydrogen fuel cells, solar and

hydrogen powered cars. These technologies, as promising as they may be, will not

completely replace the fossil fuelled internal combustion engine within the next few

decades. One of the major hindrances will be the lack of supporting infrastructure such

as fuel supply and distribution centres. There is therefore potential for a bridging or

interim technology that can be incorporated into existing technology using the existing

infrastructure, which can lead to greener use of available fossil resources. One such

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option is the introduction of hydrogen gas into the combustion process of an IC engine.

Hydrogen gas is an example of a renewable energy source that can be used to partially

supplement diesel or petrol fuel by enriching supply air. Advantages of introducing

hydrogen gas include higher net heating value and diffusivity of hydrogen in air

when compared to fossil fuels. This means that including it in the combustion

process can lead to a more complete combustion of the fuel air mix. A more

complete combustion can result in the reduction of harmful exhaust emissions

such as hydrocarbons (HCs), nitrogen oxides (NOx) and carbon monoxide (CO). In

addition, better diffusivity produces a much faster flame velocity (on the order of

10x) that can lead to a better acceleration and torque output from the engine.

Musmar and Al-Rousan conducted detailed research on the performance of a single

cylinder Honda G200 engine using air enriched with HHO gas. The HHO generator

used was box shaped, with electrodes made of stainless steel grade 316-L,

electrolysing water. The water was enhanced using sodium bicarbonate. The

engine speed was varied from 1000 rpm to 2300 rpm. This work demonstrated the

feasibility of introducing an HHO generator into the engine compartment as the

generator was about the size of a standard 12V car battery. In addition introduction of

HHO resulted in 54% reduction in NOx and20% reduction in CO. It was also noted

that HHO concentration varied with engine speed. This could have been a result of

no control on electric current fed to the generator. No information is given on the

performance of the HHO generator used.

In more recent work, Leelakrishnan and Suriyan investigated the effects of HHO gas

enriched air on the performance of a single cylinder, four stroke, 5.4 kW SI petrol

engine. Enriched air was supplied to the engine through a passage between the air filter

and the carburettor. Results reported indicate 5% improvement in brake power, 7%

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improvement in thermal efficiency, 6% reduction in fuel consumption,88% reduction

in unburnt hydrocarbons (HC), 94% reduction in CO and 58% reduction in NOx. These

values were reported at full load. However, no information was given on the rate of

production of the HHO gas or whether there was variation in gas production during

the test. Furthermore, the engine used is not representative of the current

technology on the road.

This project investigates the engine performance from partially including hydrogen gas

(also known as brown's gas or HHO gas) into the combustion process of a

conventional spark-ignition engine. A device, stored in the engine compartment, will

produce the HHO gas through electrolysis of distilled water and an added

electrolyte.This can increase fuel efficiency, engine torque and reduce harmful exhaust

emissions.

9.WORKING DIAGRAMPage | 14

FIGURE NO 3-WORKING DIAGRAM

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10.PARTS & MATERIAL USED IN AIR BOOSTER

1. STAINLESS STEEL PLATES

2. BIKE ENGINE

3. BIKE BATTERY

4. PVC PIPES

5. PVC PIPE CAPS

6. WASHERS

7. NOZZLES

8. M-SEAL

9. NUT & BOLTS

10. DISTILED WATER

11. ELECTROLYTE

12. PVC SOLVENT CEMENT

13.MECHANICAL THREAD TAPE

10.1.STAINLESS STEEL PLATE

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FIGURE NO. 4-STAINLESS STEEL PLATE

10.2 BIKE ENGINE

A 100cc Suzuki bike petrol engine is used for test.

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FIGURE NO. 5-BIKE ENGINE

10.3 BATTERY

12 volts bike battery is used in air booster.

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10.4 PVC PIPES & PVC CAPS

Pipe diameters 110mm & 75mm

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Pipe caps diameters 110mm & 75mm

FIGURE NO 7- PVC PIPES AND CAPS

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10.5 WASHERS, CLIPS,NUTPage | 21

FIGURE NO. 8-WASHERS,CLIPS,NUT

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10.6 PVC SOLVENT CEMENT AND THREAD TAPE

FIGURE NO. 9-PVC SOLVENT CEMENT AND THREAD TAPE

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11.SAFETY PRECAUTIONS

Before getting into the details of how to construct the booster,you must be aware of

what needs to be done when using a hydrogen generator of any design. Firstly, hydroxy

hho gas is highly explosive. If it wasn’t, it would not be able to do it’s job of improving

the gas milege your vehicle is getting, Hydroxy gas needs to be treated with care and

caution. It is important to make sure that it goes into the engine as designed and

nowhere else. It is also important that it gets ignited inside the engine and nowhere else.

To make this happen, a number of common-sense steps need to be taken. Firstly, the

hydrogen generator must not make hydrogen gas when the engine is not running. The

best way to arrange this is to switch off the electricity going to the booster. It is not

enough to just have a manually-operated dashboard On/Off switch as it is almost certain

to be forgotten one day. And the generator will be left on making gas while the engine is

off Instead, the electrical supply to the booster is sent through the ignition switch of the

car. That way, when the engine is turned off, we can be sure that the hydrogen generator

is turned off. So as not to put too much amp load through the ignition switch, and to

allow for the possibility of the ignition switch being on when the engine is not running,

instead of wiring the hydrogen generator directly to the switch, it is recommended that

you wire a standard automotive relay across the oil pressure sending unit and then the

relay carry the amp load electricity.

The fuel pump is powered down automatically when the key is off, and so this will also

shut off the hydrogen generator.

An extra safety feature is to allow for the (very unlikely) possibility of an electrical

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short circuit occurring in the Hydrogen generator or its wiring. This is done by

putting a fuse or contact-breaker between the battery and the new Wiring As shown

FIGURE NO. 10- SAFETY PRECAUTIONS

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12.REFRENCES

1. A. Al-Rousan, "Reduction of fuel consumption in gasoline engines by introducing

HHO gas into intake manifold," International Journal of Hydrogen, vol. 35, pp. 12930-

12935, August 2003

2.M. S. Yadav, S. M. Sawant, and H. V. Chavan, "Investigations on generation methods

for oxy-hydrogen gas, its blending with cenventional fuels and effect on the performance

of internal combustion engine," Journal of Mechanical Engineering Reserach, vol. 3, no.

9, pp. 325-332, September 2011.

3. S. A. Musmar and A. A. Al-Rousan, "Effect of HHO gas on combustion emissions in

gasoline engines," journal of Fuel and Energy, vol. 90, pp. 3066-3070, 2011.

4. WWW.WIKIPEDIA.COM

5. WWW.HHOGENERATOR.COM

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