THESIS

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R.B, KLING R.W.NODDINS

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AN INVESTIGATION OF CHEMICAL MEANS OF PRODUCING

ELECTRICITY FROM COAL.

A Thesis Submitted to
The Faculty of

MICHIGAN AGRICULTURAL OOLLEGE

By

R. Be Kling R. W e Nodding

Candidates for the Degree of

Bachelor of sSoience.

June, 1920.
 

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“I THINK THE MOST IMPORTANT LINE OF INVESTIGATION
IS PHE PRODUCTION OF ELECTRICITY DIRECT

FROM THE COMBUSTIBLE".

Thomas A. Bdison.

402039
BIBLIOGRAPHY.

Klectricity Direct from Ooal.
By Emil Baur
Scientific Amerioan Supplement, May 31, 1915.

Hleotrioal Energy Direct from Carben.
By A. B. Kennelly,
Electrical World and Eleotrican, Jan. 5, 1901.

Carbon Cell Without a Metal Mleotrode.
By C. Jd. Reed,
Kleotrical World, Nov. 21, 1896.

Direct Production of Electricity from Coal.
George Herbert Stockbridge,
Engineering Magazine, July, 1896.

Electrolytic Dissociation,
By Svante Arrhenius,
Scientific American Supplement, April 20, 1912.

BRleotrolytioc Dissolution and Deposition of Carbon.
Héaitorial, London Electrician, June 12, 1896.

Eleotricity Applied to Chemistry,
By Harvey C. Jones,
Engineering and Mining Journal, May 25, 1912.
Kleotricity and Ohemical Action,
By Harvey C. Jones,
Engineering end Mining Journal, May 18, 1912.

Janger's Oarbon Cell,

Centralblatt Acoumulation, page 53-54,
April 5, 1907.

Science Abstracts No. 752, page 3038, 1907.
Transformation of the Bnergy of Carbon into Other
Available Forms,
By GCG. Je Reed,
Eleotrical tiorld, Yol. 38, 1896.

Practical Eleotro-chemistry, page 349,
By Bertram Blount,

Electricity from Coal Gas,
Electrical World, Vol. 70, page 472.

A New Primary Battery in Which Carbon is Consumed,
By Willard &. Case,
Bleoetrical World, Vol. page 132.

An Experimental Carbon Cell,
By S. J. Reed,
Eleotrical World, May 11, 1918.
Some New Forms of Gas Batteries and a New Carbon
Consuming Battery.
By Willard EK. Case,
Electrical Review, Sept. 1897.
The Misuge of Coal,
Electrical Review Lond., April 18, 1902.

An Experimental Carbon Cell,
By S. Albert Reed,
American Bleotro-chemical Soolety,
April - May, 1918.
Kleotriaity from Coal,
Bditorial Eleotrical Age, April, 1908.

Bleotrioity Direct from Carbon,
By Prof. Richard Lorens,
Electrochemical Industry, Jan. 1904.

The Carbon Cell,
By Prof. F. Haber and lL. Bruneo,
Int. Klectrical Congress of St. Louis,
Sept. 1904.
The Coal Battery,
By Hugo Jone,
Western Bleoctriocian, Nov. 21, 1903.

The Reid Process,
ElLeotrioal Review, Hew York, Dea. 12, 19035.

Fuel and Heat Batteries,
By ©. J. Reed,
Eleotro-ohemioal Industry, Jan. 1904.
The Carbon Ceil,
Western Electrician, Sept. 3, 1897.

The Jacques Carbon Battery,
By C. J. Reed,
KLeotriceal Engineering, July 22, 1896.

Solvents of Coal,
Soientifio American Supplement, Vol. 84, page 131.

A New Primary Battery,
By H. Bellini,
Engineering Magazine, Vol. 49, page 436-7.

Electricity Direct from Coal,
By We. Ramsay,
Rieotrical Review and Western Eleotrician,
Vol. 9, page 692.
Thermo-eleotric Batteries,
By Ce. Je Reed,
American Hleotrioian, 1897, page 118.
Progeedings of The American Institute of Kleotrical
Engineers,
Mareb, 1888.
Comparison of Efficiencies of Steam Engine and Carbon
Celli,
Seientifio American Supplement, May 31, 1918.
MLACTRICAL GNARGY DIxuCT FROM CARBON.

By A. C. Kennelly.

A pound of good coal when burned in air liberates

about five and seven tenths horsepower hours of energy.

In ordinary fairly large engines it takes from
two to three pounds of coal per boiler horsepower hour.

If eoal were converted to ooke and if coke could
be consumed in a galvanic battery in the same way in
whieh sine is eonsumed there would be no such necessary
waste of energy as there is in a thermo-dynamic process,
and theoretically almost all of the energy of combination
of coke carbon and oxygen oould be liberated in the
eleotrical cirauit of the apparatus.

This wuld represent the direct generation of
the energy of coke carbon into eleotrical mergy.
Unfortunately, however, carbon refuses to behave like
sino and burn in a voltaic cell.

The only known means by Which oarbon could be
made vo give out ite energy in a voltaic oell in
competition with the use of coal in a steam engine, is
by the formation of either carbon monoxide or carbon
dioxide: in other words the same oxidation which yields
the energy of carbon in the process of combustion mst

take place eleotro-chenically. The oxygen for the
purpose must be obtained from some cheap electrolyte
eontaining oxygen and cannot so far as known be obtained
from the atmosphere directly. In other words it is
necessary to rob an electrolyte of oxygen in order that
carbon shall combine with it electrolytically. If the
oxygen of the electrolyte were but feebly held, that is
to say, if the electrolyte oomisted of a chemical
combination with oxygen so unstable as to require but a
negligibly small amount of mergy to tear the oxygen
away, and if moreover the substance or substances with
which oxygen was unstably linked were eapable of enter-
ing into combination with the other plate of the
voltaic couple with tt little absorption of eergy:
then it might be possibie for the voltaioa cell te work
with a power output theoretically approaching that of
the combustion valve of carbon and oxygen.

The union of carbon and oxygen in the oell: would
take place without sensible elevation of temperature, the
eleotrolyte would give up its oxygen for the formation of
earbon diexide and the products of the cell wuld have to
be chemically eliminated in some continuous manner, to
be replaced by fresh electrolyte.

All this requires the existanoe of m electrolyte
possessing properties of small chemical stability, to-
gether with the capability of forming suitable chemical
combinations at both plates of the couple. Moreover the
 

mee ea le
electrolyte must be so abundant as to be very cheap.

An examination of thermo-chemioal data confi rms
the results of the very large amount of expa imental
inquiry made during the pst century and leads to the
condlusion that there is no oheap electrolyte available for
the buming of earbon in a voltaic cell at ordinary
temperatures with an efficieoy that can compete with
that of a steam engine.

Prospects from thermo-chemiocal data seem equally
unfavorable. The hot voltaio cell is complicated by the
introduction of thermo-electrice effeets.

If a cell is a mere thermo-eleotrico couple it
mst do work in the cirouit by receiving heat at a high
temperature at one contact and rejecting heat at a lower

temperature at the ether contact.

The prospects are not enoouraging for the hot
voltaic cell but there is hope that it may be found.

Apart fromthe solution of the problem by
improvements in heat engines, or by the discovery of a
suitable wrking substance in the voltaio cell, there is
always the possibility of finding some new meochaniem by
which the heat energy of carbon atoms can be converted
inte the energy of mass rotation. We are still so pro-
foundly ignorant of how the energy of carbon is stored
relatively to that of oxygen that 2 discovery of the hidden
, en
mechanism of the storage rnrinaiple might lead to a
discovery of a new means of releasing it. In other words
there is something in a lump of carbon in conjunction |
with a lump of oxygen which corresponds either to a bent
spring or to the motion of a gyrostat. All we know is
that when the two mbstances are brought into mfficiamtly
intimate contaet with the aid of a high temperature either
the spring is released or the gyrostatic motion is
arrested with the prodmotion of the jostie energy among
the molecules of a substance, or of that particular kind
of rapid osgeillatory motion which we assume heat to be.

It is conceivable that if we had a clear idea of the
nature of the invisible gyrostate, we might discover some
means by which the springs might be released without the
production of jostle energy and with the direct production
of some kind of utilisable force.

The fact that by chemical processes we are able to
transfer a part of the energy to a differmt substance in
chemical form without first liberating it in heat should
encourage hope that we may find a means of transferring
it in some other form than ohemical or thermel.

Exoept in localities where water power is available

ceal is the main source from which we derive our electrical

power.

Unfortunately in the process of converting the
potential mergy of coal into eleotrioal energy, a series
of heavy losses is incurred.

There is firstly a loss of heat in the stack,
heat whigdh should have gone to the boiler; seoondly
power is lost through the fact that a heat mgine at
. best can transform into useful work only a define
fraction of the heat supplied; thirdly we have the
losses due to friction in the engine, dynamo, eta.
These losses could be avoided if we could eonstruot
an efficient galvanic cell in whioh carbon is
consamed instead of some costly materials usually

employed in galvanic cells now in use.

The problem of constructing a carbon oell is
therefore one of peculiar interest and resolves itself
into that of onstructing a cell of the type
O/eisotrolyte/O, -
Lz

JUNGER'S CARBON CELL.

Carbon burns in sulphuric acid of more than
fifty percent, which, to improve its conduetivity,
should be heated. In sulphuric aoid of 95%, carbon is
electrically almost as active at 95 or 100° C. as
sino is in dilute sulphuric acid. The acid is ée-
composed, the prodiots being CO, Hp, 50,4; and depolari-
sers are required in such carbon cells. 5. We. Junger
combines an anode of amorphous carbon with a cathode of

graphite, depolarised by air or in other ways.

The cathode is a perforated tube made of
graphite powder and solium silicate, which is after-
wards rendered insoluble, by dipping the mass in magnesium
salts, end compressed; powdered glass may also be fused with
the graphite. The anode consists of pieces of coke,
covered by a heavy perforated horisontal anode plate.
The cell box stands within another cell box, the space
between the two being charged with steam; the outer box
48 pecked with heat-insulating material. Air is foroed
through the cathodes. The eleotrolyte, concentrated
sulphuric acid, may be charged with NO, No0g, Og,
oxygen compounds of chlorine, or sulphates of metals
which form several sulphates; then a diaphragm of briok
graphite or asbestos ig applied. The working eleoctro-
motive force is 0.5 volt. Several arrangements are

proposed.
13

The twe chief reactions on whim this new carbon
cell is based are SOp + 0 + HpO = HpS0y; and & Hp804 + 0 =
S0p + & Hy.

Phe first step is carried out in cells built up
of earthen-ware vessels, with a vertioal diaphragm of the
same material both compartments being sealed by the
cover, and vertical electrode slabs of grephite, the
enode packed with porous graphite moistened with
nitrosyl-sulphurio acid (depoleriser) and the cathode
with very small grains of coke and poreus ooal in

order to secure a large surface.

Through pipes air and supherous acid are blown
into the compartrents; sulphurie acid trickles down
the cathode compartments, from which it is drawn eff,
while the current generated flows through the cirouit.
The electromotive foroe varies with the concentration
of the acid (generally 80%) from 0.5 to 0.3 volts (in
more conoentrated acid). The second step, the reoonversion
of sulphuric into sulphurous acid is effected by heat-
ing the sulphurio acid with coal or ooke.
JACQUES* CARBON CELL.

The dgacques Cell which produces Eleotrioci ty
from Coal and Atmospheric Oxygen at Three-hundred
Degrees Centigrade.

The iron oerucible whioh is the outer part of
the Jacques cell serves as a positive electrode. It
is heated to about three-hundred degrees centigrade
‘and filled with oaustic soda. The bottom is covered
with a layer of granulated quicklime which acts as a
diaphragm as a sheet iron cylinder is set with its
serrated lower edge resting upon this layer. The
cylinder divides the contemts of the orucibie into a
cathode chamber and anode chamber.

Into the anode chamber depends a carbon rod
while into the cathode chamber a wuentity of manganese
dioxide is added to the caustic soda. The dioxide
dissolves in the fused alkali and takes up oxygen
from the air forming a green melt containing sodium
manganate and having approximately the same potential

as oxygen.

On alosing the oirouit the manganate beoOmes
reduoed to magnetite which is in turn reoxidiszed by the

air.

Te earbon reacts with the caustic soda with
 

 

    
   

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formation of sodium carbonate end hydrogen, and it ig
really this latter which fumishes the sleotronotive
force, 80 that to be precise, this oell is not a oar-
bon eell but an ox-hydrogen cell. And in point of

fact the voltaze is approximately that corresponding

to oxygen and hydrogen electrodes.

It was reported that with a battery of 10u
pote each 12 inches deep and 11/2 inches in diameter
a ourrent averaging 90 volts md 16 siiperes was
obtained for 19 hours. Bight pounds of carbon was
oonsumed in the pot, representing 94% effioienay.

(Coal for heat or air not mentioned).
16

BAUR'S OCARBON-OXYGEN CELL.

To avoid wastefpl secondary reactions it is
necessary to use high temperatures. Only at bright
red heat where garbon burns vigorously in sir, oan
we hope to avoid these wasteful secondary reactions,
and to thus obtain a cell practically free from
polarization effeuts over wide ranges of working
conditions. The diffieulty which now presants itself
is to find a aitable oxygen electrode.

Looking areund for an appropriate material we
finally hit upon molten silver.

When the molten metal is allowed to cool at
the surface so as to form a semi-colid crust, little
craters are formed upon the crust which present the

eppearance of a boiling mass.

This effect is due to the liberation of oxygen
Whieh is dissolved in the molten silver and which is
liberated ag the metal cools. One oubic ingoh of silver
GQissolves in the molten state, ten oubic inches of
oxygen measured at ordinary temperature. Such a mass
of molten silver should form a very effeotive oxygen
@leotrode aapable of furnishing a considerable ourrent,
in view of the high diffusion velocities prevailing at

red heat.
 

 

Baur’ CLL.

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£- FLecTRo.y7é
O- Vip a for

CARBON.

24774, 2
M-Macwesia DIAPHRAGM.

P- Porceraiw CruciBee.
Ae - Mo.ren Sitver

 
isxperience has in fact confirmed this expeotation.
All that is necessary is to combine suoh am electrode
with a fused eleotrolyte and a carbon electrode, and we
obtain a oell whose electromotive force is practically
that caloulated from thermo-dynamios data - a cell
furthermore which shows very little polarisation when
preperly handled.

The constrmotion of such a cell is shown below:

When working, this celi must of course be placed
ina mitable furnace.

A oarben electrode C. whioh is formed into an
inverted bell to present a large surface, hangs dom into
@ poreelain srucible P, whose bottom is covered with
silver (AG). Into this dips a porcelain tube 0 through
whioh air or oxygen is introduced. <A stout nickle
wire (not shown] forms the second electrode. The space
between the carbon and the silver is ocooupied by the
fused electrolyte E. In order to prevent particles of
coal fron falling into the silver it is well to provide a
magnesia diaphragm Mas shown. The electrolyte met be
an exy-salt which is fixed at a thousand degrees centi-
grade, whioh does not decompose at this temperature, ani
also is unattacked by oarbon, or at least not sufficiently

attacked to cause my inoonvenienoce.

Fortunately there are a number of salts which
satisfy these requirements and which present the further
advantage of cheapness. lkolten glass is one suoh
substance, also borax, potassium and sodium carbonate,

or oryolite od alunina.

Theory demands that the electromotive forge of
the earbon-oxygen cell must be independent of the nature
of the electrolyte, and this is indeed found to be very
nearly true: the aleotromotive force is in all cases

close to one volt.

The differences are due in fact to accidental
variations in the conditions of the experiment, md are
in fact asoribable to the fact that the gas liberated at
the carbon electrode is not pure carbon dioxide mt
oontains more or less carbon monoxide - in some cases

as much as 99%.

The presence of oarbon monoxide is attended by
an inorease in the electromotive foroe of the cell, in

fact coalqmilation gives the following figures:

sor pure COp EoM.Fo =» 0.997
For 99% CO, 1% COe, 8M.¥. = 1.129

The problem of oonstructing a reversible carbon

oe@ll is therefore solved.

An important circumstance from a teohnical
point of view, is the fact that the oell is capable of
fumishing a considerable current without losing
 

appreciably its electromotive force and furthermore, the
internal resistance of the cell is relatively smell.

The prospects of the oommerocial exploitation of
the carbon oell are therefore good. Tha prineipal, _
question which now faces us is whether the shaped ooke
electrodes om be made sufficiently cheaply.

If a ton of coke oo sts $5.00 and the carbon is
burned to OO in the cell, furnishing an electromotive
- foree of one volt the kilowatt-hour costs 1.25 cents.
But the electrodes used at the present day in the
@lectro-chamical and sted furnaces cost $45.00 to
$50.00 per ton. With these it wuld not be possible
to work economically.

The carbon monoxide we cannot look upon as a
by-product, for at least a yert of it could be consumed
in heating up the eell.

The cost of silver might at first be thought
prohibitive. But it is not impossible that by
economical use of the metal the investment of a large

amount of capital might be avoided.

As regards the recovery of waste heat and the
durability of the vessels employed, modern glasses industry
ie quite able to take care of this. Lastly a number of
minor diffiouities of construction remain to be disposed

of. They are however no more serious than those
commonly met in developing a new process.

w

 

 
 

Ma: BCUROLYVIC DusrOLlVIOGN CE CARBON
By Dr. Coehn.
Sditorial from London Hleotrician, April 3, 1896.

“a noteworthy paper by Jr. Alfred Coehn was
recently read before the German Zleotro-technical
Association end printed in the Eleotro-technisohe
Seltachrift from which we transoribe its essential
argument. It deals primarily with the question whether
carbon is competent to form ions and thus take sotive
part in an electrolytis circuit, in other wrds, can
carbon be caused to dissolve from an anode in the
manner gharacteristio of a metal? An observation
Dearing on the point was made by Bartoti and Papasogii,
who found that on passing mrrent between carbon
electrodes immersed in dilute sulphurio both carbon
monoxide ana oarbon dioxide appear at the anode in
addition to oxygen, whence it follows that the mode
takes an active part and suffers oxidation. Dr. Doehn
has attempted to extend this result by varying the
eoncentration, temperature, and ourrent density so as
to indaoe complete suppression of the oxygen at the
anode and ites replacement by pwrodots of the oxidation
of earbon, aad he has so far sueceeded that the gas
escaping at the anode may consist of substantially
70% COg and 80% CO. A mall quantity of oxygen

(about one percent) ia however usually present.
In these researohes it was notioed that at
moderate temperatures disintegration of the anode
ocours and particals of carbon @ pear in suspension
in the eleotrolyte.

At higher temperatures this disintegration does
not take place but a signigieant coloration of the
acid is perceptible. The liquid is at first yeliow,
and in longer trials, be comes dark red md red brown
in oOlor. If this color be due to dissolved carbon,
it my be fairly concluded that the carbon is in the
ionieo state and dirigible by the current.

Seeing that the carben thus present is not
capable of decomposing water, the solution containing it
ghould be in a condition to deposit the carbon at the
cathode. Experiment bears out this deduction, for on
substituting a platinum for a carbon cathode, oarbon is
deposited thereon in a manner charaocteristio of a netal.
The first film of carbon exhibits the color of thin
plates, but as the deposit thickens it becomes blaok
and graphio. The phenomena of solution and precipitation
oan be obtained with various forma of carbon, inoluding

carbon rods for are lighting and blast-furnace coke.

After obtaining this remarkable result, Dr.
Coehn took eare to ascertain that the deposits formed in
the maymer described are really carbon and not some

metallic impurity derived from the anode. The deposited
materiel is insoluble in hydrochloric acid, slightly
soluble in nitric acid - recalling in thet respeot the
behavior of carbon in steel upon which is based the
Eggerts colorimetric method of determining carbon.

The film disappears completely on heating in
contact with air. Determination by combustion (such as is
practiced in ultimate organic analysis) suffices to
establish the belief that the deposit is chiefly
carbon, associated, however, with oxygen and hydrogen
{n the proportions to form water and thus to be regarded
as hydrated. This hypothesis is borne out dy the be-
havior of the film with strong sulphuric soid whieh acts
upon it much as if it were a garbmydrate. .

The establishment of these facts led br. Coehn a
step forther. To construct a cell ocapable of yielding
eleotrical mergy by the oxidation of carbon, it is
necessary to find a cathode eleotro-negative to the

carbon, which has to fanotion as anode.

Lead peroxide in the form of a plate from a
secondary oell fulfills this need. ishen such a cathode
is opposed to carbon anode in a bath of sulphurio acid
of the right temperature and concentration a wimaery
cell is obtained in whieh carbon is the material attacked:
@ cell made in this manner gives a voltage of 1.03 on a

circuit having an external resistance of 100 ohms.
 -_

Dr. Coehn does not state what fraction of the

total energy appears as electrical mergy.

The question now arises, how far the results
recorded are really due to carbon acting as a soluble
eanode? Platinum when exposed to lead peroxide in
sulphuric acid electrolyte becomes en anode, and gives
a current which however decreases to a vanishing point
eas soon as the platinum electrode has aaquired its
complement of oxygen. No such arrest of the output of a
carbon-lead peroxide cell takes place. ‘Zhe current is
Obtained until the cathode is exhausted, and the cell
recains its efficienoy when a fresh plate of lead

neroxide is supplied.

Dre Coehn ends his paper by the following

oonalusions:

le It is possible to prepare a solution of carbon

by eleotrolytic means,

2. Carbon oan be separated from suc a solution at

the cathodes

3. A cell may be meade having its soluble eleotrode of

carbon.
A NEW PRIMARY BATTERY IN VHICH CARBON IS CONSUMED.
By Willard E. Case. |

The high oost of zine consumed in the primary
battery has always stood in the way of its more general
adoption as a source Of electricity, and hence it has
been the endeavor of many to find a substitute less
costly. Carbon in its different forms evidently
presents a number of advantages, principal along which
is its oheapness. EHleotric currents have been produced
by the union of oarbon and oxygen in the past, but the
methods employed have required a high temperature and
hence enteiled considerable loss of energy in the form
of heat.

In the usual styles of batteries carbon
constitutes the insoluble or negative eleotrode, but in

the new cell carbon is a positive or soluble electrode.

The accompanying illustration shows one form of
the cell, which oonsists of the glass jar A, containing
@ porous cup V, in which ia placed a conducting body
of hard carbon D, such as ooke. The negative electrode is
a sheet of platinum OC.

In the porous cup is placed a quantity of carbon
E, in comminuted form, previously moistened with sulphuric
aciaé. In the outer vessel A, is placed aulphurio acid.
A cel. thus arranged will give substantially no current,

 
zo

inasmuch as both elements resist the action of the acid,
however, ohlorate of potash is gradually added in smell
quantities. The result of the reaction of the sulphuric
acid and the ehlorate of potash is the formation (among
other things) of peroxide of chlorine, C109, which is a
yellowish-red gas and which permeates the liquid,
gradually turning it to a red color. fFor practical
purposes it is sufficient to cease adding chlorate of
potash when the acid turns s distinct red. A reaction
betwem the oarbon and the peroxide of chlorine will,
however, begin as soon as the oxygen permeates the porous
cell mad reaches the carbon, and if the eddition of
chlorate be suspended, this reaction will continue until
the acid loses its red hue, wha probably the chemical
affinities between the oxygen ani the carbon are satisfied.
More chlorate mst then be added. (C10, ise very unstable
oxygen compound, decomposing under the action of sunlight
and exploding at about 140° F.) ‘The cell should be
covered to prevent the escape of gas and the jar made

opaque.

The peroxide of chlorine formed apparently de-
composes into chlorine and oxygen. The oxygen attacks
the carbon producing apparentiy carbonic acid. The other
products of the reaction of chlorate of potash and
sulphurie acid are seemingly inert in the cell. A certain
amount of polarisation occurs which may be reduced by

agitating the liquid.
 

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The eleotromotive foroe of this cell is

approximately 1.25 volta.

Note-

The porous oup is not essential. It merely
prevents the oarbon of the anode from mreading
through the whole of the electrolyte.
BP EilThausys.

Nearly all the experiments were performed with the
sulphurie acid type of cell. It was stated in the article
on Junger's cell that carbon was as active in sulphuric
aoid of more than 95% concentration as gino in weak

sulphurio acid.

The first necessity was Zo find some substance
which could be used as the negative electrode of the
battery; oarbon being the negative.

The material used in almost all the previons
experiments was platinum but this material was not

available.

Dre Alfred Coehn used lead peroxide in his oell
as the pesitive electrode. This was the mterial used
in all the experiments as it was available in the form

of plates from secondary cells.
auxperiment No. l.

The object of this exveriment was to determine
whether or not carbon was active in concentrated sulphuric
aoid and the temperature at which it was most active if

any chemical aotion took place.

The electrodes were a small piece of lead peroxide
Plate from a storage cell and a carbon rod from m exhausted

dry cell.

 @hese vere dipped in electrolyte of 75 o.c0. of
concentrated sulphuris acid which was contained in a

250 o.c. beaker.

 

DATA

Time EMF. Curent Temp. Time EMF. Current Ffemp.
volts. milii- oF, volts. milli- op
amps alps

2:48 1,010 00 87 6:41 0226 80 168
3:00 66 00 88 3:43 e220 75 168
3:08 e 260 650 88 6:46 »200 65 164
3:10 e266 50 68 3347 e196 60 160
$:11 e200 65 638 3349 e240 90 184
3:13 e180 60 88 5: 53 e260 100 201
6:15 0170 53 88 3; 56 e240 90 £02
3:17 e160 50 88 3: 68 ~210 76 £201
3:19 ei 87 5O 88 4:02 e320 130 280
3:28 elLl4 45 88 4:05 e520 125 300
3:25 «200 66 120
5:27 0195 63 121
3:29 e180 §8 120
5:53 ol FZ 50 120
3:35 0265 100 155
$:37 ~ 260 100 168
3:39 e200 85 161
CONCIUSION.

Inoreasing the temperature increased the sotivity
of the substances to a very slight extent. The greatest
ourrent and voltage was obtained at 155° F; showing a

Slight advantage in inoreasing the temperature.
4

oxperiment No. 3.

The object of this experiment was to determine
whether a difference in the degree of concentration would
make the cell more active and to determine the degree of

eoncentration which would give the greatest output.

The dleotrodes and other apparstus was the same as

used in Experiment No. l.

 

DATA
Time E.M.F. Current Temp. HoS0g HpO % Concentration
volts. WMilli- °F CG eGe OedDe
anps a

1:55 58 0.00 66. 75. ili. 67.2

2:00 «70 152. . 17. 61.6
074 155. 20. 79.5
77 158. 24. 76.7
82. 164. dl. 71.7
85 170. 33. 69.5
88 170. ' 66. 67.5
092 172. 41. 64.6
o 94 175. 47. : 61.5
296 172. 49. 60.5

243 169. 56. 57.2
Time EMF. Current Tem. Hpg804 HeO % Concentration

 

volts milli- oF CeGeo GceC.
GMB.
1.90 0.00 163, 62. 54.7
| 66. 53.2
3:45 ~60 ° 87. 80. 56.5
5:48 48 50. 85.
3:49 040 50. 64.
3;60 023 50. 80.
Cell was shorted until 1:15 pem. April 26.
upon opening the ocirouit the following
results were obtained.
1:15 e015
weight of Hlesctrodes
Carbon Lead peroxide
Before experiment | 77.3 68.3
After experiment 81.7 89.3

The inorease in weight was due to the absorption
of the electrolyte by the electrodes. They were nearly
dry at the beginning of the experiment.

CONCLUSION.

The greatest output was obtained with a concentration
of 54.7% During the last part of the experiment the cell
wes short oirouited for 69 hours. After being shorted for
this length of time the cell still gave am E.M.F. of 015

volt as s00n as the circuit was opened.

The aleotrodes were weighed before and after the
experiment but they were both practioally dry whem placed
in the electrolyte go botn absorbed acid and were heavier

after being used than before.

No ohange or evidence of asction could be observed on

the darbon electrode.
 

 

 

Experiment No. 3.

The object of this experiment was to détermine
whether any eleetromotive force could be obtained from
a eel consisting of lead peroxide and a carbon rod as
electrodes and nitrie acid for the electrolyte. In
the later part of the experiment the effect of adding

hydrogen peroxide to the cell was noted.

 

DATA
Time eM. Current Nitrio Hydrogen
volts. milli- aoié peroxide
anps. Gee OeBo
5:28 o 54 00. 55. 15.
6: 31 266 00.
6:32 o 34 125.
3: 33 052 . 135.
3: 35 81 130.
3:40 eda 126.
33:45 025 80. 20.
3: 50 DO 90.
3; 52 024 70. Ges oolleots around carbon and
3: 55 o 24 70. lowers E.M.F.
4:05 e21 60.
4:10 e018 50. 25.
4320 e1l9 55.
4:25 o22 60.
4:30 e£2 66.
4:35 «20 65. S20
4:37 e28 100.
4:40 e284 76.
4:45 025 80.
4; 50 084 80.

Data on second part of experiment with Nitrio acid and
hydrogen peroxide.

EMF. Elie Fe

volts volts

open across |
oireuit 22 ohms.
54 40 oO. 25- 0.00 fo aotion
- 52 037 60. 5. gas evolved
04 7. from both
016 10. electrodes.
°L8 50. 13.

220 650. 14.
ave

The action of the hydrogen peroxide and hitrio
acid on the lead peroxide plate rapidly reouded it to
white lead oxide; so another cell was made which had a
porous coup to keep the solution oontaining the hydrogen
peroxide from the lead peroxide. This mede the
reduction of the lead peroxide such slower and inoreased

the iH.l.F. of the cell.

with 30 0.0. of nitric acid and 10 a.a. of
hydrogen peroxide an op@m cirouit voltage of .63 volt was
obtained. \When short olrouited thru a milliammeter a
voltage of .20 and ourrent of 75 milliamperes were obtained.

When this oell was left short-cirguited for about
twenty hours She lead peroside was partially decomposed to
white lead oxide. The carbon did not show any evidence

of decomposition.

he experinents with this type of cell were all

performed at room bemperature.

From these experiments it was conoluded that the
BMF. and the ourrent obtained were dne to the chemical
agtion within the electrolyte and the decomposition of
the lead peroxide plate.
 

BXPERIMENTS WITH SULPHURIC ACID CELL
WHOSE ELECTROLYTR CONTAINS
PEROXIDE OF CHLORINE

The objeot of these experiments was first to
determine the effeot of adding potassium chlorate to
the enlphuric acid eleotrolyte of the cell and to
test a celi whose electrolyte was sulphurio acid
containing peroxide of achlorine and whose electrodes were

oarbon roés and a lead peroxide plate.

Vhen potassium chlorate is added to cencentrated
sulphuric acid ehlorine gas is given off and the acid
tums red due to the presence of peroxide of chlorine

whioh is a powerful oxidising agent.

Peroxide of chlorine is decomposed by sunlight
and explodes at about 140° F.

 

DATA
Time Bo Me. Fo Current HpS0,4
volts milli-
amps.
2:40 ol7 50. 50. One carbon rod.
2:43 ei 60.
£:47 220 55.
2:48 0235 90. 75. Two carbon rods Pb0g
2:53 e22 90. game sise.
2: 55 226 100. Three oarbon rods Pb0s
$:14 28 125. 125. same sise.
e 26 £00.
026 200.

4:00 03 Short oirocuited.

a a>
. alos otssaqiog Saw evyioisse.s avom ifso s
orow. seheitee fs odo.dw pas eatioldo to ebixoiey ynial
F setala sbixeore: baal ea bos ebor mt

hetstsmegnon’ of SoBhs el starcLino mrteeasoe ii
Show ead bre zo mvig af aan oattofio hios oft
ee a i
‘enbsofdo To shiroxvs; Yo sompasy eos of us Des |

4 «

 

i
dalle we Beaoan ove 6 ai enitol[ie to shixored
seF & -% ef “OSL f0ds ta senvi ins,
a r f ' ATAC
Bae poGgh oo jmerts) = wt KD
ee ir ~i LL bm oJ Lev
res oe ee — : : so =
ae Be, Bousae er ae OE.
; oad Us.
ee rodeo ony 4 ay «Ge aS.
aks ' OR a
goes aber. pao eeu? OGL 356
,. sete ease -8al -G82 aS.
‘ 008 38.
a ‘ .0e8 uo.
‘ hes lietin tronic &.
‘5
| om, 5 :

CTT ued Sarthe tigre nl eect
—_— A asl

«THORS garde isi: ao Istvevwoy 3s att: °°

\
 

The reostat was then adjusted for an E.M.F.
of .3 volt and the cell left connected across the

rheostat. for 20 hours.

At the end of this time the polarity was
reversed and the oell had an E.M.F. of .2 wolt on
open oirouit. The carbon rod was partially decomposed
and the lead peroxide plate seemed to have changed to
lead sulphate.

fests were then made to determine whiad plate
had given out or whether it was the electrolyte.

With the same eleotrolyte and oarbon rods but
a new lead peroxide plant an E.M.F. of .3 volt was
obtained.

With 014 electrodes. but new eleotrolyte an
AMF. Of e534 Volt and current of 90 milliamperes were
obtained.

With old plates and eleotrolyte but adding
more potassium chlorate to the electrolyte gave the
following results, An BoM.F. of .4 volt on open
oirouit and when short circuited through the milli-

amperes.

The results indicate that the electrolyte had

given out.
ae -- — et ir +>

The results of the first experiment using a
small amount of potassium chlorate in the sulphuric

acid were encouraging so a large cell was built.

This cell consisted of seventeen carbon rods
weighing 4.25 1b., a lead peroxide plate weighing 1 }b.,
925 0.6. eoncentrated sulphuric acid which with the
battery jar weighed 6.75 1b. A mall amount of potassium
chlorate probably about 10 gms. was added to the

electrolyte.

 

 

DAPA
Time EMF. Ourrent Temperature
volts miilili- ey
amps.
9; 57 84 00. 70.
10:26 - - 59 475.
10; 27 » 56 465. 8l.
16; 29 85 460.
10:45 053 422. Sl.
2:15 047 380.
2:15 048 400. 72.
3:15 47 390. 71.
4:15 48 400.

Cireuit left open between April 29, when oell was
built to April 30, when next readings were taken.

1:25 1206 70.
1:28 78 650.

1:30 078 610.

1:31 6 70 580.

1:37 062 §10.

1:45 e dE 480. 70.
2:00 e 56 469.

8:10 055 455.

2:50 e52 4465.

$:00 « 84 440.

May 4.

Cirouit was open from April 30 to May 4.
1:46 1.16 50.

1:47 1.8 420.

1; 50 o 96 $90.
 

Time EMF. Current Temperature
volts milli- oF
, amps
2:58 292 370.
2:00 89 368.
8:10 87 545.
2:16 085 340.
2:20 84 5335.
May 10.
The oe@ll was left open from May 4 to May 10.
R:00 1.42 000.
2:03 1.37 55.
2:05 1.10 750.
2:10 1.02 620. .
2:15 88 §75.
2:20 84 640.
2:25 82 480.
2:30 72 620.
2:35 «70 §90.
2:40 68 540.
2:45 066 530.
3:00 61 490.
5:05 62 490.
8:10 «61 490.
3:20 «59 476.
3: 35 e 58 470.
3:50 e 58 468.
$; 36 57 460.
5:40 e 56 460.
3345 56 455.
$; 50 o 56 450.
¢55 055 445.

When the cirouit was opened the E.M.F. of the cell came

up to .8 wilt within a half minute.

May 12.
The circuit was

2:04
2:04
2:05

SESaSa8a0

ro 09 89 HF DT OH WH

1.40
1010
1.03
290
82
78
76
oT
69
067
64
262

left open from May 10 to May iz.

000.
750.
760.
6350.
620.
590.
560.
540.
530.
610.
500.
480.
From May 12 until the time this date was taken
Which was about a week the cell was left open circuited.

 

Time EehieF. Curpvent

voita milii-

: amps.
1:30 1.46 000.
1:31 1244 000.
1:31 102 650.
1:38 Leiz 580.
1:40 i2.1 430.
1:45 95 445.
1: 50 90 460.
1:56 083 5S.
2:00 075 575.
2:06 e770 550.
2:10 068 §32.
2:15 65 520.
2:20 063 500.
2:25 61 460.
2:30 «60 475.
2:35 «59 460.

Lifter taking this data the cell was short oirocuited
until May 2l.

When at thie time the cirouit was opened and a
voltage reading taken, which waa 0.352 volt. |

The eleatrodes were then weighed again to determine
whether there had been any noticable shange.

Carbon rode = 4.5 ib.
Aoid and gar = 6.6 1b.
Plate of lead peroxide = 1.0 lb.

fhis indicates an inorease in weight of the carbon
but this mst have been due to the absorption of acid by
them. The aoid and the jar weigh .25 lb. less than at the
beginning of the experiment. There is no apparent change

in weight of the lead peroxide plate.
A large amount of the lead peroxide was however
off the plate and in the bottom of the jar was a grey
deposit which was probably lead sulphate with some
carbon. The carbon rods were partially decomposed
from the action of the eleotrolyte although the

results by weight show an inorease.

These experiments indicate that sleotricity can
be obtained from a cell in which carbon is one of the
sotive materials. Sulphuric acid in which was peroxide
of ochiorine was the only electrolyte found whic would

affect carbon.
INDEX

Bibliography - ------c- 7-7 rrr C7 Page 3.

Eleotrio Energy direct from Carbon - - -
By E. C. Kennelly.

Junger's Carbon Oell - -- ---+---+---

Jaques Carbon Cell ------------
Baurs Carbon Oxygen Cell ~ ----+-----

Electrolytic Desposition of Carbon ~ - - -
By Dr. Coehn.

A New Primary Battery in whioh Carbon is
Consumed- - - - ~- © = = + == = -
By Willard &. Case.

Experimmts -~ - -- - - a
Experiment #l- ----------+--+--

Mxperiment #2---------------

Experiment #3- --------------

Experiments with Sulphuric Acid Gell whose
Eleotrolyte Contains Peroxide ef
Chlorime- - ---+----+-+-+-++e-+--

?

7

12.
14.
16.

21.

28.

29.
~

 

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-- ee ee = He Iemt req:
------ - - ~&& toomtregs
Sw em eh S BR SHOP IETS

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re if etylorteos &
ee te ne ee ee  ~RabrOle

 

 

 
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