Improvements in the Recovery of Chlorine from the Residual Liquors of the Ammonia-soda Process, from Solutions of Calcium Chloride, from Certain Impure Solutions of Magnesic Chloride, and from some other Industrial Residues.
Year: 1889

page_text: Date of Application, 30th Oct., 1889
Complete Specification Left, 30th Aug., 1890-Accepted, 4th Oct., 1890
PROVISIONAL SPECIFICATION.
Improvements in the Recovery of Chlorine from the Residual
Liquors of the Ammonia-soda Process, from Solutions of Calcium
Chloride, from Certain Impure Solutions of Magnesic Chloride,
and from some other Industrial Residues.
We, FARNHAM MAXWELL LYTE, of 60, Finboro' Road, in the County of Middlesex
Analytical Chemist, and JAMES GRAHAM TATTERS, of The Manse, Runcorn, in the
County of Chester, Analytical Chemist, do hereby declare the nature of this invention
to be as follows:-
The object of this invention is the production, in the free state, of the whole of the
chlorine contained in the sodic chloride which has taken part in the ammonia-soda
process; in the magnesic chloride contained in the mothers of saltworks, and the
liquor from the treatment of carnallite; and in the hydrochloric acid from the Leblanc
process, etc., by the formation of either of the anhydrous magnesic oxychlorides.
A method for producing an anhydrous magnesic oxychloride is by combining dry
magnesia with the fused or powdered anhydrous magnesic chloride. This latter may
have been produced in the ordinary way from the ammonic-magnesic double salt,
ammonic chloride being volatilized, or by any other method.
The apparatus may be so disposed as to condense the ammonic-chloride, when it may
be employed over again, either in the treatment of the waste liquor from the ammonia-
soda process or in that of the magnesic solutions alluded to, etc., for the recovery from
them of chlorine in a free state.
We will take for example the treatment of the ammonia-soda waste liquors and shew
how, from them, the pure double salt may be continually regenerated.
Suppose that we have any given quantity of the liquor which has been distilled with
lime. This is to be concentrated by evaporation till, on cooling to ordinary temperatures,
the calcic chloride it contains would form a saturated solution, or till the boiling point
rises to 110° C. or 111° C. Most of the sodic chloride will deposit during evaporation
and the rest separates on allowing the liquor to cool and repose. This depends on
the insolubility of sodic chloride in a saturated solution of calcic chloride at ordinary
temperatures, but wo are not aware that the reaction has ever been applied to this
separation. Potassic chloride may also be separated from calcic chloride in the same
way, but rather less completely.
By this same method, sodic chloride may be separated from the magnesic chloride
solutions above mentioned, but hardly so perfectly and it is important to get rid of as
much of the sodic or potassic chlorides as possible, as they are liable to accumulate in
the magnesic chloride about to be formed. Sufficient magnesia having now been added
to the purified solution of calcic chloride, diluting it also at the same time with water,
till the specific gravity falls to 12445 at 15° Centigrade, it may, as is known, bo
converted, by means of carbonic dioxide or sulphuric acid, into a solution of pure
magnesic chloride. A sufficient amount of this solution being taken and the ammonic
chloride which was separated from the double salt by sublimation and which was collected,
being added to it a pure solution of the same double salt, of like amount and composition
to that we had at first is the result and it only requires to be evaporated to dryness and
desiccated to be recovered in the anhydrous state, fitted for a new production of the
anhydrous magnesic chloride and volatilization of sal-ammoniac and this may of course,
be repeated ad infinitum.
The anhydrous magnesic chloride produced in this, or any other, way being pounded
and mixed with a sufficiency of dry magnesia, say half its weight, and having been
agglomerated by heating in a close vessel, will form an oxychloride which may be
used in the ordinary manner to generate chlorine.

page_text: By the present method, Pechiney only recovers 40·14 per cent. of its chlorine in a
free state from his oxychloride,, where we, on the contrary; from our dry oxychloride
recover sixty per cent.
Professor Dewar says, on page 786, Journal Society Chemical Industry, Volume VI,
in his paper, to which we are indebted for statistics as to the cost of the Weldon-
Pechiney oxychloride process, that bleach as manufactured by it and that made by the
old Weldon process, even after taking account of all the costly plant used in the
former, cost the same price and, as by our method all the expense of drying (fully one
half the cost) will be done away with, it is fully evident that a saving will be effected
of over one-third on the present cost of manufacture. Besides this, there are the facts
that we are enabled to utilize the waste liquors of the ammonia-soda process, which has
never yet been done satisfactorily, and that we can have no cooling of the furnace by
the evaporation of the water, which Pechiney's oxychloride contains, as our oxychloride
is anhydrous.
All three
According to Solvay, anhydrous magnesic chloride alone may also be used to generate
chlorine. It may be fused in crucibles, air or oxygen being blown through or over
it or the fused salt may be sprayed into a current of heated air or oxygen.
of these are included in Solvay's patent. The crucibles used for this purpose may be
made with lateral openings, like the fishing or boiling down pans of alkali works or
on the principle of certain bird glasses so that the magnesia formed may be scraped
to one side and withdrawn, while by their shape they will, if kept sufficiently full,
prevent the escape of the chlorine generated. The crucibles, if of cast or wrought
iron, should have a basic lining to protect them from the chlorine evolved. One of
magnesia itself may be used or the crucibles may be made of any convenient material.
Probably cast iron lined as prescribed with a head, if not also of iron, of plumbago
will be found to answer. The same air may be made to pass through a succession of
such crucibles so as to obtain the strongest possible chlorine.
In treating the other liquors mentioned, and in fact any solutions of magnesic
chloride contaminated with sodic chloride, the above process may be varied as follows:
the whole of the magnesia may be precipitated by an addition of lime, the calcic
chloride solution which is formed purified from sodic chloride and diluted as before,
the precipitated magnesia after being washed (to get rid of Na Cl) returned to the
liquor and carbonic dioxide being passed all the time will be thrown down as calcic
carbonate and the magnesic chloride reconstituted in a pure state. The solution of
ammonic chloride necessary for the constitution of the double salt may also be made
by adding ammonic sulphate to the purified solution of calcic chloride after the
necessary dilution. It only requires to be made in this way, however, once for all as
it will always be able in future to be recovered each time it is volatilized and to be used
over again, only requiring to be dissolved in the necessary quantity more of the
magnesie chloride solution in order to constitute another similar lot of double salt.
There is another way of working which we will now describe, but it is hardly so
easy as the one just given.
In treating the dry ammonic-magnesic double chloride Mg C₁₂ (NH, CI), with
magnesia in order to evolve ammonia and form magnesic chloride or oxychloride, some
water is formed and remains occluded with the magnesic salt thus
My Oh, (NH)2 + Mg C = 2 Mg C₁₂ + 2 NH3 + H₂ ♥.
The occluded water may not be quite as much as here indicated, but still it is very
great. In this reaction, the temperature to which the mixture is heated should not be
carried beyond 300° C. or thereabouts, and when subsequently the product is exposed
to a higher temperature, say to 400° C. or 500° C., hydrochloric acid and magnesia are
formed, thus destroying part of the magnesic chloride. The decomposition due to the
occluded water, however, may equal, but cannot at the most exceed, that of half the
magnesic chloride formed. This latter reaction is thus formulated :-
2 M Cl + H. O = MỠ CL + No 0 ± 2 H CL
2 IS
The occluded water may not be quite as much as here indicated, but still it is very
great. In this reaction, the temperature to which the mixture is heated should not be
carried beyond 300° C. or thereabouts, and when subsequently the product is exposed
to a higher temperature, say to 400° C. or 500° C., hydrochloric acid and magnesia are
formed, thus destroying part of the magnesic chloride. The decomposition due to the
occluded water, however, may equal, but cannot at the most exceed, that of half the
magnesic chloride formed. This latter reaction is thus formulated:

page_text: ay be conducted in a closed iron vessel, as no chlorine is disengaged, provided
ll air or oxygen be carefully excluded and neither anhydrous hydrochloric acid nor
mmonia have any action on hot iron. By this second heating, if the fusing point of
nhydrous magnesic chloride is attained, the magnesic chloride and the magnesia
ormed will either fuse partially into a chloride or agglomerate entirely into an
xychloride according to the amount of magnesia present. The formula of the
xychloride produced, even if all the water formed has been occluded (which is
ardly probable) MgO or 2 Mg O and Mg Cl 2 (NH, Cl), having been used, will
e Mg Cl, Mg O or 2 Mg O and this may be employed to generate chlorine in the
sual way, by passing over it air or oxygen while it is maintained in a heated state.
The hydrochloric acid formed will tend to vary slightly in quantity, according to
circumstances, but at most only one molecule of water for every two molecules of
ammonic chloride is all that can be formed, only one out of the two molecules of
magnesic chloride left after the distillation of the ammonia, being all that can be
decomposed, the other molecule remaining to forin with the magnesia which remains
an anhydrous magnesic oxychloride from which chlorine may, as just stated, be
evolved. Let us suppose, that in the present instance, this extreme of decomposition
does take place; the reaction will be represented by the formula given above. The
hydrochloric acid will be gaseons and anhydrous, if the double salt has been properly
dried, and it may be employed in any of the cases where the use of dry hydrochloric
acid is deemed advisable, in the Deacon process for the manufacture of chlorine for
instance, or,
when condensed in a milk of magnesia it should be just sufficient to
reconstitute the molecule of magnesic chloride which has been destroyed. The
magnesia remaining from a previous generation of chlorine may be used for this.
Call the solution of magnesic chloride thus produced No. 1.
On the other hand distil any convenient amount of the residual liquor of the
ammonia-soda process in the usual way with lime, and condense the ammonia
which passes in cold water. The calcic chloride solution so obtained is to be purified
from sodic chloride as previously described, and then drawn off and sufficiently
diluted. The ammoniacal water in which the ammonia has been condensed is now
to be returned to this purified solution of calcic chloride and if sufficiently diluted
by this it may be converted by carbonic dioxide, etc., as before, into calcic carbonate
or sulphate and a solution of ammonic chloride. Otherwise, the liquor having been
evaporated to dryness, pure ammonic chloride may be separated from the residue
by sublimation. Call this, whether it be a solution or the solid ammonic chloride, No. 2.
A stock of this should be prepared and kept on hand.
Add now to No 1 so much of No. 2 that the resulting solution shall contain
for every. two molecules of ammonic chloride one molecule of magnesic chloride or
in other words so that there shall be as much chlorine attributable to the ammonium
A solution is thus formed of the
as that which is attributable to the magnesium.
ammoniac magnesic double chloride Mg Cl, (NH, Cl), similar both in point of
composition and in quantity to that originally treated and it only requires to be
evaporated to dryness, pulverized, and desiccated, in order to be put through the
same cycle of operations as before.
The same result may also be obtained if after eliminating the sodic chloride as
far as possible from a solution of magnesic chloride by concentration and cooling,
we add to it sufficient ammonia to precipitate half the magnesia. The magnesic
hydrate obtained by means of ammonia, lime, or any other such precipitant, is
eminently fitted for all the uses which require the magnesia to be of the easily
soluble form such as is that burnt at a low temperature. The large amount of
ammonic chloride entering into the constitution of the double salt used both in this
and in the former process is used in order to give the double salt increased
stability during evaporation and desiccation, but possibly a less amount may be
found to answer.
By a succession of such operations, the whole of the chlorine contained in the
sodic chloride which has taken part in the ammonia-soda process may also be

page_text: made to take part in the constitution of the double salt, and so may be ultimately
recovered in the free state, the double salt itself being continually regenerated.
The plain ammonic chloride recommended by Berzelius to be used mixed with
magnesia for the production of anhydrous magnesic chloride, may also be treated
in this manner with corresponding results, but hardly perhaps with the same
advantage.
The whole of each set of operations, then, although, by the description the
process may have appeared long, only really involves one evaporation to form the
dry double salt, one heating of that double salt with magnesia to evolve aminonia
and hydrochloric acid, and one heating of the oxychloride to generate chlorine,
besides one or two manipulations, scarcely worthy of consideration as a matter of
expense.
Of course, this process as well as the one first described may also be applied to
the production of chlorine from the hydrochloric acid produced in the Leblanc
process, but scarcely perhaps so advantageously. The following is an example of one
of the ways of applying it which, however, differs very little from that already given.
The necessary quantity of acid having been taken, half of it is to be neutralised with
magnesia or magnesite. This will form solution No. 1 as above. The other half is
to be neutralised with ammonia, or with lime and ammonic sulphate added.
will form a solution corresponding to No. 2 above. The two solutions, when clear,
may be mixed. Thus will be formed a solution of the double salt of the desired
composition and from it ammonia, hydrochloric acid, chlorine, and magnesia, may
be successively produced as already explained, the double salt being continually
regenerated.
This
This process may also be varied by neutralizing the hydrochloric acid, evolved in
the course of the decomposition of the double salt, with the ammonia which had been
previously expelled from that same salt and adding magnesia instead of ammonia to
the purified solution of calcic chloride before gassing. By mixing these in the right
proportions, a solution of pure ammonic-magnesic double chloride is also obtained
and it need only be evaporated and dried to be proceeded with as before.
Indeed, several such variations of this process may be devised but as they are only
for the most part modifications in the order of adding the reagents or some such
simple change and as they all result in the formation of this double salt which forms
the basis of these two processes, they would only involve useless repetition.
Dated this 30th day of October 1889.
COMPLETE SPECIFICATION.
Improvements in the Recovery of Chlorine from the Residual
Liquors of the Ammonia-soda Process, from Solutions of Calcium
Chloride, from Certain Impure Solutions of Magnesic Chloride,
and from some other Industrial Residues.
We, FARNHAM MAXWELL LYTE, of 60, Finborough Road, in the County of
Middlesex, Analytical Chemist, and JAMES GRAHAM TATTERS, of The Manse,
Runcorn, in the County of Chester, Analytical Chemist, do hereby declare the
nature of this invention and in what manner the same is to be performed, to be
particularly described and ascertained in and by the following statement:-
The object of this invention is the production in the free state of the whole or
nearly the whole of the chlorine contained in the calcic chloride resulting from the
ammonia-soda process, in the magnesic chloride contained in the mother liquors of
salt works and the liquor from the treatment of carnellite, and in the hydrochloric

page_text: acid or caleic chloride from the Leblanc or Weldon processes respectively. This we
accomplish by the repeated formation of anhydrous ammonic-magnesic double chloride
and the production therefrom of an anhydrous magnesic oxychloride, of varying
composition, from which the chlorine may be generated in the ordinary manner.
We will take, for example, the treatment of the ammonia-soda waste liquors
and show how, from them, ammonic-magnesic double chloride may be continually
regenerated.
According to one mode of working, we take anhydrous ammonic-magnesic double
chloride and from it we produce anhydrous magnesic chloride in the ordinary way,
ammonic chloride being volatilised and condensed for use in the reconstitution of the
double salt, as hereafter described. Suppose, now, that we have any given quantity
of the liquor which has been distilled with lime, and consisting chiefly of calcic and
sodic chloride. This is to be concentrated by evaporation, till, on cooling to ordinary
temperatures, the calcic chloride it contains would form a saturated solution, or till
the boiling point rises to 110° C. or thereabouts. Most of the sodic chloride will
deposit during evaporation and the rest separates on allowing the liquor to cool and
repose. This depends on the insolubility of sodic chloride in a saturated solution of
calcic chloride at ordinary temperatures, but we are not aware that the reaction has
ever been applied to this separation. Evaporation by multiple effect will here be a
great economy.
Sufficient soft burnt magnesia having now been added to the purified solution of
calcic chloride, diluting it also at the same time with water till the specific gravity
falls to about 1-2445 at 15° C., it may, as is known, be converted by means of carbonic
dioxide into a solution of pure magnesic chloride. A sufficient amount of this
solution being taken and the ammonic chloride (which was separated from the double
salt by sublimation, as above mentioned, and which was collected) being added to it,
a pure solution of the same double salt, of like amount and composition as we had at
first, is the result, and it only requires to be evaporated to dryness and desiccated to
be recovered in the anhydrous state, and from this a fresh batch of anhydrous magnesic
chloride may be obtained by volatilizing the ammonic chloride as first above described.
This may, of course, be repeated ad infinitum.
The anhydrous magnesic chloride having been fused or ground and mixed with a
sufficiency (say half its weight) of dry magnesia (obtained from a previous generation
of chlorine) and having been agglomerated by heating in a closed vessel, will form
anhydrous magnesic oxychloride which may be broken up and used in the ordinary
manner to generate chlorine.
By the method at present in use Pechiney only recovers on the first intention
40.14 per cent. of the chlorine in a free state from his oxychloride; we, on the
contrary, from our dry oxychloride recover 60 per cent., or thereabouts.
We are thus enabled to utilize the waste liquors of the ammonia-soda process which
has never yet been done satisfactorily, and we have no cooling of the furnace used to
generate the chlorine by the evaporation of the water which Pechiney's oxychloride
contains, our oxychloride being anhydrous.
In treating the impure magnesic chloride contained in the mother liquors of salt
works, and the liquor from the treatment of carnallite, the above described process is
to be preceded by a preliminary operation having for object to produce a pure calcic
chloride solution, from which pure magnesic chloride may be obtained, as before
described. We first precipitate the whole of the magnesium contained in the mother
liquor as Mg O by the addition of lime. The resulting calcic chloride solution
decanted off is then purified from sodic (or potassic) chloride by concentration, as
before described, and diluted whilst the precipitated magnesia is washed (to get rid of
sodic, or potassic, chloride) and returned to the purified solution. Carbonic dioxide
being now passed, all the lime will be thrown down as calcic carbonate and the
magnesic chloride reconstituted in a pure state. With this pure magnesie chloride
we produce ammonic-magnesic double chloride from which to obtain by sublimation
ammonic chloride for reconstituting the double salt with more pure magnesic chloride

page_text: and anhydrous magnesic chloride wherewith to form anhydrous magnesic oxychloride
for the generation of chlorine therefrom, all as before described.
There is another way of working which we will now describe, and this is the most
important. It has the advantage that iron vessels may be used. Calcic chloride
which has been purified by separation from sodic chloride, as described in the first
mode of working, is converted into ammonic chloride by saturation with ammonia and
-carbon dioxide, calcic carbonate being precipitated. The ammonic chloride thus
prepared is mixed with sufficient magnesic chloride (obtained by introducing the
hydrochloric acid liberated at the formation of a previous batch of oxychloride into
a milk of magnesia) and evaporated to dryness. The dry ammonic-magnesic double
chloride Mg Cl, (NH, C), thus formed is heated with magnesia in order to evolve
ammonia and form magnesic chloride. Some water is here formed and remains
occluded with the magnesic salt, thus-
Mg Cl₂ (NH, Cl)2 + Mg O = 2 Mg Cl, + 2 NH3 + H, 0.
In this reaction, the temperature to which the mixture is heated should not be
carried beyond 300° C. or thereabouts and when subsequently the product is exposed
to a higher temperature, say to 400° C. or 500° C., hydrochloric acid and magnesia
are formed, thus destroying part of the magnesic chloride. This latter reaction may
be thus formulated, supposing all the water formed to be occluded-
2 Mg Cl₂ + H, O
=
Mg Cl, Mg 0 + 2 H Cl
The heating for this, as well as for the former, reaction may be conducted in a
closed iron vessel, as no chlorine is disengaged, provided all air or oxygen be carefully
excluded, as neither anhydrous hydrochloric acid nor ammonia have any action on
hot iron. The presence of a small excess of magnesia, and keeping the mixture
stirred, facilitates the operation. By this second heating, if the fusing point of
anhydrous magnesic chloride is attained, the magnesic chloride and the magnesia
formed will agglomerate entirely into an oxychloride, varying in composition
according to the amount of magnesia present. The oxychloride formed may be
employed to generate chlorine, in the usual way, by passing over it air or oxygen
while it is maintained in a sufficiently heated state.
The hydrochloric acid formed (as shewn by the above equation) will tend to vary
slightly in quantity, according to circumstances, but at most one molecule of water
for every two molecules of ammonic chloride is all that can be formed and only one
out of the two molecules of the magnesic chloride left after the volatilization of
the ammonia can be decomposed, the other molecule remaining to form with the
magnesia which remains, an anhydrous magnesic oxychloride, from which chlorine
may, as just stated, be evolved. The hydrochloric acid will be gaseous and anhy-
drous, if the double salt has been properly dried and when condensed in a milk
of magnesia it should be about sufficient to reconstitute the molecule of magnesic
chloride which has been destroyed. The magnesia remaining from a previous
generation of chlorine may be used for this
By a cycle of such operations nearly the whole of the chlorine contained in the
calcic chloride left from the ammonia-soda process may be made to take part in
the constitution of the double salt, and so may be ultimately recovered in the free
state; while the double salt itself may be continually regenerated, by utilizing the
ammonia and the hydrochloric acid which were successively disengaged when the
previous batch was heated with magnesia.
The whole of each set of operations then, although by the description the process
may have appeared long, only really involves one evaporation to form the dry
double salt, one heating of that double salt with magnesia to evolve aшimonia and
hydrochloric acid, both of which may be used over again, and one heating of the
oxychloride to generate chlorine, besides one or two manipulations scarcely worthy
of consideration as a matter of expense.
It will be evident that this process, as well as the one first described, may also

page_text: be applied to the hydrochloric acid produced in the Leblanc process and to the
calcic chloride from the Weldon process but scarcely perhaps so advantageously.
The following is an example of one of the ways of applying it to hydrochloric acid
which however, differs very little from that just given. The necessary quantity of
acid having been taken, half of it is to be neutralized with magnesia or magnesite.
The other half is to be neutralized with ammonia. The two solutions when clear may
be mixed. Thus will be formed a solution of the double salt of the desired composition
and from it, ammonia hydrochloric acid and magnesic oxychloride are successively
produced, as already explained, the oxychloride yielding chlorine and magnesia which
with the ammonia is used for neutralising more hydrochloric acid and continually
reconstituting ammonie-magnesic double chloride.
Many variations of this process may be devised but as they are only for the most
part, modifications in the order of adding the reagents or some such simple change
and as they all result in the formation of this double salt which forms the basis of
these two processes, a description of these modifications wouid only involve useless
repetition.
Having now particularly described and ascertained the nature of the said inven--
tion and in what manner the same is to be performed, we declare that what we
claim is;
1. In the recovery of chlorine from waste chloride liquors, the systematic and con-.
tinuous regeneration of anhydrous ammonic-magnesic double chloride, (in order to
produce anhydrous magnesic chloride therefrom) by obtaining pure magnesic chloride.
from the waste liquor and mixing it with the ammonic chloride volatilised from a
previous batch of the double salt, substantially as specified.
2. In the recovery of chlorine from waste chloride liquors the systematic and con--
tinuous production of anhydrous magnesic oxychloride and regeneration of ammonic-
magnesic double chloride, by converting the calcic chloride (contained in, or obtained
from, the waste liquor) into ammonic chloride, mixing therewith pure magnesic
chloride to form the double salt, heating the dry double salt with magnesia to produce-
magnesic chloride (and ammonia for treating the next batch of calcic chloride) heating
the magnesic chloride to form anhydrous magnesic oxychloride and hydrochloric
acid, and condensing the latter with magnesia to form magnesic chloride for treating
the next batch of ammonic chloride, substantially as specified.
3. In the herein described process of recovering chlorine from waste chloride
liquors, as specified in Claim 2, the formation of a solution of ammonic chloride from
a solution of the purified calcic chloride by treatment with ammonia and carbonic-
dioxide, substantially as specified.
4. In the herein described processes of recovering chlorine from waste chloride
liquors, the herein described method of purifying solutions of calcic chloride when
they are contaminated with sodic or potassic chloride, which consists in evaporating
them to such a point that the liquor when cooled will be a saturated solution of the
earthy salt and most of the sodic or potassic chloride will be deposited, the rest.
separating after a short period of cooling and repose, as specified.
5. In the herein described processes of recovering chlorine from waste chloride
liquors, the herein described method of eliminating the alkaline chlorides contained in
impure solutions of magnesic chloride and of obtaining a solution of pure magnesic
chloride, which consists in precipitating the magnesia with lime, purifying the calcic
chloride so formed by the method specified in Claim 4, washing the precipitate and
returning it to the purified calcic chloride, diluting the latter and reconverting it, by
carbonic dioxide, into a solution of pure magnesic chloride.
6. In the recovery of chlorine from the hydrochloric acid produced by the Leblanc
process, converting the acid partly into magnesie and partly into ammonic chloride to.
form ammonic-magnesic double chloride and treating the double salt as herein
described and claimed under Clause 2, to successively form ammonia, magnesic oxy--
chloride, hydrochloric acid, and magnesia, as, and for the purpose, specified.

page_text: 7. The economic production of chlorine from solutions of calcic chloride or from
hydrochloric acid, by the combination of the different steps or processes and chemical
operations and reactions hereinbefore described and set forth.
Dated this 20th da at tum1800
F. MAXWELL LYTE.
J. G. TATTERS.
By A. M. & Wm. Clark,
53, Chancery Lane, London, Patent Agents.