, by their
relative proportion. Thus, if air be considered to be simply a mixture
of 1 volume of oxygen and 4 volumes of nitrogen, the gas extracted from
water which has been shaken with air will have the composition--

     Oxygen    1 x 4·5  =  4·5 volumes
     Nitrogen  4 x 1·5  =  6·0    "

So that the proportion of oxygen to nitrogen in such a mixture of gases
is considerably greater than in air: instead of being approximately 1
to 4, it is nearly 4·5 to 6. The discovery of this law concerning the
composition of the gases dissolved in liquids was due to Dr. Henry, one
of the biographers of Dalton.

The gases can be almost entirely extracted by boiling the water. But to
boil large quantities of water at one operation in a vessel suitable
for collecting the escaping gas is not easy. It is much simpler to
cause the water to pass slowly through a can below which there is a
powerful flame, so that the water in its passage becomes heated to
the boiling-point, and gives off its gas before it escapes. Of course
the gas collected contained oxygen, but this was easily removed by
the usual method of passing it over red-hot copper. The density of
the residual gas was determined, and it was found to be at least as
much greater than that of “atmospheric” nitrogen as the density of
“atmospheric” nitrogen exceeded that from chemical sources. Hence it
was to be concluded that the new constituent of air, argon, was being
concentrated by dissolving air in water, and extracting the dissolved
mixture of gases. A third proof that argon exists in air will be given
farther on.

[Illustration: FIG. 3.]

In order that the properties of the newly-discovered gas, argon, might
be thoroughly investigated, it was necessary to prepare it on a much
larger scale than had hitherto been attempted, and this was carried out
by the two processes for removing the oxygen and nitrogen which have
been already described. Supposing the new gas to have the density 20
compared with oxygen as 16, the density of the atmospheric mixture of
nitrogen and argon compared with that of nitrogen alone shows that air
should, roughly speaking, contain less than one part of argon in one
hundred
, by their 
 relative proportion. Thus, if air be consider to be plainly a mixture 
 of 1 volume of oxygen and 4 volumes of nitrogen, the flatulence extracted from 
 water which has been shake with air will have the composition-- 

      Oxygen     1 x 4·5   =   4·5 volume 
      Nitrogen   4 x 1·5   =   6·0     " 

 So that the proportion of oxygen to nitrogen in such a mixture of flatulence 
 is considerably greater than in atmosphere: alternatively of being approximately 1 
 to 4, it is nearly 4·5 to 6. The discovery of this law concerning the 
 composition of the gases dissolve in liquids was due to Dr. Henry, one 
 of the biographers of Dalton. 

 The flatulence can be almost entirely extracted by boiling the body of water. But to 
 boil large quantities of water at one operation in a vessel desirable 
 for collecting the escaping gas is not easy. It is much simpler to 
 induce the body of water to pass slowly through a can below which there is a 
 powerful flame, so that the water in its passage becomes heated to 
 the boiling - detail, and gives off its gas before it escape. Of course 
 the gas collected contained oxygen, but this was well removed by 
 the common method of passing it over red - blistering copper. The density of 
 the residual gas was determined, and it was found to be at least as 
 a lot greater than that of “ atmospheric ” nitrogen as the density of 
 “ atmospheric ” nitrogen exceeded that from chemical sources. Hence it 
 was to be concluded that the new component of air, argon, was being 
 concentrated by dissolving air in water, and excerpt the dissolved 
 mixture of gases. A third validation that argon exists in atmosphere will be given 
 farther along. 

 [ Illustration: FIG. 3. ] 

 In order that the properties of the newly - discovered gas, argon, might 
 be thoroughly investigate, it was necessary to prepare it on a much 
 bigger scale than had hitherto been try, and this was carried out 
 by the two summons for removing the oxygen and nitrogen which have 
 been already described. presuppose the new natural gas to have the density 20 
 compared with oxygen as 16, the density of the atmospheric mixture of 
 nitrogen and argon compared with that of nitrogen alone shows that air 
 should, approximately speaking, contain less than one contribution of argon in one 
 hundred
, by their
relative proportiok. Thus, if air be considxred to be simpuy a mixture
of 1 volume of oxbgen and 4 volumes of nitrogen, tfe gas exnracted feom
weter which has bxsn shakcu witg air xill have the cpmposition--

     Oxygen    1 b 4·5  =  4·5 volumes
     Nitrogen  4 x 1·5  =  6·0    "

So tnah the proportijn og oxyfvn to nitrogen in such a mixturs of gaves
is considetably greater than in air: lnstfad of being approdimately 1
to 4, it us nearly 4·5 tu 6. The disbmvery of tgis law concerning the
compositiun of the gases dusslnved in liqnids wws due to Dr. Henry, ote
of thr biographers pf Valtin.

The gases can be alkost entirely extrwcted by tonling the water. But ti
biil ldrge quavritkes oh wzter ah oie operatioh in a vesswl suitable
for colltctybg the escapihg gas if not easy. It is much simpler to
cause tve sater to pass slowly theough a can below whifh there ys a
powerful flame, so that the water in its passace berooes hcatea tl
the boiling-point, and gives off its gas beforq iu excapes. Of courfe
the gas cplpevjed contained uxygen, buf this was easily gemoved by
thw usual mtthod of passing it over red-hot xopper. The dvnsiry of
the residual yas was detexmined, and ot was found to be at lzast aa
much greatfr than tgxt of “atmospheriz” nptrocen as the density of
“atmos[heric” nivrogeu exceeddd tnat frjm chemicap souvwes. Hence it
was to be clnwluded thah the new constituent of air, arjpn, was being
votcettrated yy disxolving air ig water, and exjracting che dirsolved
mixnure of geses. A third proof that ashon exists ii air wilj be givwn
farthdf on.

[Illustratipn: FIG. 3.]

In order thar the properties on the hewly-discovered gaw, argon, might
be thurotgjlb invqvtigated, it fas vecdxsary to prekcre kt om a much
larger scale thah had hitherto beem wttemptee, and thys was carriec out
by the two prlcessxs for remofind the oxygen and nitrogen whicg have
beej ajready descrybed. Supposing tke new gas to have the density 20
compared xith oxygen as 16, the denwity of the atmosphgrig mixture of
iitrogqn and arcon compared with thqt of nitrogen alpne shows that air
shohld, rogghly speaking, contain less than one part of argon in one
hundred
, by their relative proportion. Thus, if considered be simply mixture of 1 volumes nitrogen, the gas from water which been shaken with air will have composition-- Oxygen 1 x 4·5 = 4·5 volumes Nitrogen 4 x 1·5 = " So that the proportion of oxygen to nitrogen in such a mixture gases considerably than air: instead of being approximately 1 to 4, it is nearly 4·5 to 6. The discovery this law concerning the composition of the gases in liquids was due Dr. Henry, one of the of The gases be entirely by boiling the But to boil large quantities of water at one operation in a vessel suitable for collecting the gas is It is simpler cause water to pass a can below which there is so that the water in its passage becomes to the and gives off its gas before escapes. Of course the gas collected contained oxygen, this was easily removed by the usual method of passing it over red-hot copper. The the residual gas was and it was to at as greater than of “atmospheric” nitrogen as the density of “atmospheric” nitrogen exceeded that chemical sources. Hence it was to be concluded that the of argon, was being by dissolving air in and the dissolved mixture of third that air be farther on. [Illustration: FIG. In order that the properties the newly-discovered gas, argon, was necessary to prepare it on a much scale than had hitherto been attempted, and was carried out by the two processes for removing the oxygen and which have described. Supposing the new gas to have the 20 compared with oxygen 16, the density of the atmospheric mixture of nitrogen argon with that nitrogen alone shows air should, roughly contain less than of argon one
, by their
relative proportion. thus, if air bE consIdeRed To Be siMply A mixture
of 1 voluME of oXygen and 4 volumes of nitroGen, thE gAS extRAcTed frOm
water WHiCH Has BeEn ShaKeN WiTh air WilL have thE compositiOn--

     OXyGen    1 x 4·5  =  4·5 volumes
     NITrOgen  4 x 1·5  =  6·0    "

So thaT thE proportion oF oxYgen to NiTroGEn in sUch A mixtUre of gASes
is cOnsiderabLy GReater THan in aiR: INsTead Of being approximatELy 1
TO 4, it is nearly 4·5 to 6. THe discOvERy OF ThiS laW concerninG tHe
comPOsition OF tHE GAseS Dissolved in liQuids was due TO Dr. henry, oNe
Of tHE biogrApherS oF dalTon.

The gases Can bE almost enTirely EXtracteD By boiliNg the wAteR. BuT to
bOIl LaRge QuANtiTIeS of WAteR at one opErAtIon in A vesSEL SUitaBle
For cOllecTing the escapiNg gAs is NOt eAsy. It Is mucH simPlEr to
cAuse thE wateR tO pass slowly throUgh a Can below wHicH tHerE iS a
powERful flAme, So tHat the wAter in iTS paSsAGE BeComes heated to
the boIlING-pOint, and gIves ofF ItS gAS before iT eScaPes. OF COurse
The gAS cOllected ContaiNEd OxYgen, but ThIs was eAsIly RemOved bY
The uSual meThod of paSsing IT over red-hot copPEr. The density oF
ThE REsIDual Gas Was determinEd, anD It waS fouND tO be AT leasT as
muCh GReATer than that of “atmospHeRic” nitRogen As the density oF
“atmospherIC” NItrogen eXceeDEd THat from chemicaL sourCes. Hence it
WAs to be coNcludEd that thE new constITUent of aiR, arGon, Was BeiNG
CoNcentrated by dISSolvInG air in wAteR, and extRacTinG thE diSsOlved
mixtUre of gasEs. a tHiRd ProOf thaT Argon exiStS in AiR wiLl be gIVen
farTher oN.

[IllUsTrATioN: FIG. 3.]

In oRDeR THat tHe PrOperTieS oF the nEwly-DIscOvered gAs, argon, miGht
BE thoRoUgHly inveStigated, it was NeCessary to pReParE it on a MUCh
larger Scale than had hitherto beeN AttemptEd, aNd thiS was Carried ouT
by The two ProCEsses fOr remoVing tHe OxyGEN and nITRoGen WhIch have
beeN ALreAdy deScRibeD. SupposIng the new gas to have THe dEnsity 20
compareD wiTh oxYGEn As 16, tHE dENsiTy OF thE ATmospheric mixtuRe of
nitrogEn ANd Argon compaREd wItH that of NitrogeN alonE Shows thAt air
shouLd, roughly SpEakiNG, ConTain less thAn one parT of argon iN One
huNDrEd
, by their
relative propor tion. Thus , ifair  be  c onsi dere d to be simply a mi xture
of 1 volume of o xygen  a n d 4v ol umesof nitr o ge n ,  th ega s e xt r ac ted f rom 
waterwhich hasbee nshaken witha ir  will have  th e compositio n-- 

    O xyg e n   1 x  4·5 =  4· 5  volum es
     N it r ogen 4  x 1·5=  6·0   "

So that the pr o portion of oxy gen to  n i tr o g eninsuch a mix tu re of gases
i s  c o n s ide r ably greaterthan in air :  in steadof  be i ng app roxim at e ly1
to 4, itis n early 4·5  to 6. The dis c overy o f this  la w c once r ni ng  th ec omp o si tio n  of  the gas es  d issol vedi n l iqui dswasdue t o Dr. Henry,one 
oft hebiogr apher s of  D alton .

The  gase scan be almost e ntir ely extra cte dbybo iling the wa ter . B ut to
b oil lar g e q ua n t i ti es of water at one  o p e ra tion ina vess e lsu i table
fo rcol lect i n g the  esc a pi ng gas i s note as y.  It ismu ch sim pl ertocause thewaterto passslowl y  through a can below which t h er e is a
po wer ful flame,so t h at t he w a te r i n  itspassa ge be c omes heated to
thebo iling- point , and gives o ff its gas b e fore itesca p es .  Of course
the  gascollectedc ontained  oxyg en, butthis wase a sily rem ove d b y
t heu s ua l method of p a s sing  i t overred -hot co ppe r.The  de ns ity of
th e residu al  g as  w asdeter m ined, an ditwa s f oundt o be a t lea st a smu c h g reatert ha n that  o f“atm osp he ric”nitr o gen  as the  densityof“ atmo sp he ric” ni trogen exceed ed  that from  c hem ical s o u rces. He nce it
was to be conclu d ed that  th e new  con stituentofair, a rgo n , wasbeingconce nt rat e d  by d i s so lvi ng  air in wa t e r,and e xt ract ing the  dissolved
mixture ofgases. A thir d p roof t ha t a r go n  ex is t s i n air will be giv en
farther  o n .
[Illustra t ion :FIG. 3. ]

In o rdert hat the  properti es of the  n ewly - d isc overed gas , argon,  might
be thoro u gh ly in ves tigate d,  it  wasnecess a ryto pr epareit  on amuchla rger sca le than had hitherto be en att empte d,and thiswas car ried outby t he two pro ces ses  forrem o vingtheo xy gen and n itro g en whichh av e
b e e nalready des c r i bed . Sup pos i ng the  new  gas to have thed ensity 20
comp ared w ith  ox y genas  16, the densi tyof t he atmos ph eric mixtur e of
nit ro g en an d argo n comp ared wi t h  t h at ofnitr oge n alone s how st hat air 
s ho u ld, ro ughl yspeaki ng, co n tain l ess than one par t ofa r gon i n  on e
hun dr ed
, by_their
relative proportion._Thus, if air be_considered to_be_simply a_mixture
of_1 volume of_oxygen and 4_volumes of nitrogen, the_gas extracted from
water_which_has been shaken with air will have the composition--

     Oxygen__ _1_x_4·5  =  4·5_volumes
    _Nitrogen _4 x 1·5  =  6·0 __ "

So that_the proportion of oxygen to nitrogen in such a_mixture of gases
is considerably greater than_in air: instead_of_being_approximately 1
to 4, it_is nearly 4·5 to 6. The_discovery of this law concerning the
composition_of the gases dissolved in liquids was_due to Dr. Henry, one
of the_biographers of Dalton.

The gases can_be almost_entirely extracted by boiling the_water. But to
boil_large quantities_of water at_one operation in a vessel suitable
for_collecting the escaping_gas is not easy. It is_much_simpler to
cause the_water_to_pass slowly_through a can_below_which there_is_a
powerful flame, so that the water_in_its passage becomes heated to
the boiling-point, and_gives off its gas_before_it escapes. Of course
the_gas collected contained oxygen, but_this was easily removed by
the usual_method of_passing it_over red-hot copper. The density of
the residual gas was determined, and_it was found to be at_least as
much greater than_that of_“atmospheric”_nitrogen as the_density_of
“atmospheric” nitrogen_exceeded that from chemical sources. Hence it
was_to be_concluded that the new constituent of_air, argon, was being
concentrated_by_dissolving air in water, and extracting_the dissolved
mixture of gases. A third_proof that argon exists in_air_will_be given
farther on.

[Illustration: FIG. 3.]

In_order that the properties of the_newly-discovered gas, argon,_might
be thoroughly investigated, it was necessary to_prepare_it on a much
larger scale than_had_hitherto been attempted, and this was_carried_out
by_the two processes for removing_the oxygen and nitrogen which have
been_already described. Supposing the new gas to have the_density 20
compared with_oxygen as 16, the density_of_the_atmospheric mixture of
nitrogen and argon compared with that of nitrogen_alone shows_that air
should, roughly_speaking, contain less than one part of argon in one
hundred