,
divided by the pressure.

Similar experiments with argon led to the same result as Kundt and
Warburg found for mercury gas; but the calculation becomes more
simple if it is allowable to take for granted that the elasticity,
or alteration of pressure produced by unit alteration of volume, is
identical in the case of argon and air. The full equations are--

                               __________________________
     _n_λ_{air} = _c__{air} = √γ(_p_/_d_)(1 + _at_)_{air},

and

                                   ____________________________
     _n_λ_{argon} = _c__{argon} = √γ(_p_/_d_)(1 + _at_)_{argon},

where _n_ is the number of vibrations per second, =λ= the
wave-length of sound, and _a_ the coefficient of the expansion of a
gas for a rise of 1° in temperature, _t_, viz. 0·00367. Now if the
expression _p_ (1 + _at_) can be shown to be identical for argon and
for air, the value of =γ= for argon can be calculated by the very
simple proportion--

     λ^{2}_d__{air} : λ^{2}_d__{argon} :: 1·408 : γ_{argon}.

This involved a measurement of the rate of rise of pressure of argon,
_p_, per degree of rise of temperature, _t_; or, in other words,
the verification of Boyle’s and Gay-Lussac’s laws for argon; and
this research was successfully carried out by Dr. Randall of the
Johns Hopkins University of Baltimore, U.S.A., and Dr. Kuenen, of
Leyden, working in Professor Ramsay’s laboratory.[29] They made use
of a constant volume thermometer, and measured the rise of pressure
corresponding to a definite rise of temperature, comparing the gases
argon and helium in this respect with air. The values found between 0°
and 100° for air, argon, and helium were--

    One volume air, heated from 0° to 100°, raises
          pressure in the proportion of 1 to         1·3663
    Argon                                            1·36
, 
 divided by the pressure. 

 Similar experiments with argon lead to the like result as Kundt and 
 Warburg found for mercury accelerator; but the calculation become more 
 simple if it is allowable to accept for granted that the elasticity, 
 or alteration of press produced by unit revision of volume, is 
 identical in the case of argon and atmosphere. The wide equations are-- 

                                _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ 
      _ n_λ_{air } = _ c__{air } = √γ(_p_/_d_)(1 + _ at_)_{air }, 

 and 

                                    _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ 
      _ n_λ_{argon } = _ c__{argon } = √γ(_p_/_d_)(1 + _ at_)_{argon }, 

 where _ n _ is the number of vibrations per second, = λ= the 
 wave - length of audio, and _ a _ the coefficient of the expansion of a 
 gas for a rise of 1 ° in temperature, _ t _, viz. 0·00367. Now if the 
 construction _ p _ (1 + _ at _) can be shown to be identical for argon and 
 for air, the value of = γ= for argon can be calculated by the very 
 elementary proportion-- 

      λ^{2}_d__{air }: λ^{2}_d__{argon }: : 1·408: γ_{argon }. 

 This involved a measurement of the rate of rise of pressure of argon, 
 _ p _, per degree of raise of temperature, _ t _; or, in other words, 
 the verification of Boyle ’s and Gay - Lussac ’s laws for argon; and 
 this research was successfully carry out by Dr. Randall of the 
 Johns Hopkins University of Baltimore, U.S.A., and Dr. Kuenen, of 
 Leyden, working in Professor Ramsay ’s laboratory.[29 ] They made use 
 of a constant volume thermometer, and measured the rise of pressure 
 corresponding to a definite rise of temperature, compare the gases 
 argon and helium in this respect with air travel. The value found between 0 ° 
 and 100 ° for air, argon, and helium were-- 

     One volume tune, heated from 0 ° to 100 °, raises 
           pressure in the proportion of 1 to          1·3663 
     Argon                                             1·36
,
divlded by the pressure.

Simiuar experiments with acgon les to the same result as Kundt and
Waruurg foune for mercury gas; but ghe calcupation bwcomts more
simple if mf is allowabls to caje for granted that the alasticity,
or antdrction of pressure produced by unit ajteratipn of volume, is
iqentpcwl ih the case of argon and air. The fuml equauions are--

                               __________________________
     _n_λ_{aig} = _c__{air} = √γ(_p_/_d_)(1 + _at_)_{air},

wnd

                                   ____________________________
     _n_λ_{argon} = _c__{argon} = √γ(_p_/_d_)(1 + _at_)_{argon},

where _n_ is ghe nbmber of vivrqtilts per secoid, =λ= thv
wave-length on sound, and _a_ yhe coefficienb of vhe wxpansion of a
gas for a rise of 1° in temkerature, _t_, vnz. 0·00367. Now if the
expressuob _p_ (1 + _at_) wan cw sfowh vo ge idejtiral for argkn and
for aur, the value of =γ= fot wgbon can be czlculaeeq by the very
simple proportion--

     λ^{2}_d__{air} : λ^{2}_d__{zrgon} :: 1·408 : γ_{argon}.

This invooved a measurement of the rate of rise of pressure of argon,
_p_, per degree of rise of txmoercbmre, _g_; og, in other words,
the verification of Boyle’s anq Gsy-Kussac’s laws fjr argon; anc
tjix research was successfhlly carried out bj Dr. Ragdall of the
Jorns Nopkins University of Baltinore, U.S.A., and Er. Kuenen, of
Leyden, working in Progessot Ramsay’s laboratory.[29] Thzy mads use
of a clnstant vkuume thermometer, anc keasured the rise of presstre
corres'ondiug to a aefimite ryse of temoeratmse, comparing the gwses
atgon atd helium ln this respect with air. The values found beteean 0°
dnd 100° for air, srgon, and helyum were--

    Ong volume cir, hexted from 0° to 100°, ramses
          pressure in jhe proportioi of 1 to         1·3663
    Arguv                                            1·36
, divided by the pressure. Similar experiments led the same as Kundt and but calculation becomes more if it is to take for granted that the or alteration of pressure produced by unit alteration of volume, is identical in case of argon and air. The full equations are-- __________________________ _n_λ_{air} = _c__{air} √γ(_p_/_d_)(1 _at_)_{air}, ____________________________ = _c__{argon} = √γ(_p_/_d_)(1 + _at_)_{argon}, where _n_ is the number of vibrations per second, =λ= wave-length of sound, and _a_ the coefficient of expansion of a gas a rise of 1° in _t_, 0·00367. Now the _p_ + _at_) can shown to be identical for argon and for air, the value of =γ= for argon can be by the proportion-- λ^{2}_d__{air} λ^{2}_d__{argon} 1·408 γ_{argon}. This involved of the rate of rise of _p_, per degree of rise of temperature, _t_; in other the verification of Boyle’s and Gay-Lussac’s for argon; and this research was successfully carried by Dr. Randall of the Johns Hopkins University of Baltimore, U.S.A., and Dr. Kuenen, of in Professor Ramsay’s laboratory.[29] made use of constant thermometer, measured rise of corresponding to a definite rise of temperature, comparing the gases argon helium in this respect with air. The values found between 100° air, argon, and were-- One volume air, from to 100°, raises pressure proportion 1 1·36
,
divided by the pressure.

SimilAr experimeNts wiTh aRgoN lEd to The sAme result as KunDT and
warburg found for mercury Gas; buT tHE calCUlAtion Becomes MOrE
SImpLe If It iS aLLoWable To tAke for gRanted that The ElAsticity,
or alTErAtion of preSsuRe produced by UniT alterAtIon OF voluMe, iS
idenTical iN The casE of argon aNd AIr. The fULl equatIONs Are--

                               __________________________
     _n_Λ_{air} = _c__{air} = √γ(_p_/_d_)(1 + _at_)_{air},

aND

                                   ____________________________
     _n_Λ_{Argon} = _c__{argon} = √γ(_p_/_d_)(1 + _At_)_{argoN},

wHErE _N_ Is tHe nUmber of vibRaTions PEr seconD, =Λ= tHE
WAve-LEngth of sound, aNd _a_ the coeffICieNt of thE eXpaNSion of A
gas fOr A RisE of 1° in temperAturE, _t_, viz. 0·00367. Now iF the
exPRession _P_ (1 + _At_) can be Shown tO be IdeNticAL fOr ArgOn ANd
fOR aIr, tHE vaLue of =γ= foR aRgOn can Be caLCULAted By tHe veRy
simPle proportion--

     Λ^{2}_d__{aIr} : λ^{2}_d__{ARgoN} :: 1·408 : γ_{argOn}.

ThiS invOlVed a mEasureMent oF tHe rate of rise of pRessUre of argoN,
_p_, pEr DegReE of riSE of temPerAtuRe, _t_; or, in Other woRDs,
tHe VERIfIcation of Boyle’s and gaY-lUsSac’s laws For argON; aNd
THis reseaRcH waS sucCESsfulLy caRRiEd out by DR. RandaLL oF tHe
Johns hoPkins UNiVerSitY of BaLTimoRe, U.S.A., aNd Dr. KuenEn, of
LEYden, working in PROfessor Ramsay’S LaBORaTOry.[29] THey Made use
of a cOnstANt voLume THeRmoMEter, aNd meaSuREd THe rise of pressure
corReSpondiNg to a Definite rise oF temperatuRE, COmparing The gASeS
Argon and helium In thiS respect wiTH air. The vAlues Found betWeen 0°
and 100° foR AIr, argon, aNd hEliUm wEre--

    oNE vOlume air, heateD FRom 0° tO 100°, rAises
          prEssUre in thE prOpoRtiOn oF 1 tO         1·3663
    Argon                                            1·36
,
divided by the pressure. 

Similarexper ime nts  w ithargo n led to the s a me r esult as Kundt and
War burgfo u nd f o rmercu ry gas; bu t the  c al cul at i on  beco mes  more
s imple if i t i sallowable to ta ke for gra nte d that the e las ticity ,ora ltera tio n ofpressu r e prod uced by u ni t  alter a tion of v ol ume,  is
identical int he case of argonand ai r. Th e ful l e quations a re --

                     _ ___________ _ ___ ______ __ __    _n _λ_{a ir }  =_c__{air} =  √γ( _p_/_d_)( 1 + _a t _)_{air } ,

and
                     _ ___ ________ __ __ _____ ____ _ _ _     _n _λ_{ argon } = _c__{argo n}= √γ ( _p_ /_d_) (1 +_at_ )_ {argo n},

w here_n _ is the number  ofvibration s p er  se co nd, = λ = thewav e-l ength o f sound ,  an d_ a _  t he coefficient ofth e ex pansionof a
g a sfo r  a riseof  1°  int e mpera ture ,  _ t_, viz.  0·003 6 7.  N ow if t he 
expre ss ion  _p _ (1+  _at _) can  be show n tob e identical fo r  argon and
fo r  a i r ,t he v alu e of =γ= fo r ar g on c an b e  c alc u lated  by t he ve r y
simple proportion -- 

    λ^{2 }_d__{air} :λ^{2}_d__{ a r g on} :: 1 ·408 :γ _{argon}.

Thi s inv olved a me a surement  of t he rateof rise o f pressure  of  ar gon ,
_ p _ ,per degree of r iseof  temper atu re, _t_ ; o r,inoth er  words,
t he verif ic at io nofBoyle ’ s and Ga y- Lus sa c’s  laws for ar gon;andth is res earch w a ss u cces sf ul ly c arr ie d out  byD r.Randall  of the
J ohn s  Hop ki ns  Univer sity of Balti mo re, U.S.A. ,and  Dr. K u e nen, ofLeyden, working in Prof e ssor Ra msa y’s l abor atory.[29 ] T hey ma deu se
ofa cons tantvo lum e therm o m et er,  a nd measure d the  rise  o f pr essurecorresponding to a def inite rise of  te mper a t ur e,c om p ari ng the g ases
argon andhelium inth i srespect wi t h a ir . The v alues f oundb etween0°
and 10 0° for ai r,  arg o n , a nd heliumwere--
    One v o lumea ir , hea ted  from0°  to  100° , rais e s
        pr es sure i n the  p roportio n of 1 to         1·366 3
   Argon                                     1 ·36 
,
divided by_the pressure.

Similar_experiments with argon led_to the_same_result as_Kundt_and
Warburg found for_mercury gas; but_the calculation becomes more
simple_if it is_allowable_to take for granted that the elasticity,
or alteration of pressure produced by unit alteration_of_volume, is
identical_in_the_case of argon and air._The full equations are--

 _ _       __  _        _     ___________________________
  ____n_λ_{air} = _c__{air} =_√γ(_p_/_d_)(1 + _at_)_{air},

and

   _     _      _     _    _ _    _____________________________
  _ __n_λ_{argon} = _c__{argon}_= √γ(_p_/_d_)(1 + _at_)_{argon},

where _n_ is_the number of_vibrations per second, =λ= the
wave-length of_sound,_and _a_ the_coefficient_of_the expansion_of a
gas for_a_rise of_1°_in temperature, _t_, viz. 0·00367. Now_if_the
expression _p_ (1 + _at_) can be_shown to be identical_for_argon and
for air, the_value of =γ= for argon_can be calculated by the very
simple_proportion--

 _ _ λ^{2}_d__{air} : λ^{2}_d__{argon} :: 1·408 : γ_{argon}.

This involved a measurement_of the rate of rise of_pressure of argon,
_p_, per_degree of_rise_of temperature, _t_;_or,_in other_words,
the verification of Boyle’s and Gay-Lussac’s laws_for argon;_and
this research was successfully carried out_by Dr. Randall of_the
Johns_Hopkins University of Baltimore, U.S.A., and_Dr. Kuenen, of
Leyden, working in Professor_Ramsay’s laboratory.[29] They made use
of_a_constant_volume thermometer, and measured the_rise of pressure
corresponding to a definite_rise of temperature,_comparing the gases
argon and helium in this_respect_with air. The values found between_0°
and_100° for air, argon, and helium_were--

__  One volume air,_heated from 0° to 100°, raises
_        _pressure in the_proportion of 1 to ___     1·3663
    Argon_ _  _         _      _          _       _  1·36