﻿Havens 
  and 
  Way 
  — 
  Separation 
  of 
  Iron. 
  217 
  

  

  Art. 
  XXII. 
  — 
  Separation 
  of 
  Iron 
  from 
  Chromium^ 
  Zirconium^ 
  

   and 
  Beryllium^ 
  hy 
  the 
  Aetiori 
  of 
  Gaseous 
  Hydrochloric 
  

   Acid 
  on 
  the 
  Oxides 
  : 
  bj 
  Frank 
  E 
  Stuart 
  Havens 
  and 
  

   Arthur 
  Fitch 
  Way. 
  

  

  [Contributions 
  from 
  Kent 
  Chemical 
  Laboratery 
  of 
  Yale 
  University 
  — 
  LXXXVII.] 
  

  

  It 
  has 
  been 
  shown 
  in 
  a 
  former 
  paper 
  from 
  this 
  laboratorj^^ 
  

   that 
  iron 
  oxide 
  may 
  be 
  completely 
  volatilized 
  as 
  chloride 
  by 
  a 
  

   strong 
  current 
  of 
  hydrochloric 
  acid 
  gas 
  acting 
  at 
  a 
  tempera- 
  

   ture 
  of 
  450-500°, 
  and 
  also 
  that 
  the 
  addition 
  of 
  a 
  little 
  free 
  

   chlorine 
  to 
  the 
  gaseous 
  hydrochloric 
  acid 
  renders 
  this 
  action 
  

   complete 
  at 
  lower 
  temperatures, 
  180-200°, 
  without 
  the 
  danger 
  

   of 
  error 
  arising 
  from 
  the 
  liability 
  of 
  ferric 
  chloride 
  to 
  dissocia- 
  

   tion, 
  or 
  from 
  deficiency 
  of 
  oxidation 
  in 
  the 
  oxide 
  treated, 
  or 
  

   mechanical 
  loss 
  due 
  to 
  too 
  rapid 
  volatilization. 
  It 
  has 
  also 
  

   been 
  shown 
  that 
  this 
  reaction 
  can 
  be 
  employed 
  for 
  the 
  separa- 
  

   tion 
  of 
  iron 
  and 
  aluminum, 
  taken 
  as 
  the 
  oxides, 
  and 
  its 
  appli- 
  

   cation 
  to 
  the 
  separation 
  of 
  iron 
  from 
  other 
  metallic 
  oxides 
  has 
  

   been 
  suggested. 
  

  

  The 
  oxides 
  of 
  chromium, 
  zirconium, 
  and 
  beryllium, 
  like 
  

   aluminum 
  oxide, 
  are 
  not 
  acted 
  upon 
  by 
  a 
  current 
  of 
  dry 
  hydro- 
  

   chloric 
  acid 
  gas 
  at 
  the 
  temperatures 
  before 
  mentioned, 
  and 
  

   these 
  oxides 
  also 
  can 
  be 
  entirely 
  freed 
  from 
  iron 
  by 
  this 
  reac- 
  

   tion, 
  as 
  the 
  experiments 
  to 
  be 
  described 
  will 
  show. 
  The 
  pro- 
  

   cedure 
  was 
  the 
  same 
  in 
  each 
  case 
  and 
  analogous 
  to 
  that 
  

   employed 
  for 
  the 
  separation 
  of 
  iron 
  from 
  aluminum. 
  A 
  mix- 
  

   ture 
  of 
  a 
  weighed 
  portion 
  of 
  one 
  of 
  these 
  oxides 
  with 
  a 
  

   weighed 
  portion 
  of 
  ferric 
  oxide, 
  contained 
  in 
  a 
  porcelain 
  boat 
  

   and 
  placed 
  within 
  a 
  roomy 
  glass 
  tube 
  supported 
  in 
  a 
  small 
  com- 
  

   bustion 
  furnace, 
  was 
  submitted 
  to 
  the 
  action 
  of 
  a 
  dry 
  current 
  

   of 
  hydrochloric 
  acid 
  gas 
  and 
  chlorine 
  generated 
  by 
  dropping 
  

   sulphuric 
  acid 
  upou 
  a 
  mixture 
  of 
  strong 
  hydrochloric 
  acid, 
  

   common 
  salt, 
  and 
  a 
  small 
  amount 
  of 
  manganese 
  dioxide. 
  The 
  

   gas 
  was 
  admitted 
  at 
  one 
  end 
  of 
  the 
  combustion 
  tube 
  and 
  passed 
  

   out 
  at 
  the 
  other 
  through 
  a 
  water 
  trap, 
  while 
  the 
  required 
  tem- 
  

   perature, 
  from 
  200°-300°, 
  was 
  maintained 
  by 
  regulating 
  the 
  

   various 
  burners 
  of 
  the 
  furnace. 
  The 
  time 
  of 
  action 
  varies 
  

   somewhat 
  with 
  the 
  condition 
  of 
  the 
  oxide 
  to 
  be 
  volatilized, 
  and 
  

   the 
  temperature, 
  generally 
  an 
  hour's 
  heating 
  at 
  200°, 
  proves 
  

   sufficient 
  for 
  the 
  complete 
  removal 
  of 
  0*1 
  gram 
  of 
  iron. 
  At 
  

   higher 
  temperatures 
  the 
  action 
  is 
  more 
  rapid 
  ; 
  but 
  the 
  lighter 
  

   oxide, 
  the 
  beryllium 
  especially, 
  is 
  liable 
  to 
  mechanical 
  loss 
  

   through 
  the 
  too 
  rapid 
  volatilization 
  of 
  the 
  iron, 
  as 
  experiment 
  

   (17), 
  where 
  a 
  temperature 
  of 
  500° 
  was 
  used, 
  will 
  show. 
  It 
  is 
  

  

  Gooch 
  and 
  Havens, 
  this 
  Journal, 
  

  

  