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1998 (1)
1997 (1)
1Author    C. H. Ennig, H. O. Pperm, AnnRequires cookie*
 Title    Thermische Zersetzung und Lösungskalorimetrie von Ammoniumsamariumchloriden Therm al D ecom position and Solution C alorim etry of A m m onium Sam arium Chlorides  
 Abstract    We determined the decomposition equilibria of ammonium samarium chlorides (NH4)2SmCl5 and NH4Sm2Cl7 by total pressure measurements and derived their thermody­ namical data from the decomposition functions. The enthalpies of formation were compared with the results of the solution calorimetry. The heats of solution of all solid phases in the system SmCl3-NH4Cl and of Sm20 3 were measured in 4n HC1. The enthalpies of formation of ammonium samarium chlorides were derived from the enthalpies of formation of SmCl3 and of NH4C1 and their heats of solution. Data by total pressure measurement ZlHB((NH4)2SmCl5f298) =-407,7±2,9 kcal/mol; S0((NH4)2SmCl5x298) = 84,0 ±4,5 cal/K-mol; ZlHß((NH4)Srn2Ci7x298) = -576,8 ±3,4 kcal/mol; S0(NH4Sm2Cl7x298) = 98,l ±5,5 cal/K-mol. Data by solution calorimetry ZlH°B(SmCl3 f298) = -248,1 ±0,8 kcal/mol; zJHo B((NH4),Sm Cl,f298) = -40 4 ,3 ± l,l kcal/mol; ZlH°B(NH4Sm9Cl7 f 298)= -572,3± 1,8 kcal/mol. 
  Reference    Z. Naturforsch. 52b, 1517—1525 (1997); eingegangen am 29. September 1997 
  Published    1997 
  Keywords    Ammonium Samarium Chlorides, Samarium Chloride, Synthesis, Thermodynamical Data, Solution Calorimetry 
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 TEI-XML for    default:Reihe_B/52/ZNB-1997-52b-1517.pdf 
 Identifier    ZNB-1997-52b-1517 
 Volume    52 
2Author    C. Hennig, H. OppermannRequires cookie*
 Title    Thermische Zersetzung und Lösungskalorimetrie von Ammoniumneodymchloriden Thermal Decomposition and Solution Calorimetry of Ammonium Neodymium Chlorides  
 Abstract    The thermodynamical data of ammonium neodymium chlorides (NH4)2NdCl5 and NH4Nd2Cl7 were derived by the determination of their decomposition equilibria by total pres­ sure measurements. Moreover, solution calorimetry was applied. The enthalpies of formation of these phases were calculated from their heats of solution and from the enthalpies of formation and the heats of solution of NdCl3 and NH4C1. D ata by total pressure measurement: Z\H£((NH4)2NdCl5,f)298) = — 412,5 dh 3,6 kcal/mol; S°((NH4)2NdCl5 f 298) = 80,1 ± 5,8 cal/K m ol; Z\H£(NH4Nd2Cl7,f,298) = -579,5 ± 3,5 kcal/mol; S°(NH4Nd2Cl7,f,298) 101,8 ± 5,6 cal/K mol. D ata by solution calorim etry: 4H £(N dC l3;f,298) -251,2 ± 0,7 kcal/mol; /\H £((N H 4)2NdCl5,f,298) = -105,5 ± 1,0 kcal/mol; Z\Hß(NH4Nd2Cl7f 298) = -576,8 ± 1,7 kcal/mol. 
  Reference    Z. Naturforsch. 53b, 175—183 (1998); eingegangen am 16. Oktober 1997 
  Published    1998 
  Keywords    Ammonium Neodymium Chlorides, Neodymium Chloride, Thermodynamical Data, Solution Calorimetry, Heat of Solution 
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 TEI-XML for    default:Reihe_B/53/ZNB-1998-53b-0175.pdf 
 Identifier    ZNB-1998-53b-0175 
 Volume    53