Aqueous Sulfuric Acid. Heat Capacity. Partial Specific Heat Content of Water at 25 and -20°<sup>1</sup>

Kunzler, J. E.; Giauque, W. F.

doi:10.1021/ja01134a006

Cited by 30 publications

(18 citation statements)

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“…The reaction enthalpies can be calculated using the formation enthalpies of the starting and resulting compounds [38,[76][77][78]. The values are equal to -393.8 and -290.3 kJ/mol for reactions (1) and 2, respectively.…”

Section: Resultsmentioning

confidence: 99%

Exploration of structural, thermal and spectroscopic properties of self-activated sulfate Eu2(SO4)3 with isolated SO4 groups

Denisenko

Aleksandrovsky

Atuchin

et al. 2018

Journal of Industrial and Engineering Chemistry

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Eu2(SO4)3 was synthesized by chemical precipitation method and the crystal structure was determined by Rietveld analysis. The compound crystallizes in monoclinic space group С2/с. In the air environment, Eu2(SO4)3 is stable up to 670°C. The sample of Eu2(SO4)3 was examined by Raman, Fourier-transform infrared absorption and luminescence spectroscopy methods. The low site symmetry of SO4 tetrahedra results in the appearance of the IR inactive ν1 mode around 1000 cm-1 and ν2 modes below 500 cm-1. The band intensities redistribution in the luminescent spectra of Eu 3+ ions is analyzed in terms of the peculiarities of its local environment.

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Section: Resultsmentioning

confidence: 99%

Exploration of structural, thermal and spectroscopic properties of self-activated sulfate Eu2(SO4)3 with isolated SO4 groups

Denisenko

Aleksandrovsky

Atuchin

et al. 2018

Journal of Industrial and Engineering Chemistry

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“…D ata a t higher concentrations were obtained from our own experiments using the isopiestic method for equilibrating solutions a t two different temperatures. The relationship between the activities a t different temperatures was provided by the calorimetric measurements of the partial specific heat contents of water in sulphuric acid (Kunzler & Giauque 1952). This work is still being continued to higher sulphuric acid concentrations and will be published separately in due course.…”

Section: (B) Water Activity Of Sulphuric Acid Solutionmentioning

confidence: 99%

A theoretical treatment of cation exchangers - III. The hydration of cations in polystyrene sulphonates

Glueckauf

Kitt

1955

Proc. R. Soc. Lond. A

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The adsorption of water by the polystyrene sulphonates of cations has been investigated at 0 and 25° C, using an isopiestic method. The adsorption isotherm and the heats (enthalpies) and entropies of hydration have been obtained for the monovalent cations H, Li, Na, K, Cs, NH4, Ag and for the divalent cations Be, Mg, Ca, Sr, Ba, Hg. With the exception of H, which gives a smooth enthalpy-water-content curve, all monovalent cations show a more or less marked step in the differential enthalpy of adsorbed water between the first and second water molecule adsorbed per ion, thereafter the steps are less clearly defined. The differential entropies show similarities to those calculated for a B. E. T. isotherm, except that the curves show two minima which correspond to approximately 0.15 and 1.5 molecules of water/ion. The adsorption isotherms follow more or less the model of the B. E. T. isotherm, with several significant differences: ( a ) the volatility of the second and further water molecule/ion is not that of liquid water, but only tends to reach this value after several molecules/ion are adsorbed, and the energy levels of the first successive water molecules, though rising rapidly, differ substantially from that of liquid water; ( b ) the adsorption process of the first water molecule is significantly different from a Langmuir mechanism, and varies approximately as the one-half power of the water activity. The knowledge of the free energies, enthalpies and entropies permits a fair analysis of the hydration mechanism into its individual steps, which then permits a calculation of the standard state enthalpies and entropies of the first hydration steps. Both functions show a markedly linear relationship with the ionic radius of the unhydrated ion when summed up for the first two water molecules adsorbed. The knowledge of the adsorption isotherms permits one to differentiate between water adsorbed with zero free energy (swelling water) and the excess adsorbed water (cationic and anionic hydration water). The amount of hydration water associated with the cations has been obtained in this way both for mono- and divalent ions. The amount varies both with the water activity and with temperature. It is clear from the small free energies of hydration of all monovalent ions that the association of almost all water molecules is very loose, and is not related to the co-ordination number of the ions.

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“…The results given for eqs (1), (2), and (3) were therefore corrected to the stoichiometry specified in eqs (4), (5), and (6) by assuming that in each case only the reference component was present in water. Equations (1), (2), and (3) were combined with the heats of dilution of sulfur dioxide [1], sulfuric acid [2, 12], and hydrochloric acid [2], to obtain the processes: leftCl2(normalg)+2(SO2⋅2500normalH2O)+2502normalH2O=[normalH2SO4⋅2500normalH2O+2(HCl⋅1250normalH2O)+SO2⋅2500normalH2O]ΔH(25°C)=−75.92±0.13kcal/moleCl2. left2(HCl⋅1250normalH2O<...>…”

Section: Resultsmentioning

confidence: 99%

Heat of oxidation of aqueous sulfur dioxide with gaseous chlorine

Johnson¹,

Ambrose²

1963

J. RES. NATL. BUR. STAN. SECT. A.

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The heat of oxid ation of aqueous s ulfur diox ide ,,·it h gaseolls c hlorin e has be(, 11 deLermil1 ed by calorimetric m ethods. Thc results cOl"t"cspond to thc reaction:Cl,(g)+ SO ,·2500 H 20 + 2502 H ,O = I-I 2SO,·25 00 FLO + 2 (H CI1250 H 20 ), 6H(25 dc) = -77.28 ± 0.14 kcal / mole. Thc h eat of form ation of aqlleo us s ulfuric ac id (ill 2500 moles of lI"atcr) has becn calculated t o be -21:3.92 kca l/ moic . . Introduction.. An investigation or t h e heats of solu Lion an d c, oxidlttion or sulfur dioxide to sulfuric acid usi.ng /" bromine as the oxi.dizin g s ubstance wa s recc ntly mad e n,L the U niversity of Lund, S weden [1]. 2 Altho ugh Lhe data on the hetlLs of solution or sulfur \ dioxide were in subs tn,nLi,\l agree ment with tlte prc-( vious datft [2] Lhe cH.lculatecl h ea L or formation of j s uUuric ftcid clifrerecl by ftpproximaLcly 0 .3 kenl/ mol e from t L te resulLs obtain ed in sevcmL r ecell L c!eLcl"-;: mination s [:3. 4, 5, 6J. Becau se the heaL of forlllaLion or s uUuric a,cid sec ms to be well s ubsta ntiaLed it. see med probn,ble that the di scr epan cy mu sL be ntt ribuLed Lo the data on thc h eat or for ma tion of hydrobromic ariel. It see med des irable, ther eforc, Lo , ma,ke a new clctcrminfttion oC Lh e h eaL or oxidaLion , of sulf"ur dioxide using chlorin e as 1 he oxidizi ng agc n t. "( The combin ed data would b e indiC'i1tive or tile consistency between Lhe data on hydro chlori c <1,lld hyclro-( bromi c ac id as well as that bet ween Lite ch1,ta on sulCul' dioxide and sulf"uric acid. An error or 0.15 ]ccc1,1/mole in the h eat of formation of hy drobromic acid could acco ull t ror the apparently high value obtained for I tlte heat or formation of sulfuric acid obtained from ... the h eat or oxidation of sulfur dioxide with bromine. . Thiosulfate SolutionThe 0.05 N sodiulll thiosulfatc soluLion wa s prepH.l"ecl by adding 25 g of re,1,ge n L-grade sod ium Lhiosulfate p en La hy dmte and 0.2 g of sodium carbonate to 2 li ters of water. The concentn1Lioll or . the soluLion WU i'\ determilled by companson with li te 0.1 N ioeLi ne solution . . Sulfur Dioxide Solutioni\. mass-specLrometri c an alysis 01" the grtseous s ull"ur dioxide W,lS perform ed by E. E. Hu ghes or lIlC Applied An aly tical ResC

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Aqueous Sulfuric Acid. Heat Capacity. Partial Specific Heat Content of Water at 25 and -20°¹

Cited by 30 publications

References 0 publications

Exploration of structural, thermal and spectroscopic properties of self-activated sulfate Eu2(SO4)3 with isolated SO4 groups

Exploration of structural, thermal and spectroscopic properties of self-activated sulfate Eu2(SO4)3 with isolated SO4 groups

A theoretical treatment of cation exchangers - III. The hydration of cations in polystyrene sulphonates

Heat of oxidation of aqueous sulfur dioxide with gaseous chlorine

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Aqueous Sulfuric Acid. Heat Capacity. Partial Specific Heat Content of Water at 25 and -20°1

Cited by 30 publications

References 0 publications

Exploration of structural, thermal and spectroscopic properties of self-activated sulfate Eu2(SO4)3 with isolated SO4 groups

Exploration of structural, thermal and spectroscopic properties of self-activated sulfate Eu2(SO4)3 with isolated SO4 groups

A theoretical treatment of cation exchangers - III. The hydration of cations in polystyrene sulphonates

Heat of oxidation of aqueous sulfur dioxide with gaseous chlorine

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Aqueous Sulfuric Acid. Heat Capacity. Partial Specific Heat Content of Water at 25 and -20°¹