Heat of formation of titanium tetraiodide

Johnson, Walter H.; Gilliland, Alexis A.; Prosen, E.J.

doi:10.6028/jres.063a.009

Cited by 11 publications

(10 citation statements)

References 4 publications

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“…The glass calorimeter was, except for minor changes, the same as that previously described [7]. The Teflon bearings were removed and the stirrer shaft was supported by ball bearings placed above the calorimeter head.…”

Section: Apparatusmentioning

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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Section: Apparatusmentioning

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 calorimeter was immersed in a water bath in which the temperature, approximately 26.8 °C, varied by not more than ±0.002 °C during an experiment. The bath, temperature controls, and method of measuring electrical energy during calibrations have been described previously [ 4 , 5 ].…”

Section: Materials and Apparatusmentioning

confidence: 99%

Heats of hydrolysis and formation of dimethoxychloroborane

Kilday¹,

Johnson²,

Prosen³

1961

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

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The heat of hydrolysis of dimethoxychloroborane has been m eas ured;. for the r eaction, (CH 30hBCI (liq) + 3H20 (liq) = H 3B03(C) + 2CI-I30H (Iiq) + Hc;l (g) L'>H(25 °C) = -26.6 ± 0.8 kj /mole = -6.4 ± 0.2 kcal/ mole. From this, we have calculated the h eat of formation of dimethoxychloroboran e: for the liquid, MJf"(25 °C) = -782.1 ± l.8 kj /mole (-186.9 ± 0.4 kcal/ mole), and for the gas, L'>Hr(25 °C) = -747.9 ± 2.2 kj / mole (-178.8 ± 0.5 kcal/mole).

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“…The calorimeter was similar to that previously described [ 3 ], except that the liquid capacity was 400 ml and the resistance of the calorimeter heater was 228 ohms. The cooling constant was 0.0010 °C min −1 (°C of thermal head).…”

Section: Apparatus and Proceduresmentioning

confidence: 99%