The thermal decomposition of DMSO

Head, David Lynn; Mccarty, C. G.

doi:10.1016/s0040-4039(01)95955-6

Cited by 67 publications

(49 citation statements)

References 3 publications

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“…1 we show an image of the crystals in solution alongside the control vials into which no acid was added. Since DMSO has no acidic byproduct, we can verify whether acidity alone can cause supersaturation by attempting to crystallize the chloride system in DMSO by addition of FAH15. We observe that a concentrated solution of the chloride salts (CH 3 NH 3 Cl and PbCl 2 at 2 M concentration) does not precipitate crystals when incubated at elevated temperatures (up to 80 °C) for several hours.…”

Section: Resultsmentioning

confidence: 96%

Mechanism for rapid growth of organic–inorganic halide perovskite crystals

et al. 2016

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Optoelectronic devices based on hybrid halide perovskites have shown remarkable progress to high performance. However, despite their apparent success, there remain many open questions about their intrinsic properties. Single crystals are often seen as the ideal platform for understanding the limits of crystalline materials, and recent reports of rapid, high-temperature crystallization of single crystals should enable a variety of studies. Here we explore the mechanism of this crystallization and find that it is due to reversible changes in the solution where breaking up of colloids, and a change in the solvent strength, leads to supersaturation and subsequent crystallization. We use this knowledge to demonstrate a broader range of processing parameters and show that these can lead to improved crystal quality. Our findings are therefore of central importance to enable the continued advancement of perovskite optoelectronics and to the improved reproducibility through a better understanding of factors influencing and controlling crystallization.

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Section: Resultsmentioning

confidence: 96%

Mechanism for rapid growth of organic–inorganic halide perovskite crystals

et al. 2016

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“…Furthermore, it was found that DMSO produces acidic species during this decomposition. 52,59 Therefore, as in the case of the model compound, we expect the formation of ion pairs consisting of C]NH + units and the anionic decomposition products of DMSO for PIN1 and PIN2. This hypothesis is furthermore substantiated by elemental analysis ( Table 2).…”

Section: Synthesis and Characterizationmentioning

confidence: 85%

Porous imine-based networks with protonated imine linkages for carbon dioxide separation from mixtures with nitrogen and methane

et al. 2015

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Porous imine-linked networks (PINs) have been prepared by catalyst-free Schiff base condensation of 2,4,6-(4-aminophenyl)1,3,5-triazine with 9,10-anthracene-dicarboxaldehyde (PIN1 and PIN1_2) and with 4,4 0 ,4 00 ,4 000 -methanetetrakis-benzaldehyde (PIN2). Even after synthesis optimisation, only with DMSO (PIN1 and PIN2) microporous frameworks were obtained, whereas DMF (PIN1_2) and other solvents led to nonporous systems, estimated by argon measurements. Furthermore, 15 N solid state NMR and IR spectroscopy reveal the influence of the decomposition products of DMSO leading to protonation of the imine linkage and resulting in an ionic structure with an incorporated sulfonic counterion. Until now, protonation of an imine function due to the usage of DMSO as solvent has not been discussed in the literature. In contrast, for PIN1_2 the imine linkage remains neutral. Argon sorption isotherms for PIN1 and PIN2 exhibit surface areas of 458 m 2 g À1 and 325 m 2 g À1 and the pore structure displays micro-and small mesopores with pore diameters from 0.6 to 5 nm. Additionally, CO 2 isotherms at 273 K demonstrate ultramicropores for all three polymers with similar pore size distributions. Despite their different network structures, similar CO 2 uptakes (1.8-1.06 mmol g À1 at 273 K at 1.0 bar) and heat of adsorption Q st values of 30 kJ mol À1 were obtained. In line with the polyionic character of PIN1 and PIN2, both compounds adsorb three times more water than the more hydrophobic, neutral PIN1_2 at room temperature indicating two different adsorption mechanisms. IAST selectivity calculations show good CO 2 /N 2 (30-31) and CO 2 /CH 4 (8-12) selectivity factors. Despite their moderate BET-surface areas, the PINs show good CO 2 uptakes and selectivity factors.

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“…4, lower right panel, Table 2). In addition to DMSO being a stronger denaturing agent than FA [40,41] its thermal stability is much higher [42] whereas FA is prone to thermal decomposition at elevated temperatures [20]. Best separations were achieved using a buffer system including 7 M urea and 30% DMSO using a capillary with an effective length of 50 cm (Fig.…”

Section: Addition Of Organic Solventsmentioning

confidence: 99%