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The reaction quickly reaches equilibrium at 100°C, but at room temperature, the reverse reaction is slow enough to isolate borane carbonyl. This reaction is performed at high pressures, typically with a maximum pressure observed of 1000 to 1600 [[Pound per square inch|psi]].<ref>{{Cite journal |last=Carter |first=James C. |last2=Parry |first2=Robert W. |date=1965-06-01 |title=The Ammonia and Alkylamine Addition Compounds of Carbon Monoxide Borane |url=http://dx.doi.org/10.1021/ja01089a009 |journal=Journal of the American Chemical Society |volume=87 |issue=11 |pages=2354–2358 |doi=10.1021/ja01089a009 |issn=0002-7863}}</ref> It can also be performed at atmospheric pressure, with [[ether]]s as a [[catalyst]].<ref>{{Cite journal |last=Mayer |first=Erwin |date=1971-07-01 |title=Äther als Katalysatoren für die Reaktion von Diboran mit Lewis-Basen; vereinfachte Darstellung von Carbonylboran und Phosphinboran |url=https://doi.org/10.1007/BF00909917 |journal=Monatshefte für Chemie |language=de |volume=102 |issue=4 |pages=940–945 |doi=10.1007/BF00909917 |issn=1434-4475}}</ref><ref name=":1" />
A more recent synthesis of borane carbonyl involves slowly bubbling [[carbon monoxide]] through a 1 [[Molar concentration|M]] {{chem2|H3B\s[[Tetrahydrofuran|THF]]}} solution. The resulting gas stream can be condensed and subsequently bubbled through
== References ==
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