Practical Inorganic Chemistry

Pass, Geoffrey; Sutcliffe, H.

doi:10.1007/978-94-017-2744-0

Cited by 36 publications

(33 citation statements)

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“…The yellow precipitate of iron(II) oxalate dihydrate was washed with hot water, suction filtered, washed again with hot water, and allowed to dry in the filter for about 10 minutes before being placed in a desiccator for about a week. An excess of about 76% of oxalic acid was prescribed in this protocol (10). Three experiments were performed and a 92% yield was obtained (92.091.9%, standard deviation).…”

Section: Methodsmentioning

confidence: 99%

“…A number of experiments were initially performed following a published protocol (10) in which the product was prepared from iron(II) sulfate heptahydrate and oxalic acid dihydrate. This protocol proposed a large excess of oxalic acid, the use of sulfuric acid to acidify the iron(II) sulfate solution, and heating the mixture at temperature near the boiling point.…”

Section: Synthesis Of Iron(ii) Oxalate Dihydratementioning

confidence: 99%

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“Green Star”: a holistic Green Chemistry metric for evaluation of teaching laboratory experiments

Ribeiro

Costa

Machado

2010

Green Chemistry Letters and Reviews

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This paper presents a new semi-quantitative metric, Green Star (GS), for evaluation of the global greenness of chemical reactions used in teaching laboratories. Its purpose is to help choose the more acceptable reactions for implementing Green Chemistry (GC) and to identify suitable modifications of protocols to improve the greenness of the chemistry practiced by students. GS considers globally, in principle, all the Twelve Principles of GC. The metric consists in the evaluation of the greenness of the reaction for each principle by pre-defined criteria, followed by graphical representation of the results in an Excel radar chart Á the fuller the chart, the higher degree of greenness. To illustrate the construction and the scope of the metric, a case study is presented Á the iron(II) oxalate dihydrate synthesis performed under several sets of conditions to pursue the implementation of greenness.

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Section: Methodsmentioning

confidence: 99%

Section: Synthesis Of Iron(ii) Oxalate Dihydratementioning

confidence: 99%

“Green Star”: a holistic Green Chemistry metric for evaluation of teaching laboratory experiments

Ribeiro

Costa

Machado

2010

Green Chemistry Letters and Reviews

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“…For the second procedure, the oxidation of copper (I) chloride was observed under various conditions relevant to corrosion testing and post-test handling and storage of specimens. Copper (I) chloride was prepared in the laboratory from copper (II) chloride hydrate and sodium sulfite (Pass and Sutcliffe, 1974). Approximately 0.1 g was deposited in each of four Pyrex tubes and exposed to the following environments at 220C: (1) dry air -desiccator (CaSO4), 4% rh, 60 d; (2) moist air -50% rh, 100 h; (3) distilled water -5 mL, 100 h; and (4) natural saliva -5 mL, 100 h. After the specified time period, each sample was analyzed by XRD.…”

Section: Methodsmentioning

confidence: 99%

Crevice Corrosion Products of Dental Amalgam

et al. 1991

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The objective of this study was to determine the in vitro corrosion products that resulted from crevice corrosion of low- and high-copper dental amalgams. Specimens were potentiostatically polarized in a chloride-containing electrolyte while set against a PTFE surface to form a crevice. After 16 h, corrosion products were examined by light microscopy, SEM, EDS, and XRD. Analysis showed the presence of three previously reported products [Sn4(OH)6Cl2, SnO, and Cu2O] and a new product, CuCl, which formed on high-copper, gamma 2-free amalgams. Thermodynamic considerations show that CuCl is stable for the reported in vivo potentials of amalgam restorations and the high acidity and high chloride ion concentration associated with crevice corrosion.

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“…It is quite tempting to ascribe the capacity loss to a reaction such as SO~ 2SO2 + 2Li-~ 2Li + + 2SO2-> 2Li + + SzO~ ~-2Li + + S~O62--> Li2S206 + S [7] In this reaction three equivalents of SO2 produce two of current with formation of S and LizS206. Coupled with disproportionation of the SO2 radical ion to eventually form S and Li2S205, this offers a facile explanation for the capacity loss phenomenon, although the available data are far from defnitive.…”

Section: Sos~-+ So~ ~ S~os-= [6]mentioning

confidence: 98%

Chemical Reactions in Lithium Sulfur Dioxide Cells Discharged at High Rates and Temperatures

Bowden

Chow

Demuth

et al. 1984

J. Electrochem. Soc.

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The discharge capacity of Li/SO2 cells was examined at high current and temperatures. D cells rated at 8 Ah delivered over 7 Ah at 5A current and 55~ while cells discharged at 72~ gave 7 Ah at 3A. The cells were analyzed for residual lithium and sulfur dioxide. Spent cathodes were analyzed by infrared spectroscopy. A parasitic reaction was found in which Li2S20~ and S were formed, presumably by reaction of Li2S204 with SO2. This reaction became noticeable only under extreme combination of high rate and temperature.Lithium/SO~ cells are useful power sources for devices requiring high drain pertormance at low temperatures. Such cells generally are of a jelly roll design with layers of lithium toil, separator, and porous carbon cathode. The electrodes are surrounded by a highly conductive nonaqueous electrolyte consisting of an organic solvent (usually acetonitrile), a salt (usually lithium bromide), and sulfur dioxide, which serves as a soluble cathode material (1). In the course of cell discharge the lithium anode is oxidized, and the SO2 soluble cathode is reduced. The discharge product, identified as lithium dithionite (2), precipitates in the porous cathode and eventually may passivate it. Such cells have open-circuit voltages near 3V and discharge at around 2.8V, delivering 140-150 Wh/lb over the cells' life (3, 4). Typical SO~ D cells have short-circuit currents of over 100A and can deliver 30A pulses at specific powers of over 300 W/lb. In the course of discharging cells at elevated temperatures, it was observed that some cells delivered less than the usual capacity. We discharged a number of LO25SX and LO26SX D-type SO2 cells at different rates and temperatures to determine the extent and magnitude of this decline in capacity. We used infrared spectroscopy and specific chemical analysis to identify products of the cells. We report the results here. ExperimentalThe LO26SX, a hermetically sealed spirally wound D cell, was selected .as a test vehicle for this study. The LO26SX is distinguished by its balanced cell chemistry in which the ratio of Li metal and SO2 soluble cathode is near unity. This particular cell is rated at 8 Ah at 267 mA at 25~ Capacities were calculated to a 2V cutoff and cells used for chemical analyses were not discharged below 2V. Cells were discharged at 21 ~ 55 ~ and 72~ on selected loads, as well as at constant currents, with data collection either by a Linseis LD-12 recorder or an HP 1000 computerized data-acquisition system.Cells which were used for chemical analysis were placed in a specially made stainless steel bomb and punctured. The volatile acetonitrlle and SO2 Were

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Practical Inorganic Chemistry

Cited by 36 publications

References 0 publications

“Green Star”: a holistic Green Chemistry metric for evaluation of teaching laboratory experiments

“Green Star”: a holistic Green Chemistry metric for evaluation of teaching laboratory experiments

Crevice Corrosion Products of Dental Amalgam

Chemical Reactions in Lithium Sulfur Dioxide Cells Discharged at High Rates and Temperatures

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