The Kinetics of the Thermal Decomposition of Sodium Nitrate and of the Reaction between Sodium Nitrite and Oxygen

Freeman, Eli S.

doi:10.1021/j150545a005

Cited by 135 publications

(73 citation statements)

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“…Concentrations of nitrate in the coastal waters of west Hawaiʻi have increased dramatically since the 1950s (up to 140 μmol/m 3 in west coast bays) and has been linked to eutrophication [19]. K 2 NO 3 and Na 2 NO 3 decompose on heating to KNO 2 and NaNO 2 , respectively [20]. Thermal decomposition of NaNO 2 does not begin to take place until temperatures of around 600°C are reached, generating Na 2 O and NO 2 [20].…”

Section: Origin Of Co 2 and No 2 In The Airborne Lavaseawater Interacmentioning

confidence: 99%

“…K 2 NO 3 and Na 2 NO 3 decompose on heating to KNO 2 and NaNO 2 , respectively [20]. Thermal decomposition of NaNO 2 does not begin to take place until temperatures of around 600°C are reached, generating Na 2 O and NO 2 [20]. Nitrates of magnesium to copper in the reactivity series of metals (and ammonium nitrate) decompose on heating to ∼400°C, to form metal oxides, O 2 and NO 2 gas.…”

Section: Origin Of Co 2 and No 2 In The Airborne Lavaseawater Interacmentioning

confidence: 99%

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The airborne lava–seawater interaction plume at Kīlauea Volcano, Hawaiʻi

Edmonds

Gerlach

2006

Earth and Planetary Science Letters

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Section: Origin Of Co 2 and No 2 In The Airborne Lavaseawater Interacmentioning

confidence: 99%

Section: Origin Of Co 2 and No 2 In The Airborne Lavaseawater Interacmentioning

confidence: 99%

The airborne lava–seawater interaction plume at Kīlauea Volcano, Hawaiʻi

Edmonds

Gerlach

2006

Earth and Planetary Science Letters

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“…Melting occurs at 579 K and requires 182.4 J/g. Slow decomposition begins at about 875 K, and the pseudoequilibrium between the nitrate, nitrite, and oxygen has been examined over many years (Oza 1945, Freeman 1956, Sirotkin 1959, Arvia et al 1964, Bond and Jacobs 1966, Kust and Burke 1970. Many investigations of these reactions appear in the literature and include spectroscopic measurements of melts, gas analysis, and electrochemical measurements.…”

Section: Thermal Data For Compoundsmentioning

confidence: 99%

Calculation of reaction energies and adiabatic temperatures for waste tank reactions

Burger¹

1993

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SummaryContinual concern has been expressed over potentially hazardous exothermic reactions that might occur in Hanford Site underground waste storage tanks. These tanks contain many different oxidizable compounds covering a wide range of concentrations. Several compounds may be in concentrations and quantities great enough to be considered a hazard in that they could undergo rapid and energetic chemical reactions with nitrate and nitrite salts that are present it heated to the initiating or critical temperature. The chemical hazards are a function of several interrelated factors, including the amount of energy (heat) produced, how fast it is produced, and the thermal absorption and heat transfer properties of the system. The reaction path(s) will determine the amount of energy produced and kinetics will determine the rate that it is produced. The tanks also contain many inorganic compounds inert to oxidation. These compounds act as diluents and can inhibit exothermic reactions because of their heat capacity and thus, in contrast to the oxidizable compounds, provide mitigation of hazardous reactions.In this report the energy that may be released when various organic and inorganic compounds react is computed as a function of the reaction-mix composition and the temperature. The enthalpy, or integrated heat capacity, of these compounds and various reaction products is presented as a function of temperature; the enthalpy of a given mixture can then be equated to the energy release from various reactions to predict the maximum temperature which may be reached. This is estimated for several different compositions. Alternatively, the amounts of various diluents required to prevent the temperature from reaching a critical value can be estimated. Reactions W i g different paths, forming different products such as N20 in place of N2 are also considered, as are reactions where an excess of caustic is present. Oxidants other than nitrate and nitrite are considered briefly.The relative available energy per unit mass of the various oxidizable compounds, or "fuels," that may be present ranges from 1 to about 25. Stoichiometric mixes with oxidant, e.g., fuel plus the required amount of sodium nitrate (NaNO,) for a complete reaction, compared on a mass basis, also show large differences. This "energy density" covers a range of 1 to about 5.A consequence of different stoichiometries for different fuels is that an excess of sodium nitrate or nitrite for one reactant may be a deficiency for another. This is significant since excess nitrate or nitrite is an excellent heat sink, especially at elevated temperatures.The efficiency of various compounds as heat sinks, i.e., their enthalpies, vary greatly. In the wastes water is the most significant material at temperatures up to slightly above 100°C. From 100°C to about 300°C the greatest effect is probably from hydrated salts, with some contribution from concentrated caustic solutions. The loss of water from these materials requires a large energy input, some 50% to 100% greater than f...

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“…in method and particularly in.interpretation of..the results, they all indicate that reaction (1) is essentially completely at equilibrium within two hours at 700°C. Two Actual chemical analysis for nitrate and nitrite were used to obtain the data of reference (48) whereas only gas evolution volumes were used to obtain the results of reference (47).. The latter authors also used a very questionable crucible material (stainless steel), and it would appear that the results of reference (48) are more likely correct.…”

Section: I-mentioning

confidence: 99%