Calcium oxide incandescence

Arsenic trioxide and calcium oxide incandesce in contact with liquid hydrogen fluoride. 

Phosphorus Pentoxide (P2O5). Vigorous reaction with P205 below 2(PC.3 Oxides. Arsenic trioxide and calcium oxide incandesce in contact with the liquid.4... 

Hydrogen sulfide is rapidly oxidised, and may ignite in contact with a range of metal oxides, including barium peroxide, chromium trioxide, copper oxide, lead dioxide, manganese dioxide, nickel oxide, silver(I) oxide, silver(II) oxide, sodium peroxide, and thallium(III) oxide. In the presence of air, contact with mixtures of calcium oxide or barium oxide with mercury oxide or nickel oxide may cause vivid incandescence or explosion. 

Before the advent of electricity, calcium oxide was used to produce the so-called lime light to spotlight or illuminate the stage. When heated by an oxy-hydrogen flame, it incandesces emitting bright white light. 

Na NaOH H2SO4 vinyl acetate HgO sodium tetrafluoro silicate n-phenyl azo piperidine. Incandescent reaction of liquid HF with oxides (e.g., arsenic trioxide, calcium oxide). Dangerous storage hazard with nitric acid + lactic acid nitric acid + propylene glycol (mixtures evolve gas which may burst a sealed container). Reacts with water or steam to produce toxic and corrosive fumes. When heated to decomposition it emits highly corrosive fumes of F . See also FLUORIDES. 

EXPLOSION and FIRE CONCERNS noncombustible solid not expected to be a fire hazard incandescent reaction when mixed with calcium oxide and put into fused calcium chloride no information found concerning explosion data no information found concerning hazardous decomposition productions use appropriate extinguishing media for firefighting purposes. 

EXPLOSION and FIRE CONCERNS not combustible, but extremely irritating if involved in a fire combination with water evolves heat NFPA rating Health 4, Flammability 0, Reactivity 1 reacts explosively with cyanogen fluoride, glycerol and nitric acid, and methane-sulfonic acid violent reaction with acetic anhydride, 2-aminoethanol, chlorosulfonic acid, ethylene diamine, propylene oxide, vinyl acetate, sodium hydroxide, and sulfuric acid liquid hydrogen fluoride reacts incandescently with arsenic trioxide and calcium oxide reacts with water or steam to produce toxic and corrosive fumes incompatible with most metals, water and alkali... 

Hydrogen sulfide reacts violently with soda lime (sodium hydroxide and calcium oxide). The reaction progresses to incandescence in air, and causes explosion in oxygen (Mellor 1946). It reacts violently with many metal oxides, such as lead dioxide, nickel oxide, chromium oxide, and iron oxide, producing incandescence. Reactions with fuming nitric acid and other strong oxidizers can result in incandescence. Reaction with fluorine, interhalogen compounds, and finely divided metals can cause incandescence. 

Lead peroxide is even more active than the oxide. It reacts violently with sulphur and sulphides. When it is ground up with sulphur, the mixture combusts. With hydrogen sulphide, the reaction is very exothermic and causes peroxide to incandesce and hydrogen sulphide to combust. Finally, it reacts violently with calcium, strontium and barium sulphides on heating. 

Mellor, 1940, Vol. 8, 436 1943, Vol. 11, 162 1942, Vol. 12, 32 Pyrophoric chromium attains incandescence in the oxide, while calcium, potassium and uranium need heating before ignition occurs, when combustion is brilliant in the 53% oxygen content. 

Reduction of the oxide by aluminium, calcium, magnesium, potassium, sodium or zinc is accompanied by more or less incandescence (lithium, magnesium and zinc especially). 

The chlorides, bromides, iodides, and cyanides are generally vigorously attacked by fluorine in the cold sulphides, nitrides, and phosphides are attacked in the cold or may be when warmed a little the oxides of the alkalies and alkaline earths are vigorously attacked with incandescence the other oxides usually require to be warmed. The sulphates usually require warming the nitrates generally resist attack even when warmed. The phosphates are more easily attacked than the sulphates. The carbonates of sodium, lithium, calcium, and lead are decomposed at ordinary temp, with incandescence, but potassium carbonate is not decomposed even at a dull red heat. Fluorine does not act on sodium bofate. Most of these reactions have been qualitatively studied by H. Moissan,15 and described in his monograph, Lefluor et ses composes (Paris, 1900). 

The sulphate of lime, in contact with incandescent charcoal, yields its oxygen to the latter element, and carbonic oxide, or a mixture of this and carbonic acid is evolved, leaving protosulphide of calcium in admixture with the carbonate of soda previously prodaced,... 

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